Answer the following questions using this balanced chemical equation. 2C3H6+9O2+6H2O How many grams of C3H6 are needed to produce 4.2 mol of H2O?
To find out the number of grams of C3H6 needed to produce 4.2 mol of H2O, we need to use stoichiometry. Here are the steps to calculate it:
Step 1: Determine the molar mass of C3H6.
C3H6 (propane) has a molar mass of:
3(12.01 g/mol) + 6(1.01 g/mol) = 42.08 g/mol
Step 2: Determine the stoichiometric ratio between C3H6 and H2O.
From the balanced chemical equation:
2C3H6 + 9O2 + 6H2O
We can see that 2 moles of C3H6 produce 6 moles of H2O.
Step 3: Convert mol of H2O to mol of C3H6.
Using the stoichiometric ratio, we can set up a conversion:
4.2 mol H2O × (2 mol C3H6 / 6 mol H2O) = 1.4 mol C3H6
Step 4: Convert mol of C3H6 to grams of C3H6.
Using the molar mass of C3H6:
1.4 mol C3H6 × (42.08 g C3H6 / 1 mol C3H6) = 58.912 g C3H6 (rounded to three significant figures)
Therefore, approximately 58.912 grams of C3H6 are needed to produce 4.2 mol of H2O.
To determine how many grams of C3H6 are needed to produce 4.2 mol of H2O, you need to use the given balanced chemical equation and its stoichiometry.
The balanced chemical equation is:
2C3H6 + 9O2 → 6H2O
From the equation, we can see that for every 2 moles of C3H6, 6 moles of H2O are produced. This means that the stoichiometric ratio between C3H6 and H2O is 2:6.
First, calculate the number of moles of C3H6 required to produce 4.2 mol of H2O using the stoichiometric ratio:
(4.2 mol H2O) x (2 mol C3H6 / 6 mol H2O) = 1.4 mol C3H6
Next, use the molar mass of C3H6 to convert the moles to grams. The molar mass of C3H6 is calculated by adding the atomic masses of carbon (C) and hydrogen (H):
Molar mass of C3H6 = (3 mol C x Atomic mass of C) + (6 mol H x Atomic mass of H)
= (3 mol x 12.01 g/mol) + (6 mol x 1.01 g/mol)
= 36.03 g/mol + 6.06 g/mol
= 42.09 g/mol
Finally, calculate the mass of C3H6 needed:
(1.4 mol C3H6) x (42.09 g C3H6 / 1 mol C3H6) = 58.93 g C3H6
Therefore, you would need 58.93 grams of C3H6 to produce 4.2 moles of H2O.