2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g) If 50.0 mols of carbon dioxide were produced, how many mols of acetylene (C2H2) were used?
To determine how many moles of acetylene (C2H2) were used, we need to use the balanced chemical equation for the reaction:
2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
From the balanced equation, we can see that the coefficient in front of acetylene (C2H2) is 2. This means that for every 2 moles of C2H2 used, we will produce 4 moles of CO2.
We are given that 50.0 moles of carbon dioxide (CO2) were produced. Since the stoichiometric ratio of CO2 to C2H2 is 4:2, we can set up a proportion to find the number of moles of C2H2 used.
(50.0 mol CO2 / 4 mol CO2) = (x mol C2H2 / 2 mol C2H2)
Cross-multiplying and solving for x, we get:
x = (50.0 mol CO2 * 2 mol C2H2) / 4 mol CO2
x = 100.0 mol C2H2
Therefore, 100.0 moles of acetylene (C2H2) were used in the reaction.