Consider the following reaction
2 N2O(g)--2NO(g)+ O2(g); rate = K[N2O]
If the half life for the reaction is 0.910 s,what is the rate constant
The half-life for a first-order reaction is given by the equation:
t1/2 = ln(2) / k
where t1/2 is the half-life and k is the rate constant.
Rearranging this equation gives:
k = ln(2) / t1/2
Substituting the given half-life of 0.910 s, we get:
k = ln(2) / 0.910 s ≈ 0.762 s^-1
Therefore, the rate constant for the reaction is approximately 0.762 s^-1.
To determine the rate constant (k) for a reaction, we can use the half-life (t½) and the following equation:
t½ = 0.693 / k
Given that the half-life (t½) for the reaction is 0.910 seconds, we can rearrange the equation to solve for the rate constant (k):
k = 0.693 / t½
Substituting the given value:
k = 0.693 / 0.910
Calculating the value:
k ≈ 0.76 s⁻¹
Therefore, the rate constant (k) for the reaction is approximately 0.76 s⁻¹.
To find the rate constant for the given reaction, we can use the equation for the half-life of a first-order reaction:
t(1/2) = 0.693 / k
Given that the half-life (t(1/2)) is 0.910 s, we can rearrange the equation to solve for the rate constant (k):
k = 0.693 / t(1/2)
Plugging in the given value:
k = 0.693 / 0.910
k ≈ 0.76 s^(-1)
Therefore, the rate constant for the reaction is approximately 0.76 s^(-1).