The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain...
The reaction 4 HBr(g) + O2(g) 
2 H2O(g) + 2 Br2(g) was studied at a certain
temperature with the following results:
| Experiment | [HBr(g)] (M) | [O2(g)] (M) | Rate (M/s) |
|---|---|---|---|
| 1 | 0.00579 | 0.00579 | 0.365 |
| 2 | 0.00579 | 0.0116 | 0.732 |
| 3 | 0.0116 | 0.00579 | 0.732 |
| 4 | 0.0116 | 0.0116 | 1.47 |
(a) What is the rate law for this reaction?
______
(b) What is the value of the rate constant?
______
(c) What is the reaction rate when the concentration of HBr(g) is
0.00598 M and that of O2(g) is 0.0156
M if the temperature is the same as that used to obtain
the data shown above?
____M/s
Homework Answers
![from expo, doubling the CO2], rate also doubles. un order worot d = 1. from exp 3, 4 doubling the [HBr], rate also doubles un](http://img.homeworklib.com/questions/634f46f0-7216-11ea-88ad-138bb671a80e.png?x-oss-process=image/resize,w_560)
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The reaction 4 HBr(g) + O2(g)
2 H2O(g) + 2 Br2(g) was studied at a certain...
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at a certain...
The reaction 2 NO(g) + 2 H2(g)
N2(g) + 2 H2O(g) was studied at a certain
temperature with the following results:
Experiment
[NO(g)] (M)
[H2(g)] (M)
Rate (M/s)
1
0.0867
0.0867
71.7
2
0.0867
0.173
143
3
0.173
0.0867
285
4
0.173
0.173
570.
(a) What is the rate law for this reaction?
Rate = k [NO(g)] [H2(g)]
Rate = k [NO(g)]2
[H2(g)]
Rate = k [NO(g)] [H2(g)]2
Rate = k [NO(g)]2 [H2(g)]2
Rate = k [NO(g)] [H2(g)]3
Rate =...
6) For the reaction 4 HBr(aq) + O2(g) = 2 Br2(aq) + 2 H2O(l), K. -6.7...
6) For the reaction 4 HBr(aq) + O2(g) = 2 Br2(aq) + 2 H2O(l), K. -6.7 x 1010. Use this information to calculate the equilibrium constant for each of the following reactions. a) 2 HBr(aq) + 12 O2(g) + Brz(aq) + H2O(1) b) 4 Br2(aq) + 4H2O(l) = 8 HBr(aq) + 2 O2(g)
0/4 Submissions Used 7. /0.1 points The reaction 4 HBr(p) + 0,(g)-2 H O(g) +2 Bry(o)...
0/4 Submissions Used 7. /0.1 points The reaction 4 HBr(p) + 0,(g)-2 H O(g) +2 Bry(o) was studied at a certain temperature with the following results: 02(o)] (M) Rate (M/s) [HBr(g)) (M) Experiment 0.2011 0.404 0.404 0.812 0.00538 0.0108 0.00538 1 0.00538 0.00538 0.0108 0.0108 0.0108 (a) What is the rate law for this reaction O Rate k [HBr(o)) (0(a) O Rate k [HBr(a) (0(o)1 O Rate k [HBe(a)] (02(0) O Rate k [HBr(o))2 t0(0)) O Rate k [HBr(a)] [02(o)...
2. Good question. The reaction 2NO(g) + O2(g) → 2NO.(g) was studied by a CHEM 154...
2. Good question. The reaction 2NO(g) + O2(g) → 2NO.(g) was studied by a CHEM 154 student and the following data were obtained for the rate of consumption of oxygen. Write the rate law for this reaction. What would be the initial rate for an experiment where [NO), = 1.03 x 10-mol/L and [O),= 1.22 x 102 mol/L? Expt. [NO], (M) (01. (M) Initial rate (M/s) 1 1.66 x 10-3 1.66 x 10-3 3.32 x 10-5 2 4.98 x 10-...
