CHEMISTRY COMMUNITY

Minahil_Tufail_3I

Of course! So, I looked it up to double check and the general idea of an amine group is that it contains a nitrogen atom with a lone pair of electrons. So for (CH3)3N, it is known as a tertiary amine group, but I highly doubt you'd have to know the specifics of that! Another easy way to figure out w...

Minahil_Tufail_3I

Hi! For 9, I believe you're correct as to why (NO3)2 isn't included. As for 17, the question is just asking about how much maximum work can be reached, and since we know that delta G = wmax, you only have to use the delta G = -nfE equation. I'm not entirely sure about 21, but I think the question wa...

Minahil_Tufail_3I

Hi! For NH2NH2, you can determine it's a base because it has NH2 which is an amine group. Amines often signal that the compound is a base. For weak acids, look to see if it has COOH, otherwise known as a carboxyl group, as this indicates acidity.

Minahil_Tufail_3I

Yes, I think you can look at it that way too! Another way to understand the explanation is by looking at how K = k1/k'1. Since k1 is increasing more than k'1, it would cause K to overall increase.

Minahil_Tufail_3I

Hi! Electromotive force describes the difference in potential as a result of an electric current and can be represented by E = w / q. E represents maximum potential difference when there is very little/no electrons flowing right before the reaction occurs.

Minahil_Tufail_3I

Hi, I think that using bar is okay but if it's Torr, you should convert it into atm.

Minahil_Tufail_3I

To start off this problem, you basically are trying to determine the orders of the concentrations for A, B, and C. So, using the table, we can see that when A and B have the same concentration (they are unchanged) in steps 1 and 4, the concentration of C increases. However even though the initial co...

Minahil_Tufail_3I

Kc just refers specifically to the equilibrium constant for molar concentrations. K is the equilibrium constant, and sometimes it's specified as Kp with equilibrium constant using partial pressures.

Minahil_Tufail_3I

Hi! So since the intermediate cancels out, you don't include it in the rate law, but you use the first step reaction in order to solve for HCIO. Through solving for HCIO, you would input that equation into the rate law instead. So, you would get [HCIO] = [CIO-][H2O]/[OH-]. However, since H2O is a so...

Minahil_Tufail_3I

Hi, could someone explain how they solved this problem? I'm confused on how you solve for the activation energies in order to find the rate constants. The presence of a catalyst provides a reaction pathway in which the activation energy of a certain reaction is reduced from 125 kJ ⋅ mol − 1 to 75 kJ...

Minahil_Tufail_3I

Hi, I was wondering if someone could explain part b for this problem to me? For the reversible, one-step reaction A + A ⇄ B + C, the forward rate constant for the formation of B is 265 L ⋅ mol − 1 ⋅ min − 1 and the rate constant for the reverse reaction is 392 L ⋅ mol − 1 ⋅ min − 1 . The activation ...

Minahil_Tufail_3I

Hi, could someone explain how they solved this problem: Evaluate the unknown quantity in each of the following cells: (a) Pt(s)|H 2 (g, 1 .0 bar)|H + (pH = ?)||Cl − (aq, 1 .0 mol ⋅ L − 1 )|Hg 2 Cl 2 (s)|Hg(l), E cell = +0 .33 V. I understand how to set up the initial equation 0.33 V = +0.27 V - (0.0...

Minahil_Tufail_3I

Hi, how do you decide which is the anode and which is that cathode for La^3+ --> La and U^3+ --> U? Since both charges are being reduced, I'm not sure how to determine which is the anode.

Minahil_Tufail_3I

Hi, could someone explain how they did this problem? It asks for the half-reactions, balanced reactions, and the cell diagram for (d) Au+ (aq) → Au(s) + Au^3+ (aq). I'm confused on why the anode reaction is supposed to be Au (s) --> Au^3+ (aq) + 3e- when Au (s) is also a product. Thank you!

Minahil_Tufail_3I

Hi, is it an error in the book where it says Cl2(g) in the product? The solution manuals refers to it as Cl(aq) so I wasn't sure.

Minahil_Tufail_3I

Hi, could someone go through how they found the oxidation number for C in C2H5OH? I'm having trouble figuring out how it oxidized from -2 to -1. Thank you!

Minahil_Tufail_3I

Hi! I think the reason that you have to divide everything by 2 is because the question asks for the standard entropy change for 1.00 mol of H20. The answer that you found would technically be the entropy change for the reaction but for 2 mols of H20. If you divide that result by 2, you should get th...

