Based on C2H4 + 3 O2 = 2 CO2 + 2 H2O
how many moles of O2 are required for the complete combustion of 45 g of C2H4?
if 14.0 g of C2H4 are reacted and the actual yield of H2O is 7.84 g, what is the percent yield of water in the reaction?
if 18.0 g of CO2 are produced, how many grams of H2O are produced?
Answers: 3
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4.25g sample of solid ammonium nitrate dissolves in 60.0g of water in a coffee-cup calorimeter, the temperature drops from 22.0 c to 16.9 c. assume that the specific heat of the solution is the same as that of pure water. calculate delta(h) (in kj/mol nh4no3) for the solution proces.
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Based on C2H4 + 3 O2 = 2 CO2 + 2 H2O
how many moles of O2 are required for the complete combustion...
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