in the chemical equation :2C2H6+7O2->4CO2+6H2O, hOW many moles of c2h6 will you need to form 2.34 mol of co2? How many moles of water will be produced?
You need half as many moles of C2H6, according to the balanced equation.
To determine the number of moles of C2H6 needed to form 2.34 mol of CO2, we need to use the stoichiometric coefficients in the balanced chemical equation.
The balanced equation is:
2C2H6 + 7O2 → 4CO2 + 6H2O
From the equation, we can see that 2 moles of C2H6 will produce 4 moles of CO2. This means that the ratio of moles of C2H6 to moles of CO2 is 2:4, or simply 1:2.
Since we want to know how many moles of C2H6 are needed to produce 2.34 mol of CO2, we can set up the following proportion:
1 mol C2H6 / 2 mol CO2 = x mol C2H6 / 2.34 mol CO2
Cross-multiplying and solving for x gives us:
x = (1 mol C2H6 * 2.34 mol CO2) / 2 mol CO2
x = 2.34 / 2
x = 1.17 mol C2H6
Therefore, to form 2.34 mol of CO2, you will need 1.17 moles of C2H6.
To determine the number of moles of water produced, we can apply the same approach. From the balanced equation, we see that for every 2 moles of C2H6 consumed, 6 moles of H2O are produced. Therefore, the ratio of moles of C2H6 to moles of H2O is 2:6 or 1:3.
Again, set up the proportion:
1 mol C2H6 / 2 mol H2O = x mol C2H6 / y mol H2O
Since we want to know the moles of H2O produced, we'll set up the equation as:
1 mol C2H6 / 2 mol H2O = 1.17 mol C2H6 / y mol H2O
Cross-multiplying and solving for y gives us:
y = (1 mol C2H6 * 2 mol H2O) / 1.17 mol C2H6
y = 2 / 1.17
y ≈ 1.71 mol H2O
Therefore, when 2.34 mol of CO2 is formed, approximately 1.71 moles of H2O will be produced.
To determine the number of moles of C2H6 needed to form 2.34 mol of CO2, we can use the stoichiometric coefficients in the balanced chemical equation:
2C2H6 + 7O2 -> 4CO2 + 6H2O
The stoichiometry tells us that for every 2 moles of C2H6, 4 moles of CO2 are produced.
Therefore, we can set up a proportion to solve for the number of moles of C2H6:
2 mol C2H6 / 4 mol CO2 = x mol C2H6 / 2.34 mol CO2
By cross-multiplying and solving for x, we get:
x = (2 mol C2H6 * 2.34 mol CO2) / 4 mol CO2
x = 1.17 mol C2H6
Hence, we will need 1.17 moles of C2H6 to form 2.34 mol of CO2.
To determine the number of moles of water produced, we can use the stoichiometric coefficients in the balanced chemical equation:
2C2H6 + 7O2 -> 4CO2 + 6H2O
The stoichiometry tells us that for every 2 moles of C2H6, 6 moles of H2O are produced.
Therefore, we can set up a proportion to solve for the number of moles of H2O:
2 mol C2H6 / 6 mol H2O = 1.17 mol C2H6 / x mol H2O
By cross-multiplying and solving for x, we get:
x = (6 mol H2O * 1.17 mol C2H6) / 2 mol C2H6
x = 3.51 mol H2O
Hence, 3.51 moles of water will be produced.