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Determine the mass of co2 and the mass of h2o produced by the combustion of 1.15 g of a compound with the empirical formula ch4o.

Respuesta :

W0lf93
CO2 = 1.580 grams H2O = 0.592 grams Lookup the molar mass of each element in the compound Carbon = 12.0107 Hydrogen = 1.00794 Oxygen = 15.999 Calculate the molar mass of CH4O by adding the total masses of each element used. 12.0107 + 4 * 1.00794 + 15.999 = 32.04146 Now calculate how many moles of CH4O you have by dividing by the molar mass. m = 1.15 g / 32.04146 g/mole = 0.035891 mole Now figure out how many moles of carbon and hydrogen you have. Carbon = 0.035891 moles Hydrogen = 0.035891 moles * 4 = 0.143564 moles For Carbon Dioxide, you need 2 moles of oxygen per mole of carbon. So the mass of the carbon dioxide will be 0.035891 * 12.0107 + 2 * 0.035891 * 15.999 = 1.579516 grams For water, you need 1/2 mole of oxygen per mole of hydrogen. So the mass of H2o will be 0.035891 * 1.00794 / 2 + 0.035891 * 15.999 = 0.592308 grams
Dejanras

1) The answer is: the mass of CO₂ is 1.58 grams and the mass H₂O of is 1.296 grams.

Balanced chemical reaction: CH₄O + 1.5O₂ → CO₂ + 2H₂O.

m(CH₄O) = 1.15 g; mass of organic compound.

n(CH₄O) = m(CH₄O) ÷ M(CH₄O).

n(CH₄O) = 1.15 g ÷ 32 g/mol.

n(CH₄O) = 0.036 mol.

2) From chemical reaction: n(CH₄O) : n(CO₂) = 1 : 1.

n(CO₂) = 0.036 mol; amount of carbon dioxide.

M(CO₂) = 44 g/mol; molar mass of carbon dioxide.

m(CO₂) = n(CO₂) · M(CO₂).

m(CO₂) = 0.036 mol · 44 g/mol.

m(CO₂) = 1.58 g; mass of carbon dioxide.

From chemical reaction: n(CH₄O) : n(H₂O) = 1 : 2.

n(H₂O) = 2 · 0.036 mol.

n(H₂O) = 0.072 mol; amount of water.

M(H₂O) = 18 g/mol; molar mass of water.

m(H₂O) = n(H₂O) · M(H₂O).

m(H₂O) = 0.072 mol · 18 g/mol.

m(H₂O) = 1.296 g; mass of water.

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