At s.t.p, a mole of chlorine occupies 22.4dm3. If the temperature is changed to 35°C and the pressure to 750mHg the of the new volume will be [Cl = 35.5]
- \(\frac{760\times 22.4\times 308}{750\times 273\times 35.5} dm^3 \)
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\(\frac{760\times 22.4\times 308}{750\times 273}dm^3 \)
- \(\frac{750\times 22.4\times 35.5}{760\times 273}dm^3\)
- \(\frac{760\times 22.4\times 35.5}{750\times 22.3\times 273}dm^3 \)
- \(\frac{760\times 22.4\times 35.5}{750\times 308}dm^3 \)
The correct answer is: B
Explanation
Using the general gas law, \(\frac{P_1 \times V_1}{T_1}\) = \(\frac{P_2 \times V_2}{T_2}\)
At STP, P1 = 760mmHg, V1 = 22.4dm3, T1 = 273K, P2 = 750mmHg, V2 = ? and T2 = 350C = 35 + 273 = 308K
making \(V_2\) subject of formula, then \(V_2\) = \(\frac{P_1\times V_1\times T_2}{P_2\times T_1}\)
\(V_2\) = \(\frac{760\times 22.4\times 308}{750\times 273}\)