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Solution: The chemical reaction N2(g) + 3H2(g) → 2NH3(g) is carried out below:20.0L N2 5.0L H210.0 atm 5.0 atma. When the stopcock between the two reaction vessels is opened, the reaction proceeds. Calculate the partial pressure of NH3 after the reaction is complete. Assume 100% yield for the reaction and that the temperature is constant.b.What will be the effect on the volume of an ideal gas if both the pressure is increased 10 fold and the absolute temperature is doubled?

Problem

The chemical reaction N2(g) + 3H2(g) → 2NH3(g) is carried out below:

20.0L N2 5.0L H2

10.0 atm 5.0 atm

a. When the stopcock between the two reaction vessels is opened, the reaction proceeds. Calculate the partial pressure of NH3 after the reaction is complete. Assume 100% yield for the reaction and that the temperature is constant.







b.What will be the effect on the volume of an ideal gas if both the pressure is increased 10 fold and the absolute temperature is doubled?