CHEMISTRY COMMUNITY

JamieVu_2C

Referring to homework 7D.1 as an example, the problem gives you 2 rate constants at 2 different temperatures and asks you to find the activation energy. In this case, you would rearrange the Arrhenius equation as a difference of T1 and T2 to get ln\frac{k_{2}}{k_{1}} = \frac{E_{a}}{R}(\frac{1}{T...

JamieVu_2C

Usually, the problem should tell you whether the elementary step is slow or fast. So, the problem will tell you that there are elementary steps, and then to find the overall reaction you would add the steps together. The slow step is the rate-determining step, so you would use its rate law.

JamieVu_2C

Since these are elementary reactions, you can write the rate law using the coefficients. For part a, since there are 2 NO molecules on the reactant side, the rate = k[NO]^2, and it is bimolecular. For part b, there is only 1 Cl2 molecule, so the rate = k[Cl2], and it is unimolecular.

JamieVu_2C

The Nernst equation is E = E(standard) - (RT/nF)lnQ. Since R = 8.314 J * K^-1 * mol^-1, it will cancel out with the units for T, temperature, at Kelvin. the mol in R will also cancel with the mol for Faraday's constant, which is C/mol. Then, what you end with for the units of (RT/nF) is J/C, which e...

JamieVu_2C

The units for k will depend on the overall order of the reaction. k has the units of L^2 * mol^-2 * s^-1 when the overall order is 3.

JamieVu_2C

I think the rate of decomposition relates to the rate of formation in that they are conveyed by the same rate law. For part a, the reaction is NO + NO --> N2O2. The rate law is rate = k[NO]^2. For the decomposition of NO, the rate law is k[NO]^2, and for the rate of formation of N2O2, the rate law i...

JamieVu_2C

ClO- + H2O \rightleftharpoons HClO + OH- (fast equilibrium) HClO + I- --> HIO + Cl- (very slow) HIO + OH- \rightleftharpoons +H2O (fast equilibrium) (b) Write the rate law based on this mechanism. Since step 2 is slow, the rate law is rate = k2[HClO][I-]. Then, the solutions manual shows that you sh...

JamieVu_2C

The rate law of the reaction 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) is rate = k[NO]^2[H2], and the mechanism that has been proposed is Step 1: NO + NO --> N2O2 Step 2: N2O2 + H2 --> N2O + H2O Step 3: N2O + H2 --> N2 + H2O (a) Which step in the mechanism is likely to be rate determining? Explain your an...

JamieVu_2C

The hydrolysis of an organic nitrile, a compound containing a –CN group, in basic solution, is proposed to proceed by the following mechanism. Write a complete balanced equation for the overall reaction, list any intermediates, and identify the catalyst in this reaction. Step 1: RCN + OH- --> RCNOH ...

JamieVu_2C

The presence of a catalyst provides a reaction pathway in which the activation energy of a certain reaction is reduced from 125 kJ/mol to 75 kJ/mol. (a) By what factor does the rate of the reaction increase at 298 K, all other factors being equal? (b) By what factor would the rate change if the reac...

JamieVu_2C

For some problems where you have to calculate the cell potential using the Nernst equation, the solutions manual substitutes concentrations for aqueous species and partial pressures for gases into Q for lnQ. Don't you have to convert the units so that the species in Q are uniformly either in M or at...

JamieVu_2C

(a) Write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride. (b) Write the balanced equation for the cell reaction and devise a galvanic cell to study the reaction (write its cell diagram). The half reactions are: anode: MnO_{4}^{...

JamieVu_2C

(a) Calculate the reaction Gibbs free energy of I2(g) -->2I(g) at 1200. K (K = 6.8) when the partial pressures of I2 and I are 0.13 bar and 0.98 bar, respectively. (b) Indicate whether this reaction mixture is likely to form reactants, is likely to form products, or is at equilibrium. In the solutio...

JamieVu_2C

Suppose that each of the following pairs of redox couples is combined to form a galvanic cell that generates a current under standard conditions. Identify the oxidizing agent and the reducing agent, write a cell diagram, and calculate the standard cell potential from the standard potentials of the e...

JamieVu_2C

A student was given a standard Cu(s)|Cu2+(aq) half-cell and another half-cell containing an unknown metal M in 1.00M M(NO3)2(aq) and formed the cell M(s)|M+(aq)||Cu2+(aq)|Cu(s). The cell potential was found to be -0.689 V. What is the value of E(M2+/M)? In this problem, since Cu2+(aq)/Cu(s) is writ...

