Acetaldehyde, CH3CHO, will decompose into methane and carbon monoxide according to
CH3CHO (g) -> CH4 (g) + CO (g)
At 450C the rate of consumption of CH3CHO is measured to vary with the concetration of CH3CHO raised to the power 1.5.
With a CH3CHO concentration of 0.222M, the rate of consumption of CH3CHO at 450C is measured to be 3.33*10-3 M/s. Calculate the rate of production of carbon monoxide when the concentration of CH3CHO has fallen to 0.111M.
Express your answer in M/s:
(1.18)*10^-3
1.18*e-3
Given the rate expression for the decomposition reaction:
Rate = k[CH3CHO]^1.5
We can first find the rate constant (k) by using the initial concentration of CH3CHO and the initial rate of consumption:
[CH3CHO]1 = 0.222 M
Rate1 = 3.33 * 10^-3 M/s
Plugging these values into the rate expression, we get:
3.33 * 10^-3 M/s = k * (0.222 M)^1.5
Now we can solve for k:
k = (3.33 * 10^-3 M/s) / (0.222 M)^1.5
Next, we can use the rate constant to find the rate of production of carbon monoxide when the concentration of CH3CHO has fallen to 0.111 M:
[CH3CHO]2 = 0.111 M
Plugging this concentration into the rate expression, we get:
Rate2 = k * (0.111 M)^1.5
Finally, we can substitute the value of k and calculate the rate:
Rate2 = [(3.33 * 10^-3 M/s) / (0.222 M)^1.5] * (0.111 M)^1.5
Calculating the expression above will give you the rate of production of carbon monoxide (CO) when the concentration of CH3CHO has fallen to 0.111 M.
To calculate the rate of production of carbon monoxide (CO) when the concentration of CH3CHO has fallen to 0.111M, we need to use the given information about the rate and concentration relationship.
First, let's determine the rate law expression for the given reaction:
rate = k * [CH3CHO]^1.5
Now, let's use the initial rate and concentration to determine the rate constant (k).
Given:
Initial concentration of CH3CHO (C1) = 0.222 M
Initial rate (R1) = 3.33 * 10^-3 M/s
Using the rate law expression:
R1 = k * C1^1.5
Substituting the values:
3.33 * 10^-3 = k * (0.222)^1.5
Solving for k:
k = 3.33 * 10^-3 / (0.222)^1.5
Now that we have the rate constant (k), we can calculate the rate of production of carbon monoxide (CO) when the concentration of CH3CHO falls to 0.111M.
Given:
Final concentration of CH3CHO (C2) = 0.111 M
Using the rate law expression:
Rate of production of CO = k * [CH3CHO]^1.5
Substituting the values:
Rate of production of CO = (3.33 * 10^-3 / (0.222)^1.5) * (0.111)^1.5
Calculating this expression will give you the rate of production of carbon monoxide (CO) at 450°C when the concentration of CH3CHO is 0.111M.