11 Marks: 1 Marks: 1 Choose at least one answer. a . x =0 b . x = 0.5 c . x = 1

Question

11 Marks: 1 Marks: 1 Choose at least one answer. a. x =0 b. x = 0.5 c. x = 1 d. x = 2 e. y = 0 f. y = 0.5 g. y = 1 h. y = 2 i. Itermediate: O2 j. Itermediate: N2O4 k. Itermediate: O3 l. This rate law is consistent with the experimental one. Choose at least one answer. Question12 Marks: 1 Marks: 1 Choose at least one answer. a. x =0 b. x = 0.5 c. x = 1 d. x = 2 e. y = 0 f. y = 0.5 g. y = 1 h. y = 2 i. Itermediate: O2 j. Itermediate: NO3 k. Itermediate: O3 l. Consistent Choose at least one answer. Question13 Marks: 1 Marks: 1 Choose at least one answer. a. Reaction order at 310 K: 0 b. Reaction order at 310 K: 1 c. Reaction order at 310 K: 2 d. Reaction order at 315 K: 0 e. Reaction order at 315 K: 1 f. Reaction order at 315 K: 2 Choose at least one answer. Question14 Marks: 1
What is the rate constant at 310 K? (Use SI units. For example, use seconds not minutes or hours.) Answer: Question14 Marks: 1 Marks: 1
What is the rate constant at 310 K? (Use SI units. For example, use seconds not minutes or hours.) Answer:
What is the rate constant at 310 K? (Use SI units. For example, use seconds not minutes or hours.) Answer: Answer: Question15 Marks: 1
What is the rate constant at 315K? Answer: Question15 Marks: 1 Marks: 1
What is the rate constant at 315K? Answer:
What is the rate constant at 315K? Answer: Answer: Question16 Marks: 1
What is the activation energy (in J/mol)? Answer: Question16 Marks: 1 Marks: 1
What is the activation energy (in J/mol)? Answer:
What is the activation energy (in J/mol)? Answer: Answer: Question17 Marks: 1 When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay:

HCOOH(g) ?CO2(g) + H2 (g)

The rate of reaction is monitored by measuring the total pressure in the reaction container.

Time (s) . . . P (torr)
0 . . . . . . . . . 220
50 . . . . . . . . 324
100 . . . . . . . 379
150 . . . . . . . 408
200 . . . . . . . 423
250 . . . . . . . 431
300 . . . . . . . 435

At the start of the reaction (time = 0), only formic acid is present. What is the formic acid pressure (in torr) when the total pressure is 317? Hint: use Dalton's law of partial pressure and the reaction stoichiometry. Answer: Question17 Marks: 1 Marks: 1 When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay:

HCOOH(g) ?CO2(g) + H2 (g)

The rate of reaction is monitored by measuring the total pressure in the reaction container.

Time (s) . . . P (torr)
0 . . . . . . . . . 220
50 . . . . . . . . 324
100 . . . . . . . 379
150 . . . . . . . 408
200 . . . . . . . 423
250 . . . . . . . 431
300 . . . . . . . 435

At the start of the reaction (time = 0), only formic acid is present. What is the formic acid pressure (in torr) when the total pressure is 317? Hint: use Dalton's law of partial pressure and the reaction stoichiometry. Answer: When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay:

HCOOH(g) ?CO2(g) + H2 (g)

The rate of reaction is monitored by measuring the total pressure in the reaction container.

Time (s) . . . P (torr)
0 . . . . . . . . . 220
50 . . . . . . . . 324
100 . . . . . . . 379
150 . . . . . . . 408
200 . . . . . . . 423
250 . . . . . . . 431
300 . . . . . . . 435

At the start of the reaction (time = 0), only formic acid is present. What is the formic acid pressure (in torr) when the total pressure is 317? Hint: use Dalton's law of partial pressure and the reaction stoichiometry. Answer: Answer: Question18 Marks: 1 What is the rate constant (in s-1)? (To determine the rate, you must use a reactant concentration or pressure. Use the procedure of in the previous question to determine the HCOOH pressure as a function of the total pressure.) Answer: Question18 Marks: 1 Marks: 1 What is the rate constant (in s-1)? (To determine the rate, you must use a reactant concentration or pressure. Use the procedure of in the previous question to determine the HCOOH pressure as a function of the total pressure.) Answer: What is the rate constant (in s-1)? (To determine the rate, you must use a reactant concentration or pressure. Use the procedure of in the previous question to determine the HCOOH pressure as a function of the total pressure.) Answer: Answer: Question19 Marks: 1
What is the half-life (in s)? Question19 Marks: 1 Marks: 1
What is the half-life (in s)?
What is the half-life (in s)? a. x =0 b. x = 0.5 c. x = 1 d. x = 2 e. y = 0 f. y = 0.5 g. y = 1 h. y = 2 i. Itermediate: O2 j. Itermediate: N2O4 k. Itermediate: O3 l. This rate law is consistent with the experimental one.

Explanation / Answer

i have helped. what i can do. please rate my answer

14) Rate constant at 310K is .278

15)Rate constant at 315K is .448

16)

and use Arrhenius equation:

k = A*exp(-E/RT)

to find the activation energy. Basically, your data is k1 at T1 and k2 at T2. Put them into Arrhenius equation, we have:

k1 = A*exp(-E/(R*T1)) . . . .(1)

k2 = A*exp(-E/(R*T2)) . . . .(2)

(1)/(2), we have:

k1/k2 = exp((E/R)*(1/T2-1/T1))

Take natural logrithm:

Ln(k1/k2) = (E/R)*(1/T2-1/T1)

Thus: E = R*Ln(k1/k2) /(1/T2-1/T1)

Now, every fact at the right side of the expression is known. Please do the math to calculate out the activation energy yourself. Good Luck!!

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