General Chemistry 2

The following initial rate data was collected for the reaction, 2 NO + O$_2$ $\longrightarrow$ 2NO$_2$

[NO$_2$]$^X$[O$_2$]$^Y$

The following initial rate data was collected for the reaction, CH$_3$Br + OH$^-$ $\longrightarrow$ CH$_3$OH + Br$^-$

B. What is the rate constant?

The following initial rate data was collected for the reaction, A + B + C $\longrightarrow$ products

What are the reaction orders with respect to the reactants?

A $\longrightarrow$ products

t$_\frac{1}{2}$ = 180s

A. What % of A is left unreacted at 900 s?

B. What is the rate at [A] = 0.50 M?

The half life of uranium-238 is 4.51 x 10$^9$ years. What is the rate constant? How much uranium-238 is left after 4 half lives if we start with 64 mg?

A first order reaction has a half life of 20.0 min.

A. Calculate the rate constant for this reaction

B. How much time is required for this reaction to be 75% complete?

Below is a proposed mechanism for a reaction, with k2 > k1. What is the rate law?

$NO_2 + CO~ \xrightarrow{k_1}~ NO + NO_3$

$NO_3 + CO~ \xrightarrow{k_2}~ NO_2 + CO_2$

Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

$NO_2 + CO~ \xrightarrow{k_1}~ NO + NO_3$

$NO_3 + CO~ \xrightarrow{k_2}~ NO_2 + CO_2$

Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

$NO+ Br_2~ \mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~ NOBr_2$

$NOBr_2 + NO~ \xrightarrow{k_2}~ NOBr + NOBr$

For the mechanism proposed below, use the quasi (pseudo) steady state approximation to determine the overall rate law assuming the pseudo steady state.

$2~NO~+~2 H_2~\longrightarrow~2~H_2O~+~N_2~~{overall}$

$2~NO+~H_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~N_2O~+~H_2O$ $$

$N_2O~+~H_2~\xrightarrow{k_2}~N_2~+~H_2O$

Use the pseudo steady state hypothesis to derive the rate law for the rate of production of P

$E~+~S~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~ES$

$ES~\xrightarrow{k_2}~E~+P$

Derive the rate law for the following reaction mechanism

$OCl^-~H_2O~\leftrightharpoons~HOCl + OH^-$

$I^- + HOCl~\longrightarrow~HOI + Cl^-~~{slow step}$

$HO + OH^-\longrightarrow~H_2O + OI^-$

Find equilbirium concentrations of each species when starting with 3.0 M I$_2$

I$_2$ (g) $\leftrightharpoons$ 2 I (g) , K$_C$ = 3.8 x 10$^{-5}$

A 3.050 L reaction vessel contains 0.3500 mol CO, 0 mol Cl$_2$, 0.05500 mol COCl$_2$. Find the molarity of Cl$_2$ at equilibrium.

CO + Cl$_2$ $\leftrightharpoons$ COCl$_2$ , K$_C$ = 1200

At 1000 K, 0.250 mol SO$_2$ and 0.200 mol O$_2$ react in a 10.0 L reaction vessel to form 0.162 mol of SO$_3$ at equilibrium. What is K$_{eq}$ at 1000 K for the reaction?

2 SO$_2$ (g) + O$_2$ (g) $\leftrightharpoons$ 2 SO$_3$ (g)

3 A(s) + 5 B(g) $\leftrightharpoons$ 5 C(g) + 6 D(s) $\triangle$H = 0 kJ

A. Predict the change in A when D is added

B. Predict the direction of reaction when the pressure is increased

C. Predict the direction of reaction when the heat is increased

Determine how the following changes will effect the concentrations of the reactants and products.

2 NO$_2$ (g) $\leftrightharpoons$ N$_2$O$_4$ (g) $\triangle$H = -58 kJ

A. Addition of N$_2$O$_4$

B. Removal of NO$_2$

C. Increase in volume

D. Decrease in temperature

heat + 2 NO$_2$(g) $\leftrightharpoons$ N$_2$O$_4$(g)

Which of the following changes will not be effective in increasing the amount of N$_2$O$_4$? (more than one answer may be chosen)

a decrease in volume, an increase in heat, an addition of N$_2$, or removal of N$_2$O$_4$

A vessel contains 0.5 M acetic acid, which dissociates as shown below. What is the concentration of the acetate ion at equilibrium, given the K$_a$ below?

CH$_3$COOH (aq) $\leftrightharpoons$ CH$_3$OO$^{-}$ (aq) + H$^+$ (aq) , K$_a$ = 1.8 x 10$^{-5}$

Define acids and bases according to the Bronsted-Lowry and Lewis theories.