A 1.50 g sample of zinc pellets is poured into 25.0 mL of 2.00 M hydrochloric acid in…
CHEMISTRY · Multi-part · A Level · Chemistry · Amount of substance · Amount of substance
Problem
A 1.50 g sample of zinc pellets is poured into 25.0 mL of 2.00 M hydrochloric acid in a flask connected to an inverted graduated gas-collection tube. The hydrogen gas produced is collected over water at 25 °C. The barometric pressure in the laboratory is 755 mmHg, and the vapor pressure of water at 25 °C is 23.8 mmHg. Assume all reaction products remain in the flask except the hydrogen gas and that the temperature is constant throughout the experiment.
(1) Write the balanced chemical equation for the reaction that occurs.
(2) Determine the limiting reactant and calculate the number of moles of hydrogen gas generated.
(3) Using the laboratory data, calculate the partial pressure of the dry hydrogen gas in the collection tube.
(4) Calculate the volume, in milliliters, of the dry hydrogen gas collected at 25 °C.