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Rates
Acids/Bases
Le Chatlier's Principle
Equilibrium
100

What is the rate of the rxn:

k=[A]2[B]

if both A and B are tripled?

27x the rate

100

Which of the following are strong acids?:

-Hydrofluoric acid (HF)

-Hydrochloric acid (HCl)

-Carboxylic acid (COOH)

-Hydroiodic acid (HI)

HCl and HI

100

True/False:

Decreasing the pressure by increasing the volume of the rxn container will increase the equilibrium concentration of O3 in the following exothermic rxn:

2O3 (g) ---> 3O2 (g)

False  (will shift to the right)
100

Write the equilibrium expression for:

Br2 (L) --> Br2 (aq)

Kc= [Br2]

200
The half-life of Oxygen-15 is 2 minutes. What fraction of a sample of O-15 will remain after 5 half-lives?

1/32

200

What's the conjugate base of HCl?

Cl-

200

Consider the following equilibrium:

H2O2 (L) --> H2 (g) + O2 (g)

Which way will the equilibrium shift if some concentration of H2 is taken away?

Right

200

A rxn mixture initially contains 0.75 M of HI. At equilibrium, the concentration of I2 was found to be 0.300 M. Calculate the equilibrium concentration of HI in the mixture.

2HI --> H2 + I2

0.15 M

300

Under some conditions, hydrogen peroxide, H2O2, decomposes by at 1st order rxn with a half-life of 2.16*104 seconds. Calculate the rate constant for this rxn.

k=3.21*10-5 s-1

300

What's the conjugate acid of NH3?

NH4+

300

Is the following rxn exothermic or endothermic?:

N2 (g) + 3H2 (g) --> 2NH3 (g)

Exothermic
300

2.0 M of I2 and 2.0 M of Br2 are initially present in a rxn mixture. Calculate the equilibrium concentration of I2, Br2, and IBr at 425K when Kc=100. 

I2 + Br2 --> 2IBr

[I2]= 0.33 M

[Br2]= 0.33 M

[IBr]= 3.34 M

400

Find the rate law and the rate constant of the equation: NO + O3 --> NO2 + O2 given the table (drawn on whiteboard)

(on whiteboard)

400

Which species is acting as the base in the following rxn:

H2PO4- + HC3- --> H2CO3 + HPO42-

HC3-

400
Consider the rxn: N2 (g) + 3H2 (g) --> 2NH3 (g)

What happens when we:

a.) Add N2

b.) Remove N2

c.) Increase volume


a.) shift right

b.) shift left

c.) shift left

400

Given the rxn: I2 (g) --> 2I- (g)

The Kc was found to be 5.6*10-12 and [I2]= 0.45 M initially. Find the equilibrium concentrations.

[I2]= 0.45

[2I-]= 1.58*10-6