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For the reaction
BrO3- + 5 Br- + 6 H+ ---> 3 Br2 + 3 H2O
at a particular time, -/[BrO3-]// t = 1.5 10-2 M/s.
What is -/[Br-]//t at the same instant?

Question 2
Question: The reaction
A + 2 B ---> products
has been found to have the rate law,
rate = k [A] [B]2.

While holding the concentration of A constant, the concentration of B is increased from x to 3x.
Predict by what factor {an integer multiple} the rate of reaction increases.

Question 3 Multiple Choice
Question: Nitric oxide gas (NO) reacts with chlorine gas according to the equation

NO + ½ Cl2 ® NOCl.

The following initial rates of reaction have been measured for the given reagent concentrations.

Expt. # Rate (M/hr) NO (M) Cl2 (M)

1 1.19 0.50 0.50

2 4.79 1.00 0.50

3 9.59 1.00 1.00

Which one of the following is the rate law (rate equation) for this reaction?

A. rate = k [NO]

B. rate = k [NO] [Cl2]1/2

C. rate = k [NO] [Cl2]

D. rate = k [NO]2 [Cl2]

E. rate = k [NO]2 [Cl2]2

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General Chemistry

1. 4CuO(s) + CH4(g) CO2(g) + 4Cu(s) + 2H2O(g)
The value of Kc for this reaction is 1.10 at 25.0°C. What is the
value of Kp for this reaction? (R = 0.0821 L-atm/K-mol)

a. 4.63
b. 26.9
c. 658
d. 37.2
e. 1.52 x 10-3

2. At a certain temperature, a flask at equilibrium contains 0.0551 M
HCl, 0.112 M Cl2, and 0.105 M H2. What is the value of Kc for the
equilibrium: 2 HCl(g) → Cl2(g) + H2(g)?

a. 3.87
b. 0.258
c. 11.0
d. 1.63 x 10-5
e. 0.213

3. Consider the following incomplete table of data for the equilibrium
between dinitrogen tetroxide and nitrogen dioxide.

Exp # Equilibrium N2O4 Concentr Equilibrium NO2 Concentration
1 0.00140 M 0.0172 M
2 0.00452 ?
3 0.00280 0.0243

From the information in the table, determine the value of the
missing NO2 concentration at equilibrium.

a. 0.0309
b. 0.0486
c. 9.54 x 10-4
d. 0.115
e. 0.0814

3. Consider the gaseous equilibrium: 2 A → 2 B + C
Determine the value of the missing B concentration at equilibrium.

Exp# [A] at equilibrium [B] at equilibrium [C] at equilibrium
1 0.10 M 0.15 M 0.20 M
2 0.20 0.50 0.072
3 0.35 ? 0.15

a. 0.20
b. 0.35
c. 0.61
d. 0.40
e. 0.37

4. The expression for Kc for the reaction below is _______________.
NiCO3(s) + 2H+(aq) Ni2+(aq) + CO2(g) + H2O(l)

a. [CO2]
b. [NiCO3]/[Ni2+]
c. [Ni2+][CO2]/[H+]2
d. [Ni2+][H+]2
e. [Ni2+]/[NiCO3]

5. Consider the following chemical reaction:
H2(g) + I2(g) 2HI(g)
At equilibrium, the concentrations of H2, I2, and HI were 0.15 M,
0.033 M, and 0.55 M, respectively. The value of Kc for this reaction
is
111
9.0 x 10-3
6.1
23
61

6. Consider the following reaction:

PCl5(g) PCl3(g) + Cl2(g)

Initially, 0.84 mol of PCl5(g) was placed in a 1.0 L flask. At
equilibrium, 0.72 mol of PCl5(g) was present. The value of Kc for
this reaction at this temperature is ___________.

a. 2.0 x 10-2
b. 0.62
c. 0.60
d. 0.12
e. 0.72

7. The value of Kc for the reaction below is 0.016. Under a set of
equilibrium conditions, [HI] = 0.10 M and [H2] = [I2]. Calculate the
concentration of I2 (M).
2HI(g) H2(g) + I2(g)

a. 1.3 M
b. 3.1 x 10-1
c. 0.31
d. 4.0 x 10-2
e. 1.3 x 10-2

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