JamieVu_2C

For the cell diagram for the reaction $Ce^{4+}(aq)+I^{-}(aq)\rightarrow I_{2}(s)+Ce^{3+}(aq)$ , how do you know that Platinum is included in the cell diagram on both the anode and cathode sides of the diagram?

JamieVu_2C

Write the half-reactions and the balanced equation for the cell reaction for each of the following galvanic cells: (d) Pt(s) | O2 (g) | H+ (aq) || OH- (aq) | O2 (g) | Pt (s) For the oxidation half reaction for the anode, how do you know that O2 (g) and H+ (g) are the reactants and that H2O is the pr...

JamieVu_2C

How do you know that O3 is being reduced in the reaction of O3(aq) --> O2(g) when both O3 and O2 have an oxidation state of 0 since they're both molecules?

JamieVu_2C

How would you write the reaction equation from the given cell diagram? For example, how would you write the reaction for
Zn(s)| $Zn^{2+}$ (aq)|| $Cu^{2+}$ (aq)|Cu(s)?

JamieVu_2C

A galvanic cell is an electrochemical cell that generates an electrical current from a spontaneous reaction. In other words, if the free energy (delta G) of the reaction is negative, then the reaction proceeds in the forward direction.

JamieVu_2C

When you're relating free energy to the cell potential, as given by \Delta G=-nFE_{cell} , the cell potential (E) comes from the galvanic cell. So, you'd need to calculate the cell potential from the galvanic cell and its two electrodes – the anode and the cathode. Using the two electrodes, you can ...

JamieVu_2C

Calculate the equilibrium constant at 25.00 degreesC for the reaction AgCl(s)\rightarrow Ag^{+}(aq)+Cl^{-}(aq) . The equilibrium constant for this reaction is actually the solubility product, Ksp = [Ag+][Cl-], for silver chloride. The two reduction half reactions are R: AgCl&...

JamieVu_2C

Write the reaction for the cell Pt(s)|H2(g)|HCl(aq)|Hg2Cl2(s)|Hg(l). The textbook example shows that the reduction half reaction is Hg_{2}Cl_{2}(s)+2e^{-}\rightarrow 2Hg(l)+2Cl^{-}(aq) and that the oxidation half reaction is H_{2}(g)\rightarrow 2H^{+}(aq)+2e^{...

JamieVu_2C

You have multiple equations for finding the change in entropy. One is \Delta S=\frac{q}{T} . You use this equation when the temperature is constant. The other equation is \Delta S=nCln\frac{T_{2}}{T_{1}} . This equation is used when you have a final temperature that is different from the initial tem...

JamieVu_2C

What is the significance of the Van't Hoff equation? It connects thermodynamics with the equilibrium constant, but is it supposed to tell us anything about a reaction?

JamieVu_2C

Calculate the standard entropy of vaporization of water at 85 degreesC, given that its standard entropy of vaporization at 100. degreesC is 109.0 J/K*mol and the molar heat capacities at constant pressure of liquid water and water vapor are 75.3 J/K*mol and 33.6 J/K*mol, respectively, in this range....

JamieVu_2C

A technician carries out the reaction 2SO_{2}(g) + O_{2}(g) \rightarrow 2SO_{3}(g) at 25^{o}C and 1.00 atm in a cylinder fitted with a piston and maintained at constant pressure. Initially, 0.030 mol SO_{2} and 0.030 mol O_{2} are present in the cylinder. The technician then ...

JamieVu_2C

In 1750, Joseph Black performed an experiment that eventually led to the discovery of enthalpies of fusion. He placed two samples of water, each of mass 150. g, at 0.00 degreesC (one ice and one liquid) in a room kept at a constant temperature of 5.00 degreesC. He then observed how long it took for ...

JamieVu_2C

Is there a way to figure out the bonds that are being formed and broken without having to draw the structure of the molecule? For example, in the reaction of CH_{3}CHCH_{2}(g) + H_{2}O(g) \rightarrow CH_{3}CH(OH)CH_{3}(g) , would there be a way to figure out the bonds...

JamieVu_2C

In the textbook solutions, for some answers $\Delta H^{o}$ has the units of kJ and for other answers it has the units of kJ/mol. Are kJ and kJ/mol interchangeable as the units for the standard reaction enthalpy?

