If sodium peroxide is added to water, elemental oxygen gas is generated: Na2O2(s) + H2O(l) → NaOH(aq) + O2(g) Suppose 1.15 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced in grams?

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First balance the equation to find that so the moles of ##O_2## released is equal to one-half the moles of ##Na_2O_2## added: ##2 Na_2O_2 + 2 H_2O rarr 4 NaOH + O_2##

The molar mass of ##Na_2O_2## is 77.98 g/mol, so the moles of ##Na_2O_2## is ##(1.15g)/(77.98 g/(mol))=0.01456## mol (carries 1 extra sig fig for intermediate calculation)

The molar mass of ##O_2## is 32.00 g/mol, so the mass of ##O_2## released is ##1/2 times 0.01456 mol times 32.00 g/(mol)=0.233##g

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If sodium peroxide is added to water, elemental oxygen gas is generated: Na2O2(s) + H2O(l) → NaOH(aq) + O2(g) Suppose 1.15 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced in grams?

Leave a Comment / Uncategorized

First balance the equation to find that so the moles of ##O_2## released is equal to one-half the moles of ##Na_2O_2## added: ##2 Na_2O_2 + 2 H_2O rarr 4 NaOH + O_2##

The molar mass of ##Na_2O_2## is 77.98 g/mol, so the moles of ##Na_2O_2## is ##(1.15g)/(77.98 g/(mol))=0.01456## mol (carries 1 extra sig fig for intermediate calculation)

The molar mass of ##O_2## is 32.00 g/mol, so the mass of ##O_2## released is ##1/2 times 0.01456 mol times 32.00 g/(mol)=0.233##g

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