Minahil_Tufail_3I

For this problem, I looked at the images of each molecule that the textbook provided. For the cis molecule, you can see that the two red atoms are side-by-side whereas for the trans molecule, the two red atoms are on opposite ends of each other. This makes sense given that cis indicates that identic...

Minahil_Tufail_3I

Hi! I believe the reason we have to do n*∆Hfusion + mc∆T is because ∆Hfusion is referring to the change of ice melting into a liquid. At fusion, the temperature remains constant because all the heat is being used to break apart the solid and turn it into a liquid. Therefore once you've obtained the ...

Minahil_Tufail_3I

For these two questions, they are asking for us to find the equilibrium constant. However for 5G.21, you only have to find deltaG for the reaction then plug it into the equation of ln K = -deltaG/RT. As for 5J.15, you're supposed to first solve for delta H and delta S for the reaction then use those...

Minahil_Tufail_3I

Hi! For part a in 7, the reaction is written as 2H2O2(l) --> 2H2O (l) + O2 (g). The textbook writes the H2O's as aqueous in the solutions manual when solving for change in enthalpy and change in Gibbs free energy. Is this just an error in the book?

Minahil_Tufail_3I

Hi, while calculating the values for ΔS° in this problem, I came across negative values for the difference. For example, for part a, I got that ΔS°f= -99.38 J.K^-1mol^-1. I was wondering how to interpret the negative value? The textbook solutions manual said that it is a negative value because it ta...

Minahil_Tufail_3I

Hi, could someone explain why for an ideal gas freely expanding irreversibly and isothermally, the change of internal energy is equal to 0? I understand that w=0, but I don't understand why delta U = 0 and therefore q=0. Thank you!

Minahil_Tufail_3I

Hi! Could someone explain how to go about solving this problem?
Suppose that 50.0 g of water at 20.0 °C is mixed with 65.0 g of water at 50.0 °C at constant atmospheric pressure in a thermally insulated vessel. Calculate Δ S and Δ S tot for the process.

Minahil_Tufail_3I

For this problem, why do we multiply 1 mol of H20 by -6.01 for part a?
Use data in Table 4C.1 or Appendix 2A to calculate the entropy change for (a) the freezing of 1.00 mol H 2 O (l ) at 0.00 ° C

Minahil_Tufail_3I

Hi, could someone explain how to solve this problem? Thanks! The enthalpy of formation of trinitrotoluene (TNT) is − 67 kJ ⋅ mol − 1 , and the density of TNT is 1.65 g ⋅ cm − 3 . In principle, it could be used as a rocket fuel, with the gases resulting from its decomposition streaming out of the roc...

Minahil_Tufail_3I

Hi, I was wondering if someone could help me understand how to solve this problem? 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 idea...

Minahil_Tufail_3I

When solving for C, the textbook manual showed that it would be 3.50/7.32. Why is q a positive value when it is written as a negative one within the problem? Here's the problem for context: A constant-volume calorimeter was calibrated by carrying out a reaction known to release 3.50 kJ of heat in 0....

Minahil_Tufail_3I

Hi, how do you solve this? A piston confines 0.200 mol Ne (g ) in 1.20 L at 25 °C. Two experiments are performed. (a) The gas is allowed to expand through an additional 1.20 L against a constant pressure of 1.00 atm. (b) The gas is allowed to expand reversibly and isothermally to the same final volu...

Minahil_Tufail_3I

Hi! 6E.1 covers polyprotic acid solutions which includes carbonic acid. 6E.3 part a also has a question involving carbonic acid if you wanted to try calculating pH for it!

Minahil_Tufail_3I

For part a, all you would have to do is take the negative log of 0.025 to find the pH of the desired solution. For part b, you would take -log(200 mL*0.025M/250 mL). This would be the actual pH. You can also think of it like M1V1=M2V2! In this case, M1 = 0.0025 M, V1 = 200 mL, and V2 = 250 mL. So, y...

Minahil_Tufail_3I

What I did first was convert the moles of H2 and I2 into molarity. After that, I created an ICE table. Because the problem tells us that 60% of hydrogen has been used, it basically means that there is only 40% of hydrogen left. In other words, the 40% of hydrogen left is the equilibrium concentratio...

Minahil_Tufail_3I

For the second part, you first convert the grams into moles using the molar mass of carbon. Then, after finding the moles, you multiply it by (358.8 Kj/4 mol) since there are 4 moles of C. For the third part, you set up the equation: deltaH = n(CS2) * (358.8kJ/4mol). In other words, this is saying t...

Minahil_Tufail_3I

Hi, can someone go through how to solve part b for this problem? Thank you! Water gas is an inexpensive, low-grade fuel that can be made from coal. (a) Is the production of water gas exothermic or endothermic? The reaction is C (s ) + H 2 O (g ) → CO (g ) + H 2 (g ) (b) Calculate the enthalpy change...

Minahil_Tufail_3I

Do we take into account the bonds between C-H in this problem when calculating reaction enthalpy?
Use the bond enthalpies in Tables 4E.2 and 4E.3 to estimate the reaction enthalpy for (a) 3C2H2 (g ) → C6H6 (g).

Minahil_Tufail_3I

Hi! For the other polyprotic acids, I think when Ka2 is less than Ka1/1000 then it does not affect the pH significantly.

Minahil_Tufail_3I

Hi, I was wondering if someone could explain how they solved this problem?
Thank you!

Minahil_Tufail_3I

Hi, could someone go through how you would solve this problem: Determine the reaction enthalpy for the hydrogenation of ethyne to ethane, C2H2 (g ) + 2 H2 (g ) → C2H6 (g ), from the following data: ΔHc ° ( C2H2, g ) = − 1300. kJ ⋅ mol − 1 , ΔHc ° ( C2H6 , g ) = − 1560. kJ⋅mol − 1 , ΔHc° ( H2 , g ) =...

Minahil_Tufail_3I

For this problem, how do you find the Ka value for AlCl3?
Calculate the pH of (b) 0 .055 M AlCl3.

Minahil_Tufail_3I

Hi, how do you solve this problem?
The percentage deprotonation of benzoic acid in a 0.110 M solution is 2.4%. What is the pH of the solution and the K a of benzoic acid?
Thank you in advance!

Minahil_Tufail_3I

Hi, I was wondering if someone could explain how to solve this problem: A student added solid Na 2 O to a volumetric flask of volume 200.0 mL, which was then filled with water, resulting in 200.0 mL of NaOH solution. Then 5.00 mL of the solution was transferred to another volumetric flask and dilute...

Minahil_Tufail_3I

Yes, I believe partial pressure only applies to gases!

Minahil_Tufail_3I

For this question, are we assuming that the values of OH- and H30+ concentration are equal: The value of K w for water at body temperature (37 °C) is 2 .1 × 10 − 14 . (a) What is the molar concentration of H 3 O + ions at 37 °C? (b) What is the molar concentration of OH − in neutral water at 37 °C?

Minahil_Tufail_3I

Hi! So, for this problem on one of the earlier parts, I calculated the equilibrium constant to be 11.24. For finding the new concentrations, I first set up an ICE table. For the initial concentration of N2O4, I put 0.483, and for NO2, I put 3.33. For the change in concentrations, I had +x under N204...

Minahil_Tufail_3I

What I did for this problem was first calculate the equilibrium constant through the given constants. Therefore, K = (0.400)^2/(0.300)(0.300). As a result, I got 1.778 for the constant. Then, when the concentration of NO is increased to 0.700, I set up an ICE table. Under N2 and 02, I wrote the init...

Minahil_Tufail_3I

Hi, how would you go about finding the chemical equation for this problem: The following plot shows how the partial pressures of reactant and products vary with time for the decomposition of compound A into compounds B and C. All three compounds are gases. Use this plot to do the following: (a) Writ...

Minahil_Tufail_3I

Hi, how would you go about solving this problem? A sample of ammonium carbamate, NH 4 ( NH 2 CO 2 ) , of mass 25.0 g was placed in an evacuated flask of volume 0.250 L and kept at 25 °C. At equilibrium, 17.4 mg of CO 2 was present. What is the value of K c for the decomposition of ammonium carbamate...

Minahil_Tufail_3I

Hi, I was wondering if someone could explain to me the answer for this part of the question : Use your results from parts (a) and (b) to determine which is thermodynamically more stable relative to its atoms at 1000. K, Cl 2 or F 2 . I'm a bit confused on how you determine which is more stable. Than...

Minahil_Tufail_3I

Hi, how do you solve the value of K for (b) 1/2N2 (g ) + 3/2H2 (g ) ⇌ NH3 (g ) if the original equation is N2 ( g ) + 3H2 ( g ) ⇌ 2NH3 ( g ) at 400. K with K = 41?

Minahil_Tufail_3I

Hi, I'm a bit confused on the answer for part C in this problem: A sample of ozone, O3 , amounting to 0.10 mol, is placed in a sealed container of volume 1.0 L and the reaction 2 O3 (g ) → 3 02 (g ) is allowed to reach equilibrium. Then 0.50 mol O3 is placed in a second container of volume 1.0 L at ...

Minahil_Tufail_3I

Hi, I was wondering if someone could help me with this problem: If the initial amounts of CO and H2O were both 0.100 M, what will be the amounts of each reactant and product at equilibrium for the following reaction? Keq = 23.2 at 600K CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g) When I plug in the numbers i...

Minahil_Tufail_3I

Hi! For this problem, it asks you to decide whether the pH is greater than, equal to, or less than 7 for the aqueous solutions of the salts. I know that AlCl3 will lower the acidity of the solution because of the Al cation being highly charged and small, but I was having trouble figuring out how to ...

Minahil_Tufail_3I

Hi, this question asked whether HBrO2 or HClO2 is the stronger acid. I initially put that HBrO2 would be a stronger acid because it has a weaker bond strength than HClO2, similar to how HCI is a stronger acid than HF, but the textbook says that HClO2 is the stronger acid since it has a greater elect...

Minahil_Tufail_3I

Hi! I'm having trouble figuring out how to solve for the pH and pOH of this problem: 75.0 mL of 3.5 × 10^−4 M HBr (aq) after dilution to 0.500 L.
When finding the M2 value, I keep on getting 5.25*10^3, but the textbook says it should be 5.25*10^-5.

Minahil_Tufail_3I

Hi, I'm confused on how to understand solving this problem:
The molar concentration of HCl in hydrochloric acid is reduced to 12% of its initial value by dilution. What is the difference in the pH values of the two solutions?

Minahil_Tufail_3I

Hi, I was wondering how you would figure out this problem: Select an acid and a base for a neutralization reaction that results in the formation of (b) zinc nitrite. I know that the zinc will be bonded with OH, but the textbook solution says that it is Zn(OH)2, so I was wondering how we know that th...

Minahil_Tufail_3I

I think for some ligands, you can tell by their names. For example, with edta, its full name is: Ethylenediaminetetraacetic. You can see that is has a -di prefix along with a -tetra within its name, and edta has six donor atoms with lone pairs. So, it's a hexadentate ligand.

Minahil_Tufail_3I

Yes, I believe that's correct!

Minahil_Tufail_3I

I believe that coordination compounds are most often octahedral, tetrahedral, and square planar, so that is why seesaw wouldn't be the correct answer for the question. However, I'm not sure exactly why these shapes are the most common.

Minahil_Tufail_3I

For sodium bisoxalato(diaqua)ferrate(III), why do they use bis instead of di? I thought that you only use the 'bis' prefix if the ligand already has a name with di, tri, etc. Is it because aqua uses a di?

Minahil_Tufail_3I

Hi, I was hoping someone could explain to me how the formula would be found for this coordination compound: potassium hexacyanidochromate(III).
Thanks!

Minahil_Tufail_3I

To determine which is the strongest covalent bond of a set of different combinations, you could look at the bond length and the bond order. For example, if one of the molecules has a double bond, then that would be a stronger covalent bond than a molecule held together by a single bond. In another i...

Minahil_Tufail_3I

If there are lone pairs, then I think that the lone pairs would be at the equatorial positions because this would minimize electron repulsion since they would be spread further apart.

Minahil_Tufail_3I

Hi, I was hoping to get some help with this problem, specifically how to determine which is the largest dipole moment. Thank you!

Minahil_Tufail_3I

Hi, this question asked about the molecular shape and the bond angles for each molecule. So, I wrote out the Lewis structure for (CH3)2Be and had Be as my center atom. I put that the molecular shape would be linear, but the textbook solution manual said it would be tetrahedral according to the carbo...

Minahil_Tufail_3I

Hi, I was wondering if someone could help explain the answer for part b of this question:
a) What is the shape of a thionyl chloride molecule? Sulfur is the central atom. (b) How many different OSCl bond angles are there in this molecule?
Thank you!

Minahil_Tufail_3I

The sulfite ion would be a trigonal pyramid, because it is bonded to three Oxygen atoms and also has a lone pair.

