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ng.cengage.com Mail braulio cunha1@hotmail.com Cengage MindTap - Cengage Learning MINDTAP Braulio Cunha -L 14 Challenge Due Tomorrow at 8 AM CST Late Submission until Feb 14 at 8 AM CST is allowed, with a one time 10% penalty to subrmitted score. Use the References to access important values if needed for this question. The rate constant of the elementary reaction HCOOH(g) (g) +H2g) is k 2.05x105 s1 at 476°C, and the reaction has an activation energy of 203 kJ mol1 (a) Compute the rate constant of the reaction at a tempcrature of 778°C. b) At a temperature of 476 3.58x104 s is required for half of the HCOOH originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 778°C? A-Z Submit Answer 3 question attempts remaining Current score: 1012 pts (83.33 %)Explanation / Answer
a) Arrhenius equation
ln(K2/k1) = Ea/R[1/T1 - 1/T2]
k1 = 2.05*10^-5 s-1 , T1 = 476+273.15 = 749.15 k
k2 = x s-1 , T2 = 778+273.15 = 1051.15 k
Ea = 203 kj/mol , R = 8.314*10^-3 j.k-1.mol-1
ln(x/(8.33*10^-6)) = ((203*10^3)/(8.314))((1/749.15)-(1/1051.15)
K2 = 0.097 S-1
b) it is a first order kinetics,
k = 0.693/T1/2
at = 778 c , K = 0.097 s-1
(0.097) = (0.693/x)
x = T1/2 = half-life time = 7.14 sec
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