A first-order reaction without catalyst gives $12.0%$ conversion in $2.00 h$ . A catalyst raises the rate constant $25$ -fold. What percent conversion is reached in $2.00 h$ with the catalyst? Give one decimal. (Use $ln 0.88 = - 0.1278$ if needed.)

Numerical answer type, answer in %, tolerance 0.1.

Answer: 95.9 %

Without catalyst

k t = - ln 0.88 = 0.1278

. With catalyst

k t = 25 \times 0.1278 = 3.195

. The fraction left is

e^{- 3.195} = 0.0410

, so conversion is 95.9\%.