What is the concentration of A after 42.9 minutes for the reaction A → Products when...

Question

Question

What is the concentration of A after 42.9 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

What is the concentration of A after 50.5 minutes for the second order reaction A →...

What is the concentration of A after 50.5 minutes for the second order reaction A → Products when the initial concentration of A is 0.250 M? (k = 0.117 M⁻¹min⁻¹)
What is the concentration of A for a 1st order reaction after 3.00 minutes where the...

What is the concentration of A for a 1st order reaction after 3.00 minutes where the initial concentration of A is 0.614 M and k = 0.000165/s. A 0.982 M B 0.613 M C 0.596 M D 0.573 M
[time] [Z] 4. Suppose the data shown are for the second order reaction: → products. What...

[time] [Z] 4. Suppose the data shown are for the second order reaction: → products. What is the value of the rate constant k? O min 50.000 atm 6.250 3.333 2.273. 5. For a first order reaction (G - products) with k = 0.173 min', suppose a chemist runs the reaction starting with an initial concentration [G]. = 12.0 M. a. How many minutes will it take for [G] to decrease to 4.70 M? b. What [G] will remain after...

8. In the reaction A products the initial concentration of A is 0.52M and the concentration...

8. In the reaction A products the initial concentration of A is 0.52M and the concentration is 0.12 M after 150.0 min. What is the value of the rate constant, k, in M min'? What is the half-life? k=0.0027 M min"!, t12=97.5 min 9. Consider the following reaction: N2(g) + 3H2(g) + 2NH3(g) (K = 2.41x 10-3) Given 2.00 mole of N2(g), 4.5 mole of H2(g), and 1.5 mole of NH3(g) are mixed in a 5.00 L flask, determine the...
What is the concentration of a reactant after 30 minutes, given the initial concentration is 0.10M....

What is the concentration of a reactant after 30 minutes, given the initial concentration is 0.10M. The reaction is a first order reaction with a half-life of 75 minutes.
Consider the reaction A ⟶ Products. The rate law for this reaction is rate = k[A]...

Consider the reaction A ⟶ Products. The rate law for this reaction is rate = k[A] where k= 3.00 X × 10-3 s-1 at a particular temperature. If the initial [A] = 0.500 M, what will be the concentration of A after 2.00 minutes

1. The rate constant for a certain reaction is k = 5.70×10−3 s−1 . If the...

1. The rate constant for a certain reaction is k = 5.70×10−3 s−1 . If the initial reactant concentration was 0.750 M, what will the concentration be after 13.0 minutes? 2. A zero-order reaction has a constant rate of 4.40×10−4 M/s. If after 80.0 seconds the concentration has dropped to 1.00×10−2 M, what was the initial concentration?
The concentration of NO2NO2 was 0.00100 M after 30.0 minutes, and the rate constant for this...

The concentration of NO2NO2 was 0.00100 M after 30.0 minutes, and the rate constant for this reaction at this specific temperature was determined to be 0.543 M−1−1 s−1−1. What was the initial concentration of NO2NO2 ?
A first order reaction (A—>B) has a half-life if 30 minutes. If the initial concentration of...

A first order reaction (A—>B) has a half-life if 30 minutes. If the initial concentration of A is 0.900 M, what is the concentration of B after 60 minutes?

11 of 15 For a starting concentration of 1.0 M, the concentration after an hour for...

11 of 15 For a starting concentration of 1.0 M, the concentration after an hour for a first-order reaction where k=1.5x10-35-1 would be O 0.0045 M 04.0x10-6 M O 0.99 M O 0.00 M 12 of 15 What is the concentration of a reactant for a second-order reaction after 5 minutes where k=2.5x10-3Ms-2 if the initial concentration was 0.10 M? O 0.099 M O 0.0025 M O 0.013 M O 0.093 M