Minahil_Tufail_3I

Benzene is a good example to look at in order to understand what a delocalized pi bond is. Since it is a resonance structure, its double bonds can be shifted around, and the resonance hybrid shows that each bond is an average of the possible bonds. A delocalized pi bond is basically describing how t...

Minahil_Tufail_3I

Hi, I was reviewing the outline 3 guide and had a question about where it says, "Know the relative magnitudes of intermolecular forces and hydrogen bonds." Is this referring to how hydrogen bonds release -20 kJ/mol^-1 of energy and dispersion forces release -2 kJ/mol^-1?

Minahil_Tufail_3I

Hi, I think that when electron affinity is negative, it means that energy is being released when an electron is added. I also think that when it is more negative, that means that adding an electron to the atom is more favorable. With positive electron affinity, I believe that's when energy must be a...

Minahil_Tufail_3I

Hi, I think that the h-f, h-n, or h-o would also have to bond to h-f, h-n, or h-o on a different molecule as long as there are existing lone pairs.

Minahil_Tufail_3I

I would definitely print out the periodic table! I'm not sure if we'll really need the constants and equations sheet this time.

Minahil_Tufail_3I

Hi! I was wondering if someone could explain the answer for this problem:
Explain the difference in the boiling points of AsF3 ( 63 ) °C and AsF5 ( − 53 ) °C.
Thanks!

Minahil_Tufail_3I

Hi, I was hoping to get some help with this problem: In 1999, Karl Christe synthesized and characterized a salt that contained the N 5 + cation, in which the five N atoms are connected in a chain. This cation is the first new all-nitrogen species to be isolated in more than 100 years. Draw the most ...

Minahil_Tufail_3I

Hi, I'm having trouble figuring out how to go about solving this problem: Place the following molecules or ions in order of decreasing bond length: (a) the CO bond in CO, CO2, CO3^2 − ;(b) the SO bond in SO2 , SO3 , SO3^2− ;(c) the CN bond in HCN, CH2NH , CH3NH2 . Explain your reasoning.
Thank you!

Minahil_Tufail_3I

Hi, I was wondering if I could get some help with this problem:
Determine the numbers of electron pairs (both bonding and lone pairs) on the iodine atom in (b) ICl4^-

Minahil_Tufail_3I

Hi, Because it's asking for which M^3+ ions these configurations represent, it's basically asking which atoms, when they lose three of their electrons, are represented by these configurations. So, for a) [Ar]3d^6, you would then add three electrons to this configuration to determine what this metal'...

Minahil_Tufail_3I

Hi, I think that carbon has a higher electron affinity than nitrogen because whereas nitrogen's p-orbitals are half-full, carbon's aren't. The half-filled p-orbitals gives nitrogen some more stability, meaning it then has a lower electron affinity. I'm not sure if there are more exceptions like this...

Minahil_Tufail_3I

Hi, I was checking my answer in the book, and I was wondering why for BrF3's lewis structure, one of the F atoms loses two electrons while Br gains them?

Minahil_Tufail_3I

Hi, I'm a bit confused on how to figure out the answer for this question:
Which M^2+ ions (where M is a metal) are predicted to have the following ground-state electron configurations: (a) [Ar]3d^7

Minahil_Tufail_3I

Why are single bonds weaker than double bonds?

Minahil_Tufail_3I

Hi, Valence electrons only refer to the electrons in the outermost shell, so you don't add up the total electrons listed in the configuration. Looking at the electron configuration, we know that 5 is larger than 4, meaning the valence electrons will be found in this energy level. Then, you add up th...

Minahil_Tufail_3I

The ground state refers to the electron configuration we find based off of looking at its placement on the periodic table, and it also represents the lowest energy state of the electron. As for the excited state, this means at least one valence electron has moved to a higher energy level, increasing...

Minahil_Tufail_3I

The value of l always takes on values starting from 0 and ending to whatever the value of n-1 is. For example, if n = 3, then l = 0, 1, 2, because 3-1 = 2, meaning this is the highest value l can be.

Minahil_Tufail_3I

In order of the largest radius to the smallest, it would be: Rb-, Rb, Rb+. This is because Rb- means that the element has gained an electron, overall increasing electron repulsion that causes the radius to grow. As for Rb+, the element has now lost an electron, meaning it has a decreased electron re...

