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For the following reaction, hydrogen gas is the byproduct of the hydrolysis of water. If there are 2.00 moles of water and 0.25 moles of hydrogen dissolved into the water at equilibrium, what is the concentration of dissolved hydrogen gas?

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General Chemistry 2
Skill
Relate equilibrium concentrations of reactants and products
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Jarrod Robel
Jarrod RobelLv2
1 Sep 2020

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Related questions

(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 × 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)?

1. According to the following reaction, how many moles of hydrogen gas are necessary to form 0.683 moles nitrogen gas?

nitrogen monoxide (g) + hydrogen (g) nitrogen (g) + water (l)

2. According to the following reaction, how many moles of water are necessary to form 0.909 moles zinc hydroxide?

zinc oxide (s) + water (l) ------ zinc hydroxide (aq)

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