(a) A sample of hydrogen gas is generated in a closedcontainer by reacting 2.050 g of zinc metal with 15.0 mLof 1.00 M sulfuric acid. Write the balanced equation forthe reaction, and calculate the number of moles of hydrogenformed, assuming that the reaction is complete.(b) The volume over the solution in the container is 122mL. Calculate the partial pressure of the hydrogen gas inthis volume at 25 °C, ignoring any solubility of the gas inthe solution. (c) The Henry’s law constant for hydrogenin water at 25 °C is 7.8 x 10-4 mol/L-atm. Estimate thenumber of moles of hydrogen gas that remain dissolvedin the solution. What fraction of the gas molecules in thesystem is dissolved in the solution? Was it reasonable toignore any dissolved hydrogen in part (b)?
(a) A sample of hydrogen gas is generated in a closed
container by reacting 2.050 g of zinc metal with 15.0 mL
of 1.00 M sulfuric acid. Write the balanced equation for
the reaction, and calculate the number of moles of hydrogen
formed, assuming that the reaction is complete.
(b) The volume over the solution in the container is 122
mL. Calculate the partial pressure of the hydrogen gas in
this volume at 25 °C, ignoring any solubility of the gas in
the solution. (c) The Henry’s law constant for hydrogen
in water at 25 °C is 7.8 x 10-4 mol/L-atm. Estimate the
number of moles of hydrogen gas that remain dissolved
in the solution. What fraction of the gas molecules in the
system is dissolved in the solution? Was it reasonable to
ignore any dissolved hydrogen in part (b)?
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