Question

calculate the work done in open vessel at 27 degree Celsius when 28g Fe reacts with h2SO4

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Answer 1

Explanation:

The reaction involved is:

Fe+2HCl→FeCl

2

+H

2

Atomic mass of Fe=56g/mol

Thus, 56 g of Iron reacts with 2 moles of HCl to give one mole of Hydrogen gas.

Initial volume of H

2

gas = V

1

=0

Final volume of H

2

gas=V

2

Using ideal gas law:PV=nRT

where n=mass/molar mass, R=8314 J/K/mol and given that T=300 K

PV

2

=(112/56)×8.314×300=4988.4J

Work done =−PΔV=−P(V

2

−V

1

)=−PV

2

=−4988.4J

negative work done is work of expansion.

since 4184 J=1 kcal

thus 4988.4J=1.19kcal of work is done by the system.

Answer 2

Answer:

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