Question

( begin{array}{l}text { Asherius reaction for the same } text { reachion at tur diffecent temerat } text { log }left(frac{k_{2}}{k_{1}}right)=frac{E_{a}}{2 cdot 303 R}left(frac{1}{T_{1}}-frac{1}{7_{2}}right) text { Log }left(frac{k_{2}}{k_{1}}right)=frac{105.70 times 10^{3}}{2.303 times 8.314}left(frac{1}{313}-frac{1}{353}right. {40+273=313 k text { and } 80+273=3530 text { log } frac{k_{2}}{k_{1}}=2 frac{k_{2}}{k_{1}}=text { antilog } 2 k_{2}=100 = & 100 times 0.133 = & 13.3 mathrm{moP} / mathrm{l} / text { min }end{array} )

# temperature At 40°C, the Product is 105.73 kJ mol mint What will be the rate of formation of B The activation energy of the reaction: A products are formed at the rate of 0.133 mol products at 80°C? constant for the reaction

Solution