1) A particular first-order reaction has a rate constant of 1.35×10^2 /s at 25.0^∘C. What is the

Here they provide a proposed mechanism for the decomposition of ozone. The first step is ozone,

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1) A particular first-order reaction has a rate constant of 1.35\times 10^2 /s at 25.0$^\circ$C. What is the magnitude of $k$ at 75.0$^\circ$C if $E_a$ = 85.6 kJ/mol? 2) The decomposition of ozone, O$_3$, is believed to occur by a two-step mechanism: $\bullet$Write the equation for the overall reaction. $\bullet$Write the rate law for the overall reaction. step 1: O$_3 \rightarrow$ O$_2$ + O step 2: O$_3$ + O $\rightarrow$ 2O$_2$ Slow Fast 3) Write the equilibrium constant expression in terms of concentrations SO$_2$Cl$_2$(s) $\rightleftharpoons$ SO$_2$(g) + Cl$_2$(g)

          1) A particular first-order reaction has a rate constant of 1.35\times 10^2 /s at 25.0$^\circ$C. What is the magnitude of $k$ at 75.0$^\circ$C if $E_a$ = 85.6 kJ/mol?
2) The decomposition of ozone, O$_3$, is believed to occur by a two-step mechanism:
$\bullet$Write the equation for the overall reaction.
$\bullet$Write the rate law for the overall reaction.
step 1: O$_3 \rightarrow$ O$_2$ + O
 step 2: O$_3$ + O $\rightarrow$ 2O$_2$
Slow
Fast
3) Write the equilibrium constant expression in terms of concentrations
SO$_2$Cl$_2$(s) $\rightleftharpoons$ SO$_2$(g) + Cl$_2$(g)

1) A particular first-order reaction has a rate constant of 1.35×10^2 /s at 25.0^∘C. What is the magnitude of k at 75.0^∘C if Ea = 85.6 kJ/mol?
2) The decomposition of ozone, O3, is believed to occur by a two-step mechanism:
∙Write the equation for the overall reaction.
∙Write the rate law for the overall reaction.
step 1: O3 → O2 + O
step 2: O3 + O → 2O2
Slow
Fast
3) Write the equilibrium constant expression in terms of concentrations
SO2Cl2(s) ⇌ SO2(g) + Cl2(g)

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