Question

The rate constant of the elementary reaction C$_2$H$_5$Cl(g) → C$_2$H$_4$(g) + HCl(g) is $k = 7.28 \times 10^{-5} s^{-1}$ at 428 °C, and the reaction has an activation energy of 237 kJ/mol. Compute the rate constant of the reaction at a temperature of 465 °C. $k = \boxed{}$ s$^{-1}$ At a temperature of 428 °C, 9.52 x 10$^3$ s is required for half of the C$_2$H$_5$Cl originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 465 °C? $t = \boxed{}$ s

          The rate constant of the elementary reaction
C$_2$H$_5$Cl(g) → C$_2$H$_4$(g) + HCl(g)
is $k = 7.28 \times 10^{-5} s^{-1}$ at 428 °C, and the reaction has an activation energy of 237 kJ/mol.
Compute the rate constant of the reaction at a temperature of 465 °C.
$k = \boxed{}$ s$^{-1}$
At a temperature of 428 °C, 9.52 x 10$^3$ s is required for half of the C$_2$H$_5$Cl originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 465 °C?
$t = \boxed{}$ s

the rate constant of the elementary reaction c2h5clg c2h4g hclg is k 728 times 10 5 s 1 at 428 c and the reaction has an activation energy of 237 kjmol compute the rate constant of the r 00243

Added by Julia S.

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