We can identify the limiting reactant by using the stoichiometry (molar ratio) and the mole calculation from reacting masses.The equation below shows the formation of water:2H2(s) + O2(g) → 2H2O(s)There are 8 g of hydrogen (H2) and 128 g of oxygen (O2).Ar(H) = 1 g/mole, Ar(O) = 16 g/molWhich one of the reactants is the limiting?Please name the reactant with word formula (i.e.hydrogen, oxygen.)I DON'T KNOWSUBMIT ANSWER
Question
We can identify the limiting reactant by using the stoichiometry (molar ratio) and the mole calculation from reacting masses.The equation below shows the formation of water:2H2(s) + O2(g) → 2H2O(s)There are 8 g of hydrogen (H2) and 128 g of oxygen (O2).Ar(H) = 1 g/mole, Ar(O) = 16 g/molWhich one of the reactants is the limiting?Please name the reactant with word formula (i.e.hydrogen, oxygen.)I DON'T KNOWSUBMIT ANSWER
Solution
To identify the limiting reactant, we first need to calculate the number of moles for each reactant.
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Calculate the molar mass of each reactant:
- Hydrogen (H2): 2 * Ar(H) = 2 * 1 g/mol = 2 g/mol
- Oxygen (O2): 2 * Ar(O) = 2 * 16 g/mol = 32 g/mol
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Calculate the number of moles for each reactant:
- Hydrogen: 8 g / 2 g/mol = 4 moles
- Oxygen: 128 g / 32 g/mol = 4 moles
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Compare the mole ratio of the reactants with the stoichiometry of the reaction:
- The reaction requires 2 moles of hydrogen for every 1 mole of oxygen. We have 4 moles of each, so we have twice as much hydrogen as we need.
Therefore, oxygen is the limiting reactant.
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