CHEMISTRY COMMUNITY

Jessica Kwek 4F

At equilibrium, delta G would be 0 since the reactants and products are occurring at the same rate, which means that the reaction favors neither side.

Jessica Kwek 4F

Oxidation is when electrons are lost while reduction is when electrons are gained.

Jessica Kwek 4F

The salt bridge is in charge of the transfer of electrons.

Jessica Kwek 4F

Yes, if you have enough information you should be able to use the values of Q and K.

Jessica Kwek 4F

When balancing half reactions, make sure that your electrons cancel out. They would cancel as long as the number of electrons on both sides are equal to each other.

Jessica Kwek 4F

Positive delta S is not information to determine whether the reaction is spontaneous or not. You would need to look at the over Gibbs Free Energy equation.

Jessica Kwek 4F

Temperature remains constant during phase change because heat energy is stored as potential energy.

Jessica Kwek 4F

Entropy is used to describe the randomness and therefore disorder of molecules in the given reaction/system. It measures the number of possible arrangements the atoms in the system could have.

Jessica Kwek 4F

Gaining heat would result in a positive q value whereas releasing heat would result in a negative q value.

Jessica Kwek 4F

A closed system can only be changed by temperature, pressure, or volume. In a closed system, neither reactants or products can enter or escape, but the transfer of energy is allowed.

Jessica Kwek 4F

After compressing a gas, the reaction would favor the side with less moles of gas because this reduces the number of particles in the gas. Volume and pressure have an inverse relationship.

Jessica Kwek 4F

An isothermal process is a change of system where the temperature remains constant. Therefore, delta U would be equal to 0.

Jessica Kwek 4F

Entropy is a state function since they describe quantitatively an equilibrium state of a thermodynamic system.

Jessica Kwek 4F

A closed system has a fixed amount of matter, but it can only exchange energy with the surroundings.
An isolated system can neither exchange matter nor energy with the surroundings.

Jessica Kwek 4F

It requires energy to be inputted in order to break bonds, which is why breaking bonds makes enthalpy positive. Therefore, forming bonds would make enthalpy negative.

Jessica Kwek 4F

This tells you that the values of pressure and volume would not change.

Jessica Kwek 4F

Question: Rank the following solutions in order of increasing pH: (a) 1.0 3 1025 m HCl(aq); (b) 0.20 m CH3NH3Cl(aq); (c) 0.20 m CH3COOH(aq); (d) 0.20 m C6H5NH2(aq). Justify your ranking. How do we calculate the pH of the weak acid/bases using an ice table? I am confused on part b since CH3NH3Cl is a...

Jessica Kwek 4F

Regarding calculations, you usually have to use an ICE table for weak acids and weak bases since they do not dissociate completely. An ICE table is not needed when doing calculations for strong acids and strong bases.

Jessica Kwek 4F

This would vary depending on the situation, such as the overall heat change of the system.

Jessica Kwek 4F

You are able to skip the ICE table when K is less than 10^-3. If K is greater than 10^-3, you have to use the quadratic formula to solve for x.

Jessica Kwek 4F

Endothermic includes absorbing heat and breaking bonds.
Exothermic includes releasing heat and forming bonds.

Jessica Kwek 4F

Since the chemical reaction is endothermic, increasing the temperature would shift the reaction to the product side. Therefore, it would increase the formation of X.

Jessica Kwek 4F

Pure solids and liquids are not considered when calculating the equilibrium constant.

Jessica Kwek 4F

Change in pressure does not affect the equilibrium act it does not react with anything in the reaction.

Jessica Kwek 4F

Yes. When the volume of reaction is increased, K will shift to the side with more moles.

Jessica Kwek 4F

The equilibrium constant does not change when pressure is increased by adding an inert gas because it does not react with anything in the reaction. The concentration of each reactant are not changed. The system will still be at equilibrium, which leaves K to remain the same.

Jessica Kwek 4F

You would calculate the reactant quotient the same way that you calculate the equilibrium constant. You solve for the reactant quotient when the reaction is not at equilibrium. The equilibrium constant is calculated when the reaction is at equilibrium.

Jessica Kwek 4F

For 5l.7, the question asks whether the reaction will have a tendency to form products or reactants at equilibrium where it is given that Q=1. How do we find the value of K for the reaction to compare it to Q?

Jessica Kwek 4F

K is written in terms of partial pressures since the reactants and products for both reactions all in gas phase. This means that you would write the expression for the equilibrium constant K as a formula for Kp. This includes the partial pressure of the product in the numerator, raised to a power eq...

CHEMISTRY COMMUNITY

Search found 29 matches

Re: Equilibrium

Re: Reduction vs. oxidation

Re: Salt Bridge

Re: Sign of delta G

Re: Balancing half reactions

Re: Positive ∆S

Re: phase changes, temperature constant?

Re: Entropy + Disorder

Re: Endothermic vs Exothermic

Re: Closed Systems

Re: Compressing a gas

Re: Isothermal

Re: Entropy

Re: 4A.1

Re: reaction enthalpy

Re: Constant Pressure

6D 13

Re: Weak and strong acids/bases

Re: Endo/Exothermic Reactions

Re: ICE and quadratic formula

Re: Endothermic and exothermic

Re: 5.33

Re: K based on phases

Re: Pressure

Re: Increasing volume

Re: Pressure's Effect on Equilibrium

Re: Reactant Quotient vs Equilibrium Constant

5l.7

Re: 5G.3