Suppose 65.8 g of Carbon monoxide reacts with 8.6 g of hydrogen.
What is the limiting reagent?
What is the theoretical yield of the product in moles and grams?
If the actual yield of the product is 3.57 g, what is the percent yield?
To determine the limiting reagent, we need to compare the number of moles of each reactant to the stoichiometric ratio in the balanced chemical equation.
1. First, we need to convert the given masses of carbon monoxide (CO) and hydrogen (H2) into moles. We can use their molar masses to do this. The molar mass of CO is 28.01 g/mol, and the molar mass of H2 is 2.02 g/mol.
- Moles of CO = mass of CO / molar mass of CO
= 65.8 g / 28.01 g/mol
= 2.352 mol
- Moles of H2 = mass of H2 / molar mass of H2
= 8.6 g / 2.02 g/mol
= 4.257 mol
2. Next, we need to determine the stoichiometric ratio of CO to H2 in the balanced chemical equation. The balanced equation for the reaction is:
CO + H2 -> CH4 + O2
From the balanced equation, we can see that the stoichiometric ratio of CO to H2 is 1:1.
3. Now, we can compare the moles of CO and H2. Since the stoichiometric ratio is 1:1, the reactant with fewer moles is the limiting reagent.
In this case, CO has 2.352 mol and H2 has 4.257 mol. Since CO has fewer moles, it is the limiting reagent.
4. To calculate the theoretical yield of the product (CH4), we need to determine how many moles of CH4 can be formed from the limiting reagent. Again, we refer to the balanced chemical equation to find the stoichiometry.
From the balanced equation, we can see that the stoichiometric ratio of CO to CH4 is also 1:1. Therefore, the moles of CH4 formed will be equal to the moles of CO used.
The theoretical yield of CH4 in moles is 2.352 mol.
To calculate the theoretical yield in grams, we need to multiply the number of moles of CH4 by its molar mass. The molar mass of CH4 is 16.04 g/mol.
The theoretical yield of CH4 in grams is:
Theoretical yield = moles of CH4 * molar mass of CH4
= 2.352 mol * 16.04 g/mol
= 37.77 g
5. The actual yield of the product is given as 3.57 g.
To calculate the percent yield, we use the formula:
Percent yield = (actual yield / theoretical yield) * 100
Percent yield = (3.57 g / 37.77 g) * 100
= 9.46 %
Therefore, the percent yield is 9.46%.