JamieVu_2C

An ice cube of mass 50.0 g at 0.0 degreesC is added to a glass containing 400.0 g of water at 45.0 degreesC. What is the final temperature of the system (see Tables 4A.2 and 4C.1)? Assume that no heat is lost to the surroundings. I know that you use the equation q(ice) = -q(water) since the heat los...

JamieVu_2C

(a) Calculate the heat that must be supplied to a copper kettle of mass 500.0 g containing 400.0 g of water to raise its temperature from 22.0 degrees C to the boiling point of water, 100.0 degrees C. Why do you need to find the heat (q) for copper and the heat (q) for water and add them together? W...

JamieVu_2C

Calculate the final temperature and the change in enthalpy when 765 J of energy is transferred as heat to 0.820 mol Kr(g) at 298 K and 1.00 atm (a) at constant pressure; (b) at constant volume. Treat the gas as ideal. For part b, \Delta U = q, which is 765 J. Then, you use \Delta U to find \Delta H,...

JamieVu_2C

In a combustion chamber, the total internal energy change produced from the burning of a fuel is -2573 kJ. The cooling system that surrounds the chamber absorbs 947 kJ as heat. How much work can be done by the fuel in the chamber? In the solutions manual, it says that q = –947 kJ. How is q negative ...

JamieVu_2C

An ideal gas in a cylinder was placed in a heater and gained 5.50 kJ of energy as heat. If the cylinder increased in volume from 345 mL to 1846 mL against an atmospheric pressure of 750. Torr during this process, what is the change in internal energy of the gas in the cylinder? With the equation \De...

JamieVu_2C

A constant-volume calorimeter was calibrated by carrying out a reaction known to release 3.50 kJ of heat in 0.200 L of solution in the calorimeter (q = -3.50 kJ), resulting in a temperature rise of 7.32 degrees C. In a subsequent experiment, 100.0 mL of 0.200 M HBr(aq) and 100.0 mL of 0.200 M KOH(aq...

JamieVu_2C

\Delta A piece of copper of mass 20.0 g at 100.0 C is placed in a vessel of negligible heat capacity but containing 50.7 g of water at 22.0 C. Calculate the final temperature of the water. Assume that no energy is lost to the surroundings. In the solutions manual, the equation to solve for the fina...

JamieVu_2C

Since enthalpy is a state property, only its present state is taken into account. Thus, the paths taken to reach that present state do not matter, since only the current state matters. However, the intermediary states are still taken into account, for example with phase changes, or with the bond ent...

JamieVu_2C

The Lewis structures were drawn to just give a better idea of the bonds that would be broken and formed in the reaction. However, we won't have to draw the Lewis structures, but they do give a better idea of the structures and bonds of each molecules so that we know the bond enthalpies for each bond.

JamieVu_2C

Why is work not a state property when work is force times distance? Since the path doesn't matter for a state property, why would work not be considered a state property?

JamieVu_2C

Steam burns are more severe due to the enthalpy of vaporization. At 100 degrees Celsius, water changes from a liquid to gas, and additional energy is needed for the change. However, despite the additional energy, the temperature is the same at 100 degrees Celsius, so both liquid and gaseous water ca...

JamieVu_2C

The method using bond enthalpies is the least accurate since for many different molecules – that are not diatomic– the bond enthalpies are averages.

JamieVu_2C

Calculate the pH of 0.15 M H2SO4(aq) at 25 degrees C. For polyprotic acids, I thought you only needed to calculate the first Ka value and consider the other deprotonations as insignificant. However, the solutions manual shows that the first ionization is complete but the second one isn't, so you cal...

JamieVu_2C

The lower the pKa or pKb, the stronger is the acid or the base.

JamieVu_2C

[H3O+][OH-] = 10^-14 For this equation if the concentration of H3O+ is large, then the concentration of OH- must be low since their product is always a constant at 10^-14, and vice versa. pKa + pKb = pKw Similarly, if pKa is large, then pKb is low since their sum always equals pKw, which is 14, and ...

JamieVu_2C

(a) When the pH of 0.10 M HClO2(aq) was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid? To find [H3O+], you take the antilog of the pH, and [H3O+] also equals [ClO2-]. For the Ka equation, Ka = [H3O+][ClO2-]/[HClO2]. How do you know that [HClO2] = (.10 - .06) wh...