1. The rate of the reaction (8) + NO2(g) → NO(g) + O2(g) was studied at...
1. The rate of the reaction (8) + NO2(g) → NO(g) + O2(g) was studied at a certain temperature. (a) In the first set of experiments, NO2 was in large excess, at a concentration of 1.0 x 10'3 molecules/cm with the following data collected: Time (s) [O] (atoms/cm) O 5.0 x 10' 1.0 x 102 1.9 x 10° 2.0 x 102 6.8 x 108 3.0 x 10-2 2.5 x 108 What is the order of the reaction with respect to...
The elementary reaction 2 H2O(g) + 2 H2(g) + O2(g) proceeds at a certain temperature until...
The elementary reaction 2 H2O(g) + 2 H2(g) + O2(g) proceeds at a certain temperature until the partial pressures of H20, H2, and O2 reach 0.010 bar, 0.0025 bar, and 0.0015 bar, respectively. What is the value of the equilibrium constant at this temperature? K = 11
For the reaction H2 (g) + Br2 (g) → 2 HBr (g) AH° = - 104...
For the reaction H2 (g) + Br2 (g) → 2 HBr (g) AH° = - 104 kJ Which of the following statements are correct? 1) Increasing the temperature will make the equilibrium ratio [HBr] / [H2] decrease. 2) At equilibrium the specific rate constant for the forward reaction must equal the specific rate constant for the reverse reaction. 3) At equilibrium the rate of the forward reaction will equal the rate of the reverse reaction. 4) A catalyst that increases...
4. In the reaction: CH4 (g) + 2 O2(g) → CO2(g) + 2 H2O(g) the initial...
4. In the reaction: CH4 (g) + 2 O2(g) → CO2(g) + 2 H2O(g) the initial concentration of CO2 is 0.000 M, and after 30.0 sec, the concentration of CO2 is 0.670 M. What is the average reaction rate over this time span? A) 2.50 M/s B) 0.0223 M/s C) 0.25 m/s D) 1.1 M/s
At 700 K, Kc = 1.56×10–2 for the reaction 2 HBr(g) ⇌ H2(g) + Br2(g). In...
At 700 K, Kc = 1.56×10–2 for the reaction 2 HBr(g) ⇌ H2(g) + Br2(g). In a given experiment, 0.050 mol of H2, and 0.050 mol Br2 are introduced into a 5.0-L flask. What is the equilibrium concentration of HBr?
The reaction 2 HgCl2(aq) + C2042(aq) + 2Cl(aq) + 2 CO2(g) + Hg2Cl2(s) was studied at...
The reaction 2 HgCl2(aq) + C2042(aq) + 2Cl(aq) + 2 CO2(g) + Hg2Cl2(s) was studied at a certain temperature with the following results: Experiment [HgCl2(aq)] (M) [C2042(aq)] (M) Rate (M/s) 0.122 0.122 0.244 0.244 0.122 0.244 0.122 0.244 2.58e-05 0.000103 5.16e-05 0.000206 (a) What is the rate law for this reaction? Rate = k [HgCl2(aq)] [C2042-(aq)] Rate = k [HgCl2(aq)]? (C2042-(aq)] Rate = k [HgCl2(aq)] [C2042-(aq)]2 Rate = k [HgCl2(aq)]2 (C2042-(aq)]2 Rate = k [HgCl2(aq)] (C2042 (aq)]3 Rate = k...
The reaction 2 NO(g) + 2 H2(g)
N2(g) + 2 H2O(g) was studied at a certain
temperature with the following results:
Experiment
[NO(g)] (M)
[H2(g)] (M)
Rate (M/s)
1
0.0867
0.0867
71.7
2
0.0867
0.173
143
3
0.173
0.0867
285
4
0.173
0.173
570.
(a) What is the rate law for this reaction?
Rate = k [NO(g)] [H2(g)]
Rate = k [NO(g)]2
[H2(g)]
Rate = k [NO(g)] [H2(g)]2
Rate = k [NO(g)]2 [H2(g)]2
Rate = k [NO(g)] [H2(g)]3
Rate =...
