Multiple Choice
In the reaction 3 N2H4(l) -> 4 NH3(g) + N2(g), how many moles of N2H4 are required to produce 2.39 moles of NH3?
3. Chemical Reactions
Stoichiometry
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A mixture of 1.88 moles of hydrogen and 0.92 moles of oxygen are used in the reaction. According to the balanced chemical equation 2H₂ + O₂ → 2H₂O, how many moles of water would be produced if you used up all the hydrogen?
A
3.76 moles
B
1.88 moles
C
0.46 moles
D
0.92 moles
Verified step by step guidance1
Identify the balanced chemical equation for the reaction: 2H₂ + O₂ → 2H₂O. This equation tells us that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water.
Determine the limiting reactant. Since we have 1.88 moles of hydrogen and 0.92 moles of oxygen, we need to check which reactant will be completely consumed first. According to the stoichiometry of the reaction, 2 moles of H₂ are needed for every 1 mole of O₂.
Calculate the amount of hydrogen needed to react with the available oxygen. Since we have 0.92 moles of O₂, we need 2 × 0.92 = 1.84 moles of H₂ to completely react with the oxygen.
Compare the available moles of hydrogen (1.88 moles) with the required moles (1.84 moles). Since 1.88 moles of H₂ is more than 1.84 moles, hydrogen is in excess, and oxygen is the limiting reactant.
Use the stoichiometry of the reaction to determine the moles of water produced. Since 2 moles of H₂ produce 2 moles of H₂O, the moles of water produced will be equal to the moles of hydrogen used, which is 1.88 moles.
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