Question

In: Chemistry

22. The rate constant for a reaction is 4.62 x 10-3 s -1 at 300°C. The...

22. The rate constant for a reaction is 4.62 x 10-3 s -1 at 300°C. The activation energy for the reaction is 46 kJ/mol. What is the rate constant at 600°C?

A. 1.28 x 10-1 s -1 <-Answer

B. 4.66 x 101 s -1

C. 9.37 x 10-1 s -1

D. 4.72 x 103 s -1

E. 9.37 x 103 s -1

Please explain the process in many details.

Solutions

Expert Solution

From Ahrrenius equation;

K1 = A*exp(-Ea/(RT1))

K2 = A*exp(-Ea/(RT2))

Note that A and Ea are the same, they do not depend on Temperature ( in the range fo temperature given)

Then

Divide 2 and 1

K2/K1 = A/A*exp(-Ea/(RT2)) / exp(-Ea/(RT1))

Linearize:

ln(K2/K1) = -Ea/R*(1/T2-1/T1)

get rid of negative sign

ln(K2/K1) = Ea/R*(1/T1-1/T2)

for a generic value:

ln(K) = -Ea/R*(1/T) + ln(A)

where:

x-axis = 1/T ; inverse value of absolute temperature

y-axis = ln(K) , natural log of the rate constant

slope = -E/R or Acitvation Energy divided by Ideal Gas Constant

y-intercept = ln(A) ; natural log of the Frequency Factor

Substitute

ln(K2/(4.62*10^-3) = (46000/8.314)*(1/(300+273) - 1/(600+273))

K2 = (4.62*10^-3)*exp(3.31818)

K2 = 0.1275

K = 1.275*10^-1

choose A

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

1. The rate constant for the reaction 2A → B is 7.25 × 10−3 s−1 at...
1. The rate constant for the reaction 2A → B is 7.25 × 10−3 s−1 at 110 ° C. The reaction is first order in A. How long (in seconds) will it take for [A] to decrease from 1.81 M to 0.750 M? 2. The following reaction, 2A → B is first order in A and has a rate constant, k, of 7.5 × 10−3 s−1 at 110 ° C. With a starting concentration of [A] = 1.65 M, what...
A reaction has a rate constant of 1.28×10−4 s−1 at 25 ∘C and 0.233 s−1 at...
A reaction has a rate constant of 1.28×10−4 s−1 at 25 ∘C and 0.233 s−1 at 75 ∘C. What is the value of the rate constant at 15 ∘C?
A reaction has a rate constant of 1.22×10−4 s−1 at 28 ∘C and 0.229 s−1 at...
A reaction has a rate constant of 1.22×10−4 s−1 at 28 ∘C and 0.229 s−1 at 79 ∘C . What is the value of the rate constant at 16 ∘C ?
The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial...
The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial reactant concentration was 0.850 M, what will the concentration be after 15.0 minutes? A zero-order reaction has a constant rate of 2.80×10−4 M/s. If after 75.0 seconds the concentration has dropped to 9.00×10−2 M, what was the initial concentration? A zero-order reaction has a constant rate of 2.80×10−4M/s. If after 75.0 seconds the concentration has dropped to 9.00×10−2M, what was the initial concentration?
a. A certain first-order reaction (A→products) has a rate constant of 3.00×10−3 s−1 at 45 ∘C....
a. A certain first-order reaction (A→products) has a rate constant of 3.00×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? b. A certain second-order reaction (B→products) has a rate constant of 1.85×10−3M−1⋅s−1 at 27 ∘C and an initial half-life of 300 s . What is the concentration of the reactant B after one half-life?
a) At 25 °C the first-order rate constant for a reaction is 2.0 x 103 s-1....
a) At 25 °C the first-order rate constant for a reaction is 2.0 x 103 s-1. The activation energy is 15.0 kJ/mol. What is the value of the rate constant at 75 °C? (5 pts). b)A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 8.1 x 10-2 s-1 at 0 °C and 20 °C, respectively. What is the value of the activation energy? (5 pts)
The equilibrium constant, K, for the following reaction is 2.3 x 10-4 at 300 °C: N2...
The equilibrium constant, K, for the following reaction is 2.3 x 10-4 at 300 °C: N2 (g) + C2H2 (g) ⇌ 2 HCN (g). Calculate the equilibrium concentration of HCN when 0.555 moles of N2 and 0.555 moles of C2H2 are introduced into a 0.500 L vessel at 300 °C.
A reaction has a rate constant of 1.23 x 10 ^-2 /s at 400 K and...
A reaction has a rate constant of 1.23 x 10 ^-2 /s at 400 K and .688/s at 450K. What is the activation barrier for the reaction and what is the value of the rate constant at 425 K ?
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If the initial concentration of A is 0.00680 M. what is the concentration after 315 s? b.)The rate constant for this zero-order reaction is 0.0190 M·s–1 at 300 °C. A--> products. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.240 M? c.)The rate constant for this second-order reaction is 0.520 M–1·s–1 at 300 °C. A-->...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If the initial concentration of A is 0.00680 M. what is the concentration after 315 s? b.)The rate constant for this zero-order reaction is 0.0190 M·s–1 at 300 °C. A--> products. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.240 M? c.)The rate constant for this second-order reaction is 0.520 M–1·s–1 at 300 °C. A-->...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT