When the chemical reaction 3H_2(g) + 2(g) rightarrow 2NH_3 (g) is run in a 1.0-L

Question

When the chemical reaction 3H_2(g) + 2(g) rightarrow 2NH_3 (g) is run in a 1.0-L vessel with a movable piston (assume perfectly stoichiometry amounts of hydrogen and nitrogen gasses), what will the value of w be? More information is needed to calculate the value, but we know w will be 0 J About + 50 kJ About - 50 kJ About + 0.5 J Consider the case of the same reaction of problem 16 being instead run in a closed rigid vessel. The internal and external pressures are initially both 1.00 atm, the temperature is kept constant at 300 degree C and the volume of the vessel is 10.0 L. What is the value of w, assuming 100 % of yield?

Explanation / Answer

16.

Work done due to gas produced or consumed in a chemical reaction is given by=-nRT

Where n=number of moles of gaseous products-number of moles of gaseous reactants=2-4=-2

R=universal gas constant, T=temperature

So given information is insufficient to calculate magnitude of w but we can say that w would be positive as n is negative.

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