CHEMISTRY COMMUNITY

Jessica Tsui 1H

For part a, the coefficient does not affect the rate law equation.

Jessica Tsui 1H

In the solutions manual for this problem, the answer subtracts 0.59 from the equation for ln k2 - ln k1. Why do they do this?

Jessica Tsui 1H

Is there a way to calculate A?

Jessica Tsui 1H

The rate law of multi-step reactions can't be predicted from the net reaction, so the slow step determines the rate law.

Jessica Tsui 1H

Zero-order reactions can also occur when there is a catalyst, so the reaction would depend on the catalyst instead of the concentration of reactant.

Jessica Tsui 1H

Why is the half-life for first order reaction the only one that is independent of initial [A]?

Jessica Tsui 1H

In class, Lavelle said when the activation energy is high, the reaction happens very slowly because kinetics, not thermodynamics, controls the reaction. What did he mean by kinetics rather than thermodynamics controlling the reaction?

Jessica Tsui 1H

The chemical that is reduced takes electrons from the other chemical, which is then oxidized, so is the oxidizing agent. Vice versa for the other chemical.

Jessica Tsui 1H

n is the transfer of electrons for the chemicals being reduced and oxidized. In this case, n is equal to 6 because Fe loses 6 electrons when oxidized and Cr gains 6 electrons when reduced after the reaction occurs.

Jessica Tsui 1H

I don't understand how maximum potential is calculated when there is very little current flow. How does that work?

Jessica Tsui 1H

The salt bridge or porous disk between the anode and the cathode allow cation/anion diffusion. This keeps both solutions neutral so that the reaction is able to continue.

Jessica Tsui 1H

Is there a difference between the terms "galvanic" and "voltaic"? Or are they interchangeable?

Jessica Tsui 1H

Why is a reaction at equilibrium have $\Delta$ G = 0?

Jessica Tsui 1H

R is referring to the gas constant.

Jessica Tsui 1H

Hi I was just wondering when our midterms will be passed back to us. Thank you.

Jessica Tsui 1H

Can some explain how the number of energy states/arrangements relates to the calculation for degeneracy?

Jessica Tsui 1H

In reactions with solids and liquids, why is P $\Delta$ V insignificant?

Jessica Tsui 1H

What is the difference between the $\Delta$ H values used for Hess's Law and the $\Delta$ H values used in standard enthalpy in formation?

Jessica Tsui 1H

I'm a little confused. What was the point of showing the integral for the work equation to arrive at the same work of expansion equation (w = -P $\Delta$ V)?

Jessica Tsui 1H

When work is done on a system, w is positive. When work is done by a system, w is negative.

Jessica Tsui 1H

Work done by the system is energy lost, so w is negative. Work done on the system is energy gained, so w is positive.

Jessica Tsui 1H

How does heat depend on the "path taken"?

Jessica Tsui 1H

$\Delta$ H, enthalpy, is the measure of potential energy change of a chemical reaction in kJ/mol, while q measures heat in joules. $\Delta$ H and q are related, in that - $\Delta$ H = +q.

Please correct me if I am wrong.

Jessica Tsui 1H

Are there going to be video modules for the thermochemistry unit?

Jessica Tsui 1H

When two reactions are combined, their K values are multiplied to find the K value of the new reaction.

Jessica Tsui 1H

Can we only assume x is negligible (after ICE table) if the reaction is with a weak acid?

Jessica Tsui 1H

Catalysts simply speed up the rates of both the forward and reverse reactions, and equilibrium will be reached more quickly. The concentrations of reactants and products at equilibrium will be unchanged.

Jessica Tsui 1H

When K>10 3 products are favored, meaning there is largely more product than reactant at equilibrium. The opposite is true for when K<10 -3 . For the intermediate values, neither reactants nor products are "strongly favored", meaning there is a relatively equal amount of reactant and produ...

Jessica Tsui 1H

Decreasing the amount of NH3 increases the yield of NH3 because the system would react in order to get back to chemical equilibrium. Taking away product in the system allows more reactants to react to form more product.

Jessica Tsui 1H

I think Professor Lavelle said it's because solids and liquids aren't changed in concentration during the reaction.

CHEMISTRY COMMUNITY

Search found 30 matches

Re: 6th edition 15.39

6th edition, 15.63

Frequency Factor, A

Re: fast and slow elementary reactions

Re: General Meaning of "Zero Order" Reactions

Half-Life

Kinetics vs. Thermodynamics

Re: oxidizing agent and reducing agent

Re: E cell

Maximum potential

Re: Salt Bridge/Porous Disk

Galvanic/Voltaic Cells

Equilibrium

Re: Van't Hoff Equation

Midterms

Degeneracy

Solids and Liquids

Enthalpy

Equations for w

Re: Work

Re: Piston and value of W

Heat and path taken

Re: H and Q

Thermochemistry Video Modules

Re: Using a Eq. table for questions

Approximation of x

Re: Catalysts

Re: Values of K

Re: Example in Class

Re: Liquids and Solids