Theoretical and Percentage Yield — MCQ Practice

Consider the reaction: $2Al(s) + 3Cl_2(g) \rightarrow 2AlCl_3(s)$. If $54,\text{g}$ of Aluminum reacts with $71,\text{g}$ of Chlorine, and $100,\text{g}$ of Aluminum chloride is actually produced, what is the percentage yield of the reaction? (Atomic masses: Al = $27,\text{g/mol}$, Cl = $35.5,\text{g/mol}$)

In the reaction $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)$, if $22,\text{g}$ of propane ($C_3H_8$) reacts with $96,\text{g}$ of oxygen ($O_2$), what is the theoretical yield of carbon dioxide ($CO_2$) in grams? (Atomic masses: C = $12,\text{g/mol}$, H = $1,\text{g/mol}$, O = $16,\text{g/mol}$)

If the theoretical yield of a reaction is $150,\text{g}$ and the actual yield obtained is $120,\text{g}$, what is the percentage yield?

Which of the following factors would NOT typically lead to an actual yield being lower than the theoretical yield?

For the reaction $Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)$, if $160,\text{g}$ of $Fe_2O_3$ reacts with $84,\text{g}$ of $CO$, and the percentage yield is $75\%$, what is the actual mass of Fe produced? (Atomic masses: Fe = $56,\text{g/mol}$, O = $16,\text{g/mol}$, C = $12,\text{g/mol}$)

Which statement best describes the relationship between theoretical yield and actual yield?

A student performs a reaction where the theoretical yield of product X is $20.0,\text{g}$. If the student achieves a percentage yield of $90.0\%$, what mass of product X did they actually obtain?