How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 76.6 moles of water vapor?
Are you sure it is CO2 and not CO?
To answer this question, we need to use the balanced chemical equation for the reaction between hydrogen gas and carbon dioxide to produce water vapor:
CO2 + 4H2 → CH4 + 2H2O
From the equation, we can see that 4 moles of hydrogen gas react with 1 mole of carbon dioxide to produce 2 moles of water vapor.
This means that the mole ratio of hydrogen to water vapor is 4:2, or simplifying it, 2:1.
Since we are given the number of moles of water vapor (76.6 moles), we can use the mole ratio to determine the number of moles of hydrogen gas needed.
We can set up a proportion using the mole ratio:
2 moles of water vapor / 1 mole of hydrogen gas = 76.6 moles of water vapor / x moles of hydrogen gas
Cross-multiplying and solving for x, we get:
2x = 76.6
Dividing both sides by 2, we find:
x = 38.3
So, 38.3 moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 76.6 moles of water vapor.