Methanol(CH4O),used in racing cars,burns O2 to form CO2and H2O.
2CH4O(l) + 3O2(g)-->2Co2(g) +4H2O(g)
32.0g/mol 32.g/mol 44.g/mol 18.g/mol
What is the theoretical yield of CO2 from 48 g of methanol?
What is the percent yield of CO2 if 48.0g og CO2 are formed?
66 g
72.8%
To find the theoretical yield of CO2 from 48 g of methanol, we need to use the given molar mass of methanol (32.0 g/mol) and the balanced chemical equation:
2CH4O(l) + 3O2(g) --> 2Co2(g) + 4H2O(g)
Step 1: Calculate the number of moles of methanol
48 g of methanol / 32.0 g/mol = 1.5 mol of methanol
Step 2: Use stoichiometry to find the number of moles of CO2
From the balanced equation, we know that 2 moles of methanol react to produce 2 moles of CO2.
So, 1.5 mol of methanol will produce (1.5 mol × 2 mol CO2/2 mol methanol) = 1.5 mol of CO2.
Step 3: Calculate the mass of CO2
Mass = Moles × Molar mass = 1.5 mol × 44 g/mol = 66 g
Therefore, the theoretical yield of CO2 from 48 g of methanol is 66 g.
To find the percent yield of CO2 if 48.0 g of CO2 are formed, we can use the formula:
Percent Yield = (Actual Yield/Theoretical Yield) × 100
Step 1: Determine the theoretical yield of CO2 (which we calculated as 66 g in the previous step).
Step 2: Calculate the percent yield:
Percent Yield = (48 g/66 g) × 100 = 72.7%
Therefore, the percent yield of CO2 is approximately 72.7% if 48.0 g of CO2 are formed.
To find the theoretical yield of CO2 from 48 g of methanol, we need to use stoichiometry.
First, we need to determine the molar mass of methanol (CH4O):
Methanol (CH4O) = 12.0 g/mol (C) + 4 * 1.0 g/mol (H) + 16.0 g/mol (O)
= 32.0 g/mol
Given that the balanced equation is:
2CH4O(l) + 3O2(g) -> 2CO2(g) + 4H2O(g),
we see that the stoichiometric ratio between CH4O and CO2 is 2:2 or 1:1.
Now, we can set up a proportion to find the moles of CO2:
(48 g CH4O) * (1 mol CH4O / 32.0 g CH4O) * (2 mol CO2 / 2 mol CH4O) = 3 mol CO2
So, the theoretical yield of CO2 from 48 g of methanol is 3 mol.
To calculate the percent yield of CO2, we need the actual yield of CO2. Let's assume that the actual yield is 48.0 g of CO2.
The percent yield is calculated using the following formula:
Percent yield = (actual yield / theoretical yield) * 100%
Plugging in the values, we get:
Percent yield = (48.0 g CO2 / 3 mol CO2) * (44.0 g/mol CO2) * 100%
Percent yield = 800%
Since percent yield cannot exceed 100%, it seems there is an error in the data provided or the calculation.