Hydrogen and oxygen react under a specific
set of conditions to produce water according
to the equation
2 H2(g) + O2(g) −→ 2 H2O(g).
How much hydrogen would be required to
produce 8.3 mol of water?
How much oxygen would be required?
To determine the amount of hydrogen and oxygen required, we need to use the stoichiometry of the reaction.
According to the balanced chemical equation:
2 H2(g) + O2(g) --> 2 H2O(g)
We can see that for every 2 moles of hydrogen gas (H2), 2 moles of water (H2O) are produced. This means that the ratio of hydrogen to water is 2:2, or simply 1:1.
To find the number of moles of hydrogen required to produce 8.3 moles of water, we can use this ratio:
8.3 moles of water * (1 mole of hydrogen / 2 moles of water) = 4.15 moles of hydrogen
Therefore, 4.15 moles of hydrogen would be required to produce 8.3 moles of water.
Similarly, since the ratio of oxygen to water in the balanced equation is also 1:1, the amount of oxygen required would be the same as the amount of hydrogen:
4.15 moles of oxygen would be required to produce 8.3 moles of water.