Step-by-step explanation:
Acetylene will burn according to the following equation:
2 C₂H₂ + 5 O₂ ----> 4 CO₂ + 2 H₂O
We have to find the mass of CO₂ that is produced when 14.5 g of C₂H₂ are burnt. First we have to convert the mass of C₂H₂ into moles using its molar mass.
mass of C₂H₂ = 14.5 g
molar mass of C₂H₂ = 26.04 g/mol
moles of C₂H₂ = 14.5 g * 1 mol/(26.04 g)
moles of C₂H₂ = 0.557 moles
2 C₂H₂ + 5 O₂ ----> 4 CO₂ + 2 H₂O
According to the coefficients of the equation, 4 moles of CO₂ are produced when 2 moles of C₂H₂ are burnt. We can use that ratio to find the moles of CO₂ that should be produced.
2 moles of C₂H₂ : 4 moles of CO₂ molar ratio
moles of CO₂ = 0.557 moles of C₂H₂ * 4 moles of CO₂/(2 moles of C₂H₂)
moles of CO₂ = 1.114 moles
And finally we can convert back to grams the moles of CO₂ that should be produced.
molar mass of CO₂ = 44.01 g/mol
mass of CO₂ = 1.114 moles * 44.01 g/mol
mass of CO₂ = 49.0 g
Now, to determine if the trial is successful we can find the percent yield of the reaction. The percent yield is defined like the actual yield of the reaction divided by the theoretical yield mulitplied by 100.
% yield = actual yield/(theoretical yield) * 100
During the experimental trial 30 g of CO₂ (actual yield) were produced but we found that 49.0 g of CO₂ should be produced (theoretical yield).
% yield = actual yield/(theoretical yield) * 100
% yield = 30.0 g/(49.0 g) * 100
% yield = 61.2 %
Since the % yield is only 61.2 % we can say that the designers shouldn't be happy with the results of the trial.
Answer:
a. 49.0 g of CO₂ should be produced.
b. Since the % yield of the reaction is only 61.2 % we can say that the designers shouldn't be happy with the results of the trial.