Answer:
The mass of CO2 produced from 20 grams of C2H2 is approximately 67.61 grams.
Step-by-step explanation:
The balanced equation for the combustion of C2H2 with O2 to produce CO2 and H2O is:
C2H2 + 2O2 → 2CO2 + H2O
From the balanced equation, we can see that the stoichiometric ratio of C2H2 to CO2 is 1:2. This means that for every 1 mole of C2H2 that reacts, 2 moles of CO2 are produced.
To determine the mass of CO2 produced from 20 grams of C2H2, we first need to calculate the number of moles of C2H2:
n(C2H2) = m/M
where:
m = mass of C2H2 (20 g)
M = molar mass of C2H2 (2 x 12.01 g/mol + 2 x 1.01 g/mol = 26.04 g/mol)
n(C2H2) = 20 g / 26.04 g/mol
n(C2H2) = 0.7686 mol
Since the stoichiometric ratio of C2H2 to CO2 is 1:2, the number of moles of CO2 produced is twice the number of moles of C2H2:
n(CO2) = 2 x n(C2H2)
n(CO2) = 2 x 0.7686 mol
n(CO2) = 1.5372 mol
Now, we can calculate the mass of CO2 produced:
m(CO2) = n x M
where:
n = number of moles of CO2 (1.5372 mol)
M = molar mass of CO2 (12.01 g/mol + 2 x 16.00 g/mol = 44.01 g/mol)
m(CO2) = 1.5372 mol x 44.01 g/mol
m(CO2) = 67.61 g
Therefore, the mass of CO2 produced from 20 grams of C2H2 is approximately 67.61 grams (to two decimal places).