Of course! I can help you solve each of these problems step by step. Let's start with problem 1:
1. To determine which reactant is limiting and which is in excess, we need to compare the amount of each reactant to the stoichiometric ratio in the balanced equation.
Given:
Mass of Fe2O3 = 43.5 grams
Mass of CO = 43.5 grams
Balanced equation: Fe2O3 + 3CO --> 3CO2 + 2Fe
a) Calculate the number of moles for each reactant:
Molar mass of Fe2O3 = 159.69 g/mol
Molar mass of CO = 28.01 g/mol
Number of moles of Fe2O3 = Mass / Molar mass = 43.5 g / 159.69 g/mol
Number of moles of CO = Mass / Molar mass = 43.5 g / 28.01 g/mol
b) Compare the moles of each reactant to the stoichiometric ratio in the balanced equation. From the balanced equation, we can see that the ratio of Fe2O3 to CO is 1:3.
Since 1 mole of Fe2O3 reacts with 3 moles of CO, we need to determine which reactant has the smallest number of moles.
c) Calculate the mole ratio for each reactant:
Moles of Fe2O3 / Stoichiometric coefficient of Fe2O3 = 43.5 g / (159.69 g/mol) = 0.2723 mol
Moles of CO / Stoichiometric coefficient of CO = 43.5 g / (28.01 g/mol) = 1.553 mol
d) Compare the mole ratios:
Fe2O3:CO = 0.2723 mol : 1.553 mol
Since Fe2O3 has the smaller mole ratio, it is the limiting reactant, and CO is in excess.
Moving on to problem 2:
2. To calculate the percent yield of carbon dioxide, we need to compare the actual yield of CO2 to the theoretical yield, and then express it as a percentage.
Given:
Mass of CO2 produced = 20.0 grams
Mass of butane reacted = 19.5 grams
Balanced equation: 2C4H10 + 13O2 --> 8CO2 + 10H2O
a) Calculate the number of moles for each reactant and product:
Molar mass of CO2 = 44.01 g/mol
Molar mass of butane (C4H10) = 58.12 g/mol
Number of moles of CO2 = Mass / Molar mass = 20.0 g / 44.01 g/mol
Number of moles of butane = Mass / Molar mass = 19.5 g / 58.12 g/mol
b) Determine the stoichiometric ratio between CO2 and butane from the balanced equation. From the balanced equation, we can see that the ratio of butane to CO2 is 2:8 (which simplifies to 1:4).
c) Calculate the theoretical yield of CO2:
Theoretical yield of CO2 = Moles of butane * (Moles of CO2 / Moles of butane) * Molar mass of CO2
= (19.5 g / 58.12 g/mol) * (8 mol CO2 / 2 mol butane) * 44.01 g/mol
d) Calculate the percent yield of CO2:
Percent yield = (Actual yield of CO2 / Theoretical yield of CO2) * 100
= (20.0 g / Theoretical yield) * 100
For problem 3, 4, and 5, please provide more specific information such as the balanced equations and any given masses.