.72 (mol/L)/s
24
24 (mol/L)/s
0.72 (mol/L)/s
The reaction rate would decrease
It is multiplied by 2 if the intermediate reaction is multiplied by 2
24
Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.
.72
24 (mol/L)/s
0.72 (mol/L)/s
24 (mol/L)s
0.4 (mol/L)/s
Rate = k[A]2[B]0
It is multiplied by 2 if the intermediate reaction is multiplied by 2
the answer is rate
The reaction rate would decrease
2 fast rates of reaction