JamieVu_2C

A student added solid Na2O to a volumetric flask of volume 200.0 mL, which was then filled with water, resulting in 200.0mL of NaOH solution. Then 5.00 mL of the solution was transferred to another volumetric flask and diluted to 500.0 mL. The pH of the diluted solution is 13.25. (b) What mass of Na...

JamieVu_2C

The value of Kw for water at body temperature (37 C) is 2.1 x 10^-14. (a) What is the molar concentration of H3O+ ions at 37 degrees C? (b) What is the molar concentration of OH- in neutral water at 37 degrees C? For part a, the solutions manual shows that you use the expression Kw=[H3O+][OH-] and s...

JamieVu_2C

I know that the quick way to explain the changes in pressure is that if the volume decreases and there are more moles of gas on the left, then the reaction proceeds to the right and vice versa. But why is this the short way? If you know that the volume decreases, then you also know that there is sti...

JamieVu_2C

Since the K value at 700K is smaller, it means that more reactants are formed since K = Products/Reactants. Since there are more reactants, it means that at 700K, there will be less products and so less ammonia will be present at the higher temperature of 700K.

JamieVu_2C

The overall photosynthesis reaction is 6CO2(g) + 6H2O(l) \rightarrow C6H12O6(aq) + 6O2(g), and \Delta H = +2802 kJ. Suppose that the reaction is at equilibrium. State the effect that each of the following changes will have on the equilibrium composition: tends to shift toward the formation of reacta...

JamieVu_2C

.001 M is the initial concentration of F2 before equilibrium is reached, but at equilibrium, the concentration of F2 is 8.3 x 10^-4M. Cl2 is more stable because its K value, the equilibrium constant, is smaller. This means that at equilibrium there are more reactants than products, so there is more ...

JamieVu_2C

For the reaction H2(g) + I2(g) \rightleftharpoons 2 HI(g), K=160. at 500. K. An analysis of a reaction mixture at 500. K showed that it had the composition PH2 = 0.20 bar, PI2 = 0.10 bar, and PHI = 0.10 bar. (a) Calculate the reaction quotient. (b) Is the reaction mixture at equilibrium? (c) If not,...

JamieVu_2C

How does Mg2+ have a larger radius than F- when F- has a greater effective nuclear charge since it is further to the right on the periodic table and when Mg2+ is in a higher energy shell?

JamieVu_2C

Why don't you include the doubly bonded oxygen atoms when counting the sites where EDTA can bind to a transition metal? So, instead of 6 attachment sites, why can't there be 10, with the 4 included double bonded oxygen atoms?

JamieVu_2C

Which of the following ligands can be polydentate? If the ligand can be polydentate, give the maximum number of places on the ligand that can bind simultaneously to a single metal center: (b) (CO3)2- (d) oxalate For (CO3)2-, all the 3 oxygen atoms have lone pairs, so why is the maximum number for th...

JamieVu_2C

(d) Write the formula for: sodium bisoxalato(diaqua)ferrate(III)

Why is the formula Na[Fe(OH2)2(C2O4)2] instead of Na[Fe(C2O4)2(OH2)2]? If the ligands are written in alphabetical order, why does (OH2)2 go in front of (C2O4)2 in the formula?

JamieVu_2C

Can we use the new IUPAC name conventions for naming coordination compounds as used in the examples in the textbook, or do we have to go with the version given on the chart on Dr. Lavelle's website?

JamieVu_2C

Why is the melting point of xenon higher than that of argon?

JamieVu_2C

Draw the Lewis structure of boric acid, B(OH)3. (a) Is resonance important for its description? (b) The proton transfer equilibrium for boric acid is given in a footnote to Table 6C.1. In that reaction does boric acid act as a Lewis acid, a Lewis base, or neither? Justify your answer by using Lewis ...

JamieVu_2C

What are the differences between the Bronsted, Lewis, and Arrhenius definitions of acids and bases? How does each definition make identifying acids and bases different?

JamieVu_2C

How do you know if a molecule accepts H+ from H2O or donates H+ to H2O without looking at a table? For example, the question asks to Write the chemical equations for the proton transfer equilibria of the following acids in aqueous solution and identify the conjugate acid–base pairs in each case: (d)...

JamieVu_2C

Identify the salt that is produced from the acid–base neutralization reaction between (b) ammonia and phosphoric acid. I know that phosphoric acid is a triprotic acid, from its formula H3PO4. The first equation for the reaction between ammonia and phosphoric acid is: NH3 + H3PO4 -> NH4H2PO4. How do ...

