500 grams of C2H10 > grams of H2O

Question

i need the answer to this its was last night homework.

Answer 1

To determine how many grams of H₂O can be produced from 500 grams of C₂H₁₀ (ethane), we first need to consider the balanced chemical equation for the combustion of ethane:

C2H10+192O2→2CO2+5H2OC2​H10​+219​O2​→2CO2​+5H2​O

From the balanced equation, we see that 1 mole of C₂H₁₀ produces 5 moles of H₂O.

Next, we need to calculate the molar masses:

Molar mass of C₂H₁₀ (ethane): 2×12.01+10×1.01=24.02+10.10=34.12 g/mol2×12.01+10×1.01=24.02+10.10=34.12 g/mol

Molar mass of H₂O: 2×1.01+16.00=18.02 g/mol2×1.01+16.00=18.02 g/mol

Now we can find the number of moles of C₂H₁₀ in 500 grams:

Moles of C2H10=500 g34.12 g/mol≈14.65 molesMoles of C2​H10​=34.12 g/mol500 g​≈14.65 moles

Since 1 mole of C₂H₁₀ produces 5 moles of H₂O, 14.65 moles of C₂H₁₀ will produce:

14.65 moles of C2H10×5=73.25 moles of H2O14.65 moles of C2​H10​×5=73.25 moles of H2​O

Finally, converting moles of H₂O to grams:

73.25 moles of H2O×18.02 g/mol=1319.57 g of H2O73.25 moles of H2​O×18.02 g/mol=1319.57 g of H2​O

Therefore, 500 grams of C₂H₁₀ can produce approximately 1319.57 grams of H₂O.