Question

365g of hydrochloric acid reacts with 230g of sodium metal in a controlled environment. Calculate the number of moles and volume of hydrogen gas liberated at STP.​



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Answer 1

Answer:

This is a “single state” problem, so we can solve it using the ideal gas law, PV = nRT. In order to find the volume of hydrogen gas (V), we need to know the number of moles of hydrogen that will be produced by the reaction. Our stoichiometry is simply one mole of hydrogen per mole of zinc, so we need to know the number of moles of zinc that are present in 5.98 grams of zinc metal. The temperature is given in centigrade, so we need to convert into Kelvin, and we also need to convert mm Hg into atm.

Conversions:

25.0C+273=298K(9.6.1)

(742mmHg)×(1atm760mmHg)=0.976atm(9.6.2)

(5.98gZn)×(1.00mol65.39gZn)=0.0915mol(9.6.3)

Substituting:

PV=nRT(9.6.4)

(0.976atm)×V=(0.0915mol)(0.0821Latmmol−1K−1)(298K)(9.6.5)

V=(0.0915mol)(0.0821Latmmol−1K−1)(298K)(0.976atm)=2.29L(9.6.6)