Decomposition of both A2(g) and B3(g) follows 1st order kinetics as:A2(g)k1−→2A(g) k1(hr−1)=102e−14000RTB3(g)k2−→3B(g) k2(hr−1)=103e−20000RTIf 1 mol of A2(g) and B3(g) are taken in a 10 L evacuated flask and heated to some temperature so that they start decomposing at the same rate, determine total pressure (in atm) in the flask after 1.0 hr.

Decomposition of both A2(g) and B3(g) follows 1st order kinetics as:A2

1.	Decomposition of both A2(g) and B3(g) follows 1st order kinetics as:A2(g)k1−→2A(g) k1(hr−1)=102e−14000RTB3(g)k2−→3B(g) k2(hr−1)=103e−20000RTIf 1 mol of A2(g) and B3(g) are taken in a 10 L evacuated flask and heated to some temperature so that they start decomposing at the same rate, determine total pressure (in atm) in the flask after 1.0 hr.
Answer» Decomposition of both $A_{2} (g)$ and $B_{3} (g)$ follows $1^{s t}$ order kinetics as: $A_{2} (g) k_{1} - \to 2 A (g) k_{1} (h r^{- 1}) = 10^{2} e^{- \frac{14000}{R T}}$ $B_{3} (g) k_{2} - \to 3 B (g) k_{2} (h r^{- 1}) = 10^{3} e^{- \frac{20000}{R T}}$ If $1 m o l$ of $A_{2} (g)$ and $B_{3} (g)$ are taken in a $10 L$ evacuated flask and heated to some temperature so that they start decomposing at the same rate, determine total pressure (in $a t m$ ) in the flask after $1.0 h r$ .