Question

At \(T\)(K), the following data is obtained for the decomposition of \(A(g)\), which follows first order kinetics \[ A(g)\rightarrow B(g)+C(g) \] \[ \begin{array}{|c|c|} \hline \text{Time (s)} & \text{Total pressure (atm)} \hline 0 & 0.5 100 & 0.6 x & 0.65 \hline \end{array} \] What is \(x\) (in s)? \[ (\log1.25=0.097,\qquad \log1.4285=0.1549) \]

• A. \(180\)
• B. \(160\)
• C. \(140\)
• D. \(200\)

Hint:

For the decomposition \[ \boxed{A\rightarrow B+C,} \] the partial pressure of reactant is \[ \boxed{ P_A=2P_0-P_t. } \] Then use the first-order equation \[ \boxed{ k=\frac{2.303}{t}\log\frac{P_0}{P_A}. } \]

Answer 1

The Correct Option is B