JamieVu_2C

Identify each compound as either a Brønsted acid or a Brønsted base: (a) NH3 ; (b) HBr; (c) KOH; (d) H2SO3 ; (e) Ca(OH)2 .

Is there a strategy for identifying each compound as a Bronsted acid/base?

JamieVu_2C

Which of the following ligands can be polydentate? If the ligand can be polydentate, give the maximum number of places on the ligand that can bind simultaneously to a single metal center: (a) HN(CH2CH2NH2)2; (b) (CO3)2-; (c) H2O; (d) oxalate. How do you determine if the ligands are polydentate? And ...

JamieVu_2C

When a molecule is drawn as a ring structure, are there still lone pairs on the atoms if they don't form octets and even if we can't see it? And we'd still include them in the hybridization?

JamieVu_2C

How does H2SeO4 have a dipole-dipole moment when the oxygen atoms are arranged around Se, with 2 H atoms attached to 2 of the O atoms? Don't the dipole moments cancel out for each oxygen?

JamieVu_2C

How is NH2OH polar?

JamieVu_2C

How do the states of the molecules (solid, liquid, gas) relate to intermolecular forces? Do solids have stronger intermolecular forces?

JamieVu_2C

Explain the trend in the boiling points of the hydrogen halides: HCl, -85 degrees Celsius; HBr, -67 degrees Celsius; HI, -5 degrees celsius. How would the boiling points depend on the forces of these molecules?

JamieVu_2C

Noting that the bond angle of an sp3 hybridized atom is 109.5 degrees and that of an sp2 hybridized atom is 120 degrees, do you expect the bond angle between two hybrid orbitals to increase or decrease as the s-character of the hybrids is increased? Can someone explain this to me? I don't understand...

JamieVu_2C

For part A, if you weren't given the information that C5H5N, pyridine, has a similar structure to benzene, how would you know to draw it as a ring structure?

JamieVu_2C

How are CH2Cl2 and SF4 polar when their dipole moments cancel in their Lewis structures?

JamieVu_2C

When drawing the Lewis structure for (S2O3)2-, does it matter which Lewis structure I draw? One structure consists of the central S atom with 3 double bonds attached to O and one single bond attached to S. The other structure is 2 double bonds between the central S atom and 2 O atoms, and 1 single b...

JamieVu_2C

For part b, the book solutions manual states that TeCl4 has a seesaw molecular shape, but its bond angles are 90 degrees and 120 degrees. If Te has a lone pair on an equatorial position in its seesaw structure, why do the bond angles equal 90 degrees and 120 degrees? Shouldn't they be slightly less ...

JamieVu_2C

For I3-, the shape is linear with 3 lone pairs around the central I atom. Why does the bond angle equal 180 degrees instead of being slightly below 180 degrees when there are 3 lone pairs of electrons around the central I atom? Wouldn't those lone pairs slightly push down on the bond angles?

JamieVu_2C

How is XeF2 polar when it has 3 lone pairs? How do the dipole moments cancel when there are two lone pairs above Xe and one lone pair below Xe?

JamieVu_2C

Yes, the d-subshell and f-subshell allows electrons to occupy more orbitals, therefore expanding its octet.

JamieVu_2C

Electronegativity is the ability of an atom to attract shared electrons toward itself. Electronegativity generally decreases down a group because there is more distance between the nucleus and the outer valence shell and increases across a period because the charge on the nucleus increases due to th...

JamieVu_2C

Can somebody please explain to me how we would use this equation? The example in the textbook makes sense but when I go to actually apply it it does not make sense at all. Like they'll give us the weight in grams but I'm not sure how that's relevant. Thank you! The equation is (delta p)(delta x) >/=...

JamieVu_2C

How do you know if a molecule is polar? Do you always have to draw it out to see if it's polar or not?

JamieVu_2C

If you're forming an ion from an atom that has its d-orbitals filled, then are the d-orbitals still considered valence electrons? For example, the electron configuration of Ga is [Ar] 3d^10 4s^2 4p^1. But if you want to form the Ga ion, you would only remove the electrons in the 4s and 4p orbitals t...

JamieVu_2C

Why is the electronic configuration for tungsten [Xe]4f^14 5d^4 6s^2? I thought that the d-subshell wants to have half-filled orbitals, so that the electronic configuration would be [Xe]4f^14 5d^5 6s^1.

