Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g)
6. A student performs an experiment to determine the volume of hydrogen gas produced when a given mass of zinc reacts with excess HCl(aq), as represented by the net ionic equation above. The student begins with a 0.0580 g sample of pure zinc and a solution of 3.0 M HCl(aq).
Calculate the number of moles of zinc in the 0.0580 g sample.
As the zinc reacts, an equal number of moles of hydrogen gas is produced and collected by water displacement at 23.0°C. The pressure of the gas in the collection tube is measured to be 775 torr.
Given that the equilibrium vapor pressure of water is 21 torr at 23.0°C, calculate the pressure of the H2(g) produced in the reaction.
Calculate the volume, in liters, that the H2(g) produced in the reaction would have.
If the temperature of the hydrogen gas sample was increased, but the pressure remained constant, how would the volume change? Justify your answer.