# Excess Reagent

4 H$_2$ (g) + CS$_2$ (g) $\longrightarrow$ CH$_4$ + 2 H$_2$S (g)

Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate the remaining mass after 36 L of H$_2$ reacts with 12 L of CS$_2$

## Related Problems

N$_2$ + 3 H$_2$ $\longrightarrow$ 2 NH$_3$

How many grams of hydrogen are needed to produce 68 g of ammonia? (molar mass of NH$_3$ = 12.031 g/mol, the molar mass of H$_2$ = 2.015 g/mol)

2 Al + Fe$_2$O$_3$ $\longrightarrow$ Al$_2$O$_3$ + 2 Fe

An operation requires at least 86.0 g of Fe to be produced. What is the minimum mass in grams of Fe$_2$O$_3$ necessary to produce the desired amount of products? How much Al$_2$O$_3$ is produced as a side product?

MM of Fe$_2$O$_3$ = 159.489 g/mol

MM of Al$_2$O$_3$ = 101.961 g/mol

H$_2$SO$_4$ + 2 KOH $\longrightarrow$ 2 H$_2$O + K$_2$SO$_4$

How many moles of KOH are requred to make 3.0 moles of K$_2$SO$_4$ ?

N$_2$ + 3 H$_2$ $\longrightarrow$ 2 NH$_3$

If 5 moles of N$_2$ react with excess H$_2$ how many moles of NH$_3$ will the reaction yield?