🤓 Based on our data, we think this question is relevant for Professor Panapitiya's class at UTD.

(A) Balanced Equation:

**2 C _{2}H_{2} + 5 O_{2} → 4 CO_{2 }+ 2 H_{2}O**

(B) How many grams of water can be formed from the consumption of 8.98 grams of acetylene

Molar mass H_{2}O = 18.02 g/mol

Molar mass C_{2}H_{2} = 26.04 g/mol

$\mathbf{8}\mathbf{.}\mathbf{98}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{2}}}\mathbf{}\mathbf{\times}\mathbf{}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{2}}}}{\mathbf{}\mathbf{26}\mathbf{.}\mathbf{04}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}}{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{18}\mathbf{.}\mathbf{02}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}{\mathbf{1}\mathbf{}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}}$

**= 6.21 g H _{2}O**

(C) How many grams of water can be formed from the consumption of 4.58 grams of oxygen

Molar mass H_{2}O = 18.02 g/mol

Molar mass O_{2} = 16.00 g/mol

$\mathbf{4}\mathbf{.}\mathbf{58}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}\mathbf{}\mathbf{\times}\mathbf{}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}}{\mathbf{}\mathbf{16}\mathbf{.}\mathbf{00}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}}{\mathbf{5}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}}\mathbf{\times}\frac{\mathbf{18}\mathbf{.}\mathbf{02}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}{\mathbf{1}\mathbf{}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}}$

**= 2.06 g H_{2}O**

When acetylene gas, C_{2}H_{2}, reacts with oxygen gas, the products are carbon dioxide and water.

(A) What is the balanced equation?

(B) How many grams of water can be formed from the consumption of 8.98 grams of acetylene

(C) How many grams of water can be formed from the consumption of 4.58 grams of oxygen

(D) What is the theoretical yield of the reaction

(E) The reaction yielded 1.00g of water. What is the percent yield?

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Our tutors have indicated that to solve this problem you will need to apply the Percent Yield concept. If you need more Percent Yield practice, you can also practice Percent Yield practice problems.

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Based on our data, we think this problem is relevant for Professor Panapitiya's class at UTD.