Question

In: Chemistry

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 will [A] be after 1.5 min?
M

3. Consider the reaction

4PH3(g)

P4(g) + 6H2(g)

At a particular point during the reaction, molecular hydrogen is being formed at the rate of

0.183 M/s.



(a) At what rate is P4 being produced?

M/s

(b) At what rate is PH3 being consumed?

M/s

Solutions

Expert Solution


Related Solutions

The reaction 2A →B is second order in A with a rate constant of 35.1 M−1...
The reaction 2A →B is second order in A with a rate constant of 35.1 M−1 · s−1 at 25°C. (a) Starting with [A]0 = 0.00781 M, how long will it take for the concentration of A to drop to 0.00180 M? s (b) Calculate the half-life of the reaction for [A]0 = 0.00781 M. s (c) Calculate the half-life of the reaction for [A]0 = 0.00269 M.   s 2. Given the same reactant concentrations, the reaction CO(g) + Cl2(g)...
The rate constant for the reaction: 2A -> 2B + C is 0.881M-1*s-1 at 333 degrees...
The rate constant for the reaction: 2A -> 2B + C is 0.881M-1*s-1 at 333 degrees Celcius. (a) Starting with a concentration of 0.0955 M, calculate the concentration of A after 12.5 seconds. (b) Calculate the half-live when [A] = 0.0444 M.
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?
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.
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 ?
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?
The reaction, 2A + 2B → C + D, has a rate constant of 6.0 ×...
The reaction, 2A + 2B → C + D, has a rate constant of 6.0 × 10-3 M-2 s-1 at 0°C. From this information, can we determine the order of this rate law? If so what is the order?
A reaction has a rate constant of 1.19×10−2 /s at 400. K and 0.693 /s at...
A reaction has a rate constant of 1.19×10−2 /s at 400. K and 0.693 /s at 450. K. A) Determine the activation barrier for the reaction B) What is the value of the rate constant at 425 K
For a given reaction, the rate constant is k'= 2.0 * 10^-4 L*mol^-1*s^-1 at T' =...
For a given reaction, the rate constant is k'= 2.0 * 10^-4 L*mol^-1*s^-1 at T' = 298K and k= 4.5 * 10^-3 L*mol^-1*s^-1 at T=345K Calculate the Arrhenius parameter A
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT