The gaseous hydrocarbon acetylene, C 2 H 2 , used in welders\' torches, releases

Question

The gaseous hydrocarbon acetylene, C2H2, used in welders' torches, releases a large amount of heat when it burns according to the following equation:
2C2H2(g)+5O2(g)??4CO2(g)+2H2O(g)

1. How many moles of water are produced from the complete reaction of 4.00 moles of oxygen?

2. How many grams of oxygen are needed to react completely with 2.20g of acetylene?

3.How many grams of carbon dioxide are produced from the complete reaction of 78.0

g of acetylene?

4.If the reaction in Part C produces 182

g of CO2, what is the percent yield of CO2 for the reaction?

Explanation / Answer

2C2H2(g)+5O2(g) ------ > 4CO2(g)+2H2O(g)

(2*26)       (5*32)                (4*44 )        (2*18)

1) 5 moles of O2 produces 2 moles of H2O

      4 moles of O2 produces = (2/5)*4 = 1.6 moles of H2O

2) (2*26)52 g   C2H2 reacts with (5*32) 160 g of O2

      2.20g C2H2 reacts =(160/52)*2.2 = 6.77 g of O2

3) 52 g   C2H2 forms (4*44) 176 g of CO2

    78.0 C2H2 forms =(176/52)*78 = 264 g of CO2

4)percent yield of CO2=( actual formed of CO2/ theoritical formed of CO2)*100

                                    = (182/264)*100

                                    =68.94 %

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