In a first order reaction the a/(a−x) was found to be 8 after 10 minute. The rate constant is:
A(g)→B(g)+C(g)
-d[A]dt=k[A]
At the beginning of this reaction, the pressure is 100 mm Hg. After 10 min, pressure increases to 120 mm Hg. The rate constant (min−1) is:
The activation energy for a reaction at temperature T K was found to be 2.303 RT J mol−1. The ratio of the rate constant to Arrhenius factor is :