To answer this question, we need to use stoichiometry and the balanced chemical equation for the reaction between carbon monoxide (CO) and hydrogen gas (H2) to determine the ratio of moles of CO to moles of H2. Then, we can use the given volume of CO to calculate the volume of H2.
The balanced chemical equation for the reaction between CO and H2 is:
CO + 3H2 -> CH4 + H2O
From this equation, we see that 1 mole of CO reacts with 3 moles of H2.
Given that we have 2.27 liters of CO, we need to convert this volume to moles using the ideal gas law, assuming standard temperature and pressure (STP), which is 1 mole of gas occupies 22.7 liters at STP.
Number of moles of CO = Volume of CO (in liters) / Molar volume at STP
= 2.27 liters / 22.7 liters/mole
≈ 0.1 moles of CO
Now, using the stoichiometric ratio from the balanced equation, we find the number of moles of H2 needed:
Number of moles of H2 = 0.1 moles of CO * (3 moles of H2 / 1 mole of CO)
= 0.1 * 3
= 0.3 moles of H2
Finally, we convert the moles of H2 to volume at STP:
Volume of H2 = Number of moles of H2 * Molar volume at STP
= 0.3 moles * 22.7 liters/mole
≈ 6.81 liters of H2
Therefore, if 2.27 liters of CO are used, approximately 6.81 liters of H2 are also consumed in the reaction.
