Acetylene (ethyne) gas reacts with oxygen and burns at 3300 C in an acetylene to

Question

Acetylene (ethyne) gas reacts with oxygen and burns at 3300 C in an acetylene torch.

Part A) Write the balanced equation for the complete combustion of acetylene. Express your answer as a chemical equation. Identify all of the phases in your answer.

Part B)How many grams of oxygen are needed to react with 8.5 L of acetylene gas at STP? Express your answer to two significant figures and include the appropriate units.

PartC) How many liters of CO2 gas at STP are produced when 33.0 g of acetylene undergoes combustion? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

C2H2 + O2 --> CO2 + H2O

balanced:

C2H2(g) + 5/2O2(g) --> 2CO2(g) + H2O(g)

b)

m of O2 if

V = 8.5 L at STP

recall that 22.4 L per mol; therefore 8.5/22.4 = 0.3795 mol of C2H2 present

the ratio is: 1 mol of C2H2 per 5 mol of O2

there we need 0.3795 *5 = 1.897 mol of O2

mass = mol*MW = 1.897¨32 = 60.72 g of O2

c)

liters of CO2 if m = 33 g of acetlyen undergoe combustion

MW C2H2 = 26 g/mol

mol = 33/26 = 1.27 mol of C2H4

ratio is 1 mol of C2H4 per 2 mol of CO2, therefore 1.27*2 = 2.538 mol of CO2 will be produced

recall that 1 mol --> 22.4 liter at STP

therefore

2.538 mol * 22.4 = 56.86 Liter of CO2

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