10.8 - 2 Does this answer make sense? According to the...

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Key: 8. What volume of hydrogen gas is required to completely react with 100.0 L of nitrogen gas at STP to yield ammonia? a. 100.0 L b. 200.0 L c. 300.0 L d. 275.0 L e. 345.0 L f. 456.0 L g. 580.0 L Remember, to completely react, you need the correct stoichiometric ratio of reactants together. This requires a balanced equation: 3 H 2 + N 2 → 2NH 3 Think of a scheme that will get you where you need to go, starting with what you have: Volume nitrogen gas→moles nitrogen gas→moles hydrogen gas→volume hydrogen gas. 100.0L N 2 │1mol N 2 │3 mol H 2 │22.4L H 2 = 300L H 2 │22.4L N 2 │ 1mol N 2 │1 mol H
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Unformatted text preview: 2 Does this answer make sense? According to the balanced equation, you need three times as much H 2 as N 2 . Since you started with 100L N 2, you would need 300L H 2 to fully react. And since the same volume of any two gases at the same T and P contain the same number of molecules, it makes sense that you need thrice the volume of nitrogen. Remember that 1 mol of gas at STP = 22.4L. If you forget this, you can always plug in the standard temperature and pressure conditions (273K, and 1atm) into the ideal gas equation(PV = nRT)....
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