At $$25$$°C, $$50$$ g of iron reacts with HCI to form $$FeCl2$$ The evolved hydrogen gas expands against a constant pressure of $$1$$ bar. The work done by the gas during this expansion is J. (Round$$ off to the Nearest $$Integer)[Given $$R=8.314dmol$$−$$1K$$−$$1$$ Assume, hydrogen is an ideal gas: [Atomic mass off Fe is $$55.85$$ u]

Question

At $$25$$°C, $$50$$ g of iron reacts with HCI to form $$FeCl2$$ The evolved hydrogen gas expands against a constant pressure of $$1$$ bar. The work done by the gas during this expansion is   J. (Round$$ off to the Nearest $$Integer)[Given $$R=8.314dmol$$−$$1K$$−$$1$$ Assume, hydrogen is an ideal gas: [Atomic mass off Fe is $$55.85$$ u]

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$$T=298K$$,$$R=8.314JmolK$$→ Chemical reaction $$isFe+2HCl$$→$$FeCl2+H2(g)50g$$ $$P=1bar=5055.85mol$$→ Work done for $$1$$ mol $$gas=$$−Pext×Δ$$V=$$Δ$$ngRT=$$−$$1$$×$$8.314$$×$$298J$$→ Work done for $$5055.85mol$$ of $$gas=$$−$$8.314$$×$$298$$×$$5055.85J=$$−$$2218.059J=$$−$$2218J$$

Fundamentals of thermodynamics

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Fundamentals of thermodynamics

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T=298K,R=8.314JmolK→ Chemical reaction isFe+2HCl→FeCl2+H2(g)50g P=1bar=5055.85mol→ Work done for 1 mol gas=−Pext×ΔV=ΔngRT=−1×8.314×298J→ Work done for 5055.85mol of gas=−8.314×298×5055.85J=−2218.059J=−2218J

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