A sample of hydrogen gas is generated in a closed container by reacting 2.050 g of zinc metal with 12.0 mL of 1.00 M sulfuric acid. Write the balanced equation for the reaction.
Calculate the number of moles of hydrogen formed, assuming that the reaction is complete.
The volume over the solution is 121 mL. Calculate the partial pressure of the hydrogen gas in this volume at 25 C, ignoring any solubility of the gas in the solution.
The Henry's law constant for hydrogen in water at 25 C is 7.8 \times 10^ 4 mol/L *atm. Estimate the number of moles of hydrogen gas that remain dissolved in the solution.