JamieVu_2C

Are resonance structures only the Lewis structures by which you can move the double triple bonds? Or do they include all the structures that you can draw for a molecule? For example, with N2O, you can draw different structures with single, double, or triple bonds, so would all those structures be co...

JamieVu_2C

Suggest, giving reasons, which substance in each of the following pairs is likely to have the higher normal melting point
(Lewis structures may help your arguments):
(c) CHI3 or CHF3.

How does CHI3 have a higher melting point than CHF3 when CHF3 is more polar due to the F atom?

JamieVu_2C

When drawing Lewis structures, are you supposed to always draw the different resonance structures and find the formal charges? For example, for 2B. 11C, when drawing H2C(NH2)COOH, if my structure is different from the solution structure, would it be wrong? Or would I have to find the formal charges ...

JamieVu_2C

The problem asks you to draw the Lewis structure for ONF. So, the structure has N as the central atom, with a double bond between O and N and a single bond between N and F. But why can't you put the double bond between N and F and the single bond between O and N?

JamieVu_2C

A resonance hybrid is a blending of the Lewis structures for a molecule. For example, with the nitrate ion, you have 3 possible Lewis structures where the double bonds are in different positions. However, instead of only having one structure represent the nitrate ion (NO3-), it's better to have a re...

JamieVu_2C

What is the difference between drawing Lewis structures for an ionic vs covalent compound? Is it only adding or subtracting the electrons for a cation or anion, respectively?

JamieVu_2C

In a polyatomic atom, how would you know which atoms are the central atoms if there are multiple of them that could act as the central atoms? So an example in the book is CH3COOH, but how would you know how to make which atoms the central ones?

JamieVu_2C

Can someone please explain the concept of ionization? How do you know that ionization energy is based off the period table? Ionization energy is the energy required to remove an electron from the atom of a gas. The ionization energy is based off the periodic table because as you go from left to righ...

JamieVu_2C

Benzene's usual structure is a 6-carbon ring structure with 3 double bonds. It can also be written as a line structure. But what's special about benzene is that, according to the textbook, the line structure doesn't fit its experimental evidence. For instance, the C-C bonds in benzene are the same l...

JamieVu_2C

Which of the following increase when an electron in a lithium atom undergoes a transition from the 1s-orbital to a 2p-orbital? (a) Energy of the electron. (b) Value of n. (c) Value of l. (d) Radius of the atom. Which answers would be different for a hydrogen atom and in what way would they be differ...

JamieVu_2C

Hund's rule basically states that for a subshell with multiple orbitals, then you fill each orbital with one electron first before you fill a single orbital with two electrons. So for example, when you're filling in the p-orbitals, you fill up the px-, py-, and pz-orbitals with one electron each bef...

JamieVu_2C

In the book, it says "Argon completes the third period. From Fig. 1E.1, you can see that the energy of the 4s-orbital is slightly lower than that of the 3d-orbitals. As a result, instead of electrons entering the 3d-orbitals, the fourth period now begins by filling the 4s-orbitals..." How ...

JamieVu_2C

So for c, would that mean there is only one orbital for the given quantum numbers?

JamieVu_2C

How many orbitals can have the following quantum numbers in an atom:
(a) n=2, l=1
(b) n=4, l=2, ml= -2
(c) n=2
(d) n=3, l=2, ml= +1?

For (b) and (c), how does the magnetic quantum number tell you how many orbitals there are? I don't understand how to find the number of orbitals with ml.

JamieVu_2C

The velocity of an electron that is emitted from a metallic surface by a photon is 3.63 x 10^3 km/s. (a) What is the wavelength of the ejected electron? (b) No electrons are emitted from the surface of the metal until the frequency of the radiation reaches 2.50 x 10^16 Hz. How much energy is require...

JamieVu_2C

Constructive interference refers to waves in phase. This means that the peak of one wave interacts with the peak of another, and the trough of one wave interacts with the trough of another. Thus, the resulting wave is larger in the sense that the trough is deeper and the peak is higher. Destructive ...

JamieVu_2C

The answer is photoelectric effect. Light is used to eject electrons from a metal, and if light acted as a wave, then increasing the intensity of the light would mean more electrons being ejected. However, this didn't work. Instead, decreasing the wavelength allowed the ejection of electrons, which ...

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