The work done by the gas liberated when 50 g of iron (molar mass 55.85 g mol -1 ) reacts with hydrochloric acid in an open beaker at 25° C

Question

The work done by the gas liberated when 50 g of iron (molar mass 55.85 g mol -1 ) reacts with hydrochloric acid in an open beaker at 25° C (A) zero (B) - 2.3 kJ (C) 2.2 kJ (D) 0.22 kJ

Tardigrade Admin · Accepted Answer

underset55.85 gFe (s)+2 HCl ( aq ) arrow FeCl 2( aq )+ underset1 mol H 2( g ) n=(50/55.85)=0.895 mol W=-n R T-0.895 × 8.314 × 10-3 × 298 =-2217.42 × 10-3=-2.2 kJ

Q. The work done by the gas liberated when $50 g$ of iron (molar mass $55.85 g m o l^{- 1}$ ) reacts with hydrochloric acid in an open beaker at $2 5^{\circ} C$

zero

- 2.3 kJ

2.2 kJ

0.22 kJ

$55.85 g F e (s) + 2 H Cl (a q) \to F e C l_{2} (a q) + 1 m o l H_{2} (g)$
$n = \frac{50}{55.85} = 0.895 m o l$
$W = - n RT - 0.895 \times 8.314 \times 1 0^{- 3} \times 298$
$= - 2217.42 \times 1 0^{- 3} = - 2.2 k J$

Q. The work done by the gas liberated when 50g of iron (molar mass 55.85gmol−1 ) reacts with hydrochloric acid in an open beaker at 25∘C