Using the balanced equation for the combustion of ethane (C2H6), answer the following questions.
Using the balanced equation for the combustion of ethane (C2H6), answer the following questions.
2C2H6 + 702 -+ 4CO2 + 6H20
Be sure each of your answer entries has the correct number of significant figures.
Part 1 of 2
How many grams of CO2 are formed from 5.7 mol of C2H6?
g CO2
How many grams of H2O are formed from 0.52 mol of C2H6?
g H2O
To solve this problem, we first need to determine the molar ratio between C2H6 and CO2, as well as between C2H6 and H2O from the balanced equation.
From the balanced equation, we can see that 2 moles of C2H6 produce 4 moles of CO2 and 6 moles of H2O.
1. For CO2:
5.7 mol C2H6 x (4 mol CO2 / 2 mol C2H6) = 11.4 mol CO2
Now, we can convert the moles of CO2 to grams using the molar mass of CO2:
11.4 mol CO2 x (44.01 g CO2 / 1 mol CO2) = 500.214 g CO2
Therefore, 5.7 mol of C2H6 produces 500.214 g of CO2.
2. For H2O:
0.52 mol C2H6 x (6 mol H2O / 2 mol C2H6) = 1.56 mol H2O
Now, we can convert the moles of H2O to grams using the molar mass of H2O:
1.56 mol H2O x (18.015 g H2O / 1 mol H2O) = 28.4744 g H2O
Therefore, 0.52 mol of C2H6 produces 28.4744 g of H2O.