Question

Calculate the work done in the following reaction at \(300\ \text{K}\),
\(\text{A}(g)+\text{B}(g)=2\text{C}(g)\)   \([R=8.314\ \text{JK}^{-1}\text{mol}^{-1}]\)

• A. \(2.494\ \text{kJ}\)
• B. \(4.988\ \text{kJ}\)
• C. \(0\ \text{kJ}\)
• D. \(-2.494\ \text{kJ}\)

Hint:

Work at constant pressure depends on the change in the number of moles of gas.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept
For a reaction involving gases at constant pressure, \(w = -\Delta n_g RT\).

Step 2: Find the change in moles of gas
The reaction is \(\text{A}(g)+\text{B}(g)=2\text{C}(g)\). \(\Delta n_g = 2-(1+1) = 0\).

Step 3: Work done
\(w = -0\times 8.314\times 300 = 0\).

Step 4: Compare the options
The work done is \(0\ \text{kJ}\).

Final Answer:
The work done is zero. \[ \boxed{\text{(C) }0\ \text{kJ}} \]