# Problem: When acetylene gas, C2H2, 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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###### FREE Expert Solution

(A) Balanced Equation:

2 C2H2 + 5 O2 → 4 CO+ 2 H2O

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

Molar mass H2O = 18.02 g/mol

Molar mass C2H2 = 26.04  g/mol

= 6.21 g H2O

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

Molar mass H2O = 18.02 g/mol

Molar mass O2 = 16.00  g/mol

= 2.06 g H2O ###### Problem Details

When acetylene gas, C2H2, 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?