6) For the reaction 4 HBr(aq) + O2(g) = 2 Br2(aq) + 2 H2O(l), K. -6.7 x 1010. Use this information to calculate the equilibrium constant for each of the following reactions. a) 2 HBr(aq) + 12 O2(g) + Brz(aq) + H2O(1) b) 4 Br2(aq) + 4H2O(l) = 8 HBr(aq) + 2 O2(g)
0/4 Submissions Used 7. /0.1 points The reaction 4 HBr(p) + 0,(g)-2 H O(g) +2 Bry(o) was studied at a certain temperature with the following results: 02(o)] (M) Rate (M/s) [HBr(g)) (M) Experiment 0.2011 0.404 0.404 0.812 0.00538 0.0108 0.00538 1 0.00538 0.00538 0.0108 0.0108 0.0108 (a) What is the rate law for this reaction O Rate k [HBr(o)) (0(a) O Rate k [HBr(a) (0(o)1 O Rate k [HBe(a)] (02(0) O Rate k [HBr(o))2 t0(0)) O Rate k [HBr(a)] [02(o)...
2. Good question. The reaction 2NO(g) + O2(g) → 2NO.(g) was studied by a CHEM 154 student and the following data were obtained for the rate of consumption of oxygen. Write the rate law for this reaction. What would be the initial rate for an experiment where [NO), = 1.03 x 10-mol/L and [O),= 1.22 x 102 mol/L? Expt. [NO], (M) (01. (M) Initial rate (M/s) 1 1.66 x 10-3 1.66 x 10-3 3.32 x 10-5 2 4.98 x 10-...
1. The rate of the reaction (8) + NO2(g) → NO(g) + O2(g) was studied at a certain temperature. (a) In the first set of experiments, NO2 was in large excess, at a concentration of 1.0 x 10'3 molecules/cm with the following data collected: Time (s) [O] (atoms/cm) O 5.0 x 10' 1.0 x 102 1.9 x 10° 2.0 x 102 6.8 x 108 3.0 x 10-2 2.5 x 108 What is the order of the reaction with respect to...
The elementary reaction 2 H2O(g) + 2 H2(g) + O2(g) proceeds at a certain temperature until the partial pressures of H20, H2, and O2 reach 0.010 bar, 0.0025 bar, and 0.0015 bar, respectively. What is the value of the equilibrium constant at this temperature? K = 11
For the reaction H2 (g) + Br2 (g) → 2 HBr (g) AH° = - 104 kJ Which of the following statements are correct? 1) Increasing the temperature will make the equilibrium ratio [HBr] / [H2] decrease. 2) At equilibrium the specific rate constant for the forward reaction must equal the specific rate constant for the reverse reaction. 3) At equilibrium the rate of the forward reaction will equal the rate of the reverse reaction. 4) A catalyst that increases...
4. In the reaction: CH4 (g) + 2 O2(g) → CO2(g) + 2 H2O(g) the initial concentration of CO2 is 0.000 M, and after 30.0 sec, the concentration of CO2 is 0.670 M. What is the average reaction rate over this time span? A) 2.50 M/s B) 0.0223 M/s C) 0.25 m/s D) 1.1 M/s
The reaction 2 HgCl2(aq) + C2042(aq) + 2Cl(aq) + 2 CO2(g) + Hg2Cl2(s) was studied at a certain temperature with the following results: Experiment [HgCl2(aq)] (M) [C2042(aq)] (M) Rate (M/s) 0.122 0.122 0.244 0.244 0.122 0.244 0.122 0.244 2.58e-05 0.000103 5.16e-05 0.000206 (a) What is the rate law for this reaction? Rate = k [HgCl2(aq)] [C2042-(aq)] Rate = k [HgCl2(aq)]? (C2042-(aq)] Rate = k [HgCl2(aq)] [C2042-(aq)]2 Rate = k [HgCl2(aq)]2 (C2042-(aq)]2 Rate = k [HgCl2(aq)] (C2042 (aq)]3 Rate = k...
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