Rates
What is the rate of the rxn:
k=[A]2[B]
if both A and B are tripled?
27x the rate
Which of the following are strong acids?:
-Hydrofluoric acid (HF)
-Hydrochloric acid (HCl)
-Carboxylic acid (COOH)
-Hydroiodic acid (HI)
HCl and HI
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)
Write the equilibrium expression for:
Br2 (L) --> Br2 (aq)
Kc= [Br2]
1/32
What's the conjugate base of HCl?
Cl-
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
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
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
What's the conjugate acid of NH3?
NH4+
Is the following rxn exothermic or endothermic?:
N2 (g) + 3H2 (g) --> 2NH3 (g)
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
Find the rate law and the rate constant of the equation: NO + O3 --> NO2 + O2 given the table (drawn on whiteboard)
(on whiteboard)
Which species is acting as the base in the following rxn:
H2PO4- + HC3- --> H2CO3 + HPO42-
HC3-
What happens when we:
a.) Add N2
b.) Remove N2
c.) Increase volume
a.) shift right
b.) shift left
c.) shift left
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