Stoichiometry Practice Stations

Given the unbalanced equation $N_2 + H_2 \rightarrow NH_3$, what is the mole ratio of $H_2$ to $NH_3$ in the balanced reaction?

If 25.0 grams of ammonium nitrate ($NH_4NO_3$) decomposes, according to the unbalanced equation $NH_4NO_3 \rightarrow N_2O + H_2O$, what mass of water ($H_2O$) is produced?

For the reaction $TiO_2 + C + Cl_2 \rightarrow TiCl_4 + CO_2$, how many grams of chlorine gas ($Cl_2$) are needed to react completely with 2.35 moles of titanium dioxide ($TiO_2$)?

In the reaction $NH_3 + O_2 \rightarrow H_2O + NO$, if 15.8 grams of ammonia ($NH_3$) reacts with excess oxygen, how many moles of water vapor ($H_2O$) are expected to form?

For the combustion of propane ($C_3H_8$) according to the unbalanced equation $C_3H_8 + O_2 \rightarrow H_2O + CO_2$, how many moles of oxygen ($O_2$) are required to completely combust 1.27 moles of propane?

If you have 4.66 g of $N_2$, determine how many grams of $H_2$ are needed to fully react and produce $NH_3$?

For the reaction $2NaOH + H_2SO_4 \rightarrow 2H_2O + Na_2SO_4$, how does increasing the amount of $H_2SO_4$ affect the amount of $Na_2SO_4$ produced, assuming $NaOH$ is the limiting reactant?

In the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if you start with 2 moles of $N_2$ and 5 moles of $H_2$, identify the limiting reactant.

Consider the reaction $C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O$. If 10 moles of $C_3H_8$ are reacted with 40 moles of $O_2$, what is the theoretical yield of $CO_2$ in moles?

If the actual yield of $H_2O$ in the reaction $C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O$ is 14.4 moles when 5 moles of $C_3H_8$ are reacted, what is the percent yield of the reaction?

For the reaction $2K + Cl_2 \rightarrow 2KCl$, if 7.84 grams of $K$ are allowed to react with excess $Cl_2$, what is the theoretical yield of $KCl$ in grams?

If the percent yield of a reaction is 85% and the theoretical yield is 40.0 grams, what is the actual yield of the product?

Given the balanced equation $4NH_3 + 5O_2 \rightarrow 4NO + 6H_2O$, if 34.0 grams of ammonia ($NH_3$) are reacted with excess oxygen, what mass of water ($H_2O$) is produced?

For the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if you start with 4.0 grams of $H_2$ and 32.0 grams of $O_2$, which reactant will be completely consumed?

Consider the reaction $C_6H_{12}O_6 \rightarrow 2C_2H_5OH + 2CO_2$. If 90.0 g of $C_6H_{12}O_6$ goes to completion, what is the theoretical mass yield of $C_2H_5OH$?

In a chemical reaction, what does the term 'stoichiometric coefficients' refer to, and how are they used in stoichiometric calculations?

How does the concept of 'limiting reactant' influence the maximum amount of product that can be formed in a chemical reaction?

Explain the difference between 'theoretical yield' and 'actual yield' in a chemical reaction, and what does the percent yield represent?

If a reaction has a high percent yield, does this always indicate that the reaction was performed without any errors or loss of product? Explain.

A student performs a reaction and calculates a theoretical yield of 25.0 grams of product. If their actual yield is 20.0 grams, explain two potential reasons why the actual yield is less than the theoretical yield.

Consider a scenario where two different reactions produce the same product. Explain how stoichiometry can be used to determine which reaction is more efficient in producing the desired product.

Explain why it is important to balance a chemical equation before performing stoichiometric calculations.

In the context of stoichiometry, what is the significance of Avogadro's number, and how is it used in converting between moles and number of particles (atoms, molecules, ions)?

Describe how the concepts of stoichiometry are applied in real-world scenarios, outside of a chemistry laboratory setting.

How does the presence of impurities in a reactant affect the accuracy of stoichiometric calculations used to predict the amount of product formed?