Minahil_Tufail_3I

Hi, Personally, I don't draw it out to help me find the answer. Because, it's asking specifically for the value of ml in the 4s subshell, it establishes that n = 1. After all, the s-block refers to when the principal quantum number is 1, meaning the electron is in the first energy level. After figur...

Minahil_Tufail_3I

Hi, for this problem, I didn't double the radius after finding the uncertainty within 1%. I think because the question specifies that the uncertainty is found within the radius, you don't have to double it like you normally would to find the diameter.

Minahil_Tufail_3I

Hi, The 60 W is basically telling you how many joules per second the bulb is burning— in this case, the bulb burns 60 joules per second, and as it burns those 60 joules, it emits 11 J of infrared radiation. For this problem, I first used the formula E = hc/lambda: E = (6.626 * 10^-34 Js) (3.00*10^8 ...

Minahil_Tufail_3I

Hi, so the problem tells you that the wavelength is 102.557 nm. Using the electromagnetic spectrum, we know that 102.557 nm lies within the wavelength range for ultraviolet light. Therefore, we now know that the light being excited to another energy level is ultraviolet light. Because of this, we ca...

Minahil_Tufail_3I

I'm pretty sure the textbook made an error with this problem by using 5 as delta v rather than 10. However, you also multiplied delta p by Planck's constant when it should be h/(4pi * delta p).

Minahil_Tufail_3I

Hi, I'm confused on how to figure out when electrons are either paired or have parallel spins. Is there a general rule to determine this?

Minahil_Tufail_3I

Hi, I was hoping to get some help with this problem:
In 1.0 s, a 60 W bulb emits 11 J of energy in the form of infrared radiation (heat) of wavelength 1850 nm. What is the energy per photon of light emitted?
How many photons of infrared radiation does the lamp generate in 1.0 s?

Thanks!

Minahil_Tufail_3I

I did the same thing I think as the other person but wrote it out using the equation editor so you could see it better :) E=h\nu =6.626\cdot 10^{-34}Js(1.14\cdot 10^{14}m/s)=7.55\cdot 10^{-20}J E_{4}=\frac{-hR}{n^{2}}=\frac{-6.626\cdot 10^{-34}Js (3.29\cdot 10^{15}Hz)}{16}=-1.36\cdo...

Minahil_Tufail_3I

Hi, I was able to solve this problem: Protons and neutrons have nearly the same mass. How different are their wavelengths? Calculate the wavelength of each particle when traveling at 2.75 × 10^5 m⋅s^−1 in a particle accelerator and report the difference as a percentage of the wavelength of the neutr...

Minahil_Tufail_3I

Hi, I'm confused on how to solve part b for this question and would appreciate some help with it: Sodium vapor lamps, used for public lighting, emit yellow light of wavelength 589 nm. How much energy is emitted by (a) an excited sodium atom when it generates a photon; (b) 5.00 mg of sodium atoms emi...

Minahil_Tufail_3I

Hi, I also got stuck on this problem and was confused how we know to use the Lyman series for this problem. I found this visual in the textbook that helped me though:

It seems like visible light uses the Balmer series, and ultraviolet light uses the Lyman series.

Minahil_Tufail_3I

Hi, I got the same balanced equation! The way I worked it out was through how the question said solid boron was ‘extracted’ from solid boron oxide which means boron oxide has to be one of the reactants if boron was then removed from it. The process in how it was removed was by boron oxide reacting w...

Minahil_Tufail_3I

Hi, I was hoping to get some help with this problem: Sodium bromide, NaBr, which is used to produce AgBr for use in photographic film, can itself be prepared as follows: Fe + Br2 --> FeBr2 FeBr2 + Br2 --> Fe3Br8 Fe3Br8 + Na2CO3 --> NaBr + CO2 + Fe3O4 What mass of iron, in kilograms, is needed to pro...

Minahil_Tufail_3I

Hi! In E.9 when they ask for formula units, they basically just want you to convert from the amount of mols to the number of atoms, ions, or molecules in that amount by using Avogadro's number, 6.022 * 10^23.

Minahil_Tufail_3I

Hi! The formula for magnesium sulfate heptahydrate would be MgSO4 · 7H2O. For part a, I first found the molar mass of the molecule which you'd find by doing: 24.31 g/mol Mg + 32.07 g/mol S + 4(16.00) g/mol O + 7(18.02) g/mol H20 = 246.52 g/mol MgSO4 · 7H2O Ordinarily, you wouldn't take into consider...

Search found 101 matches