Carbon and oxygen react to form carbon monoxide:

$$2 \mathrm { C } + \mathrm { O } _ { 2 } \longrightarrow 2 \mathrm { CO }$$

. What masses of carbon and oxygen are needed to make 56.0 g CO? Which law does this illustrate?

When sodium chloride reacts with silver nitrate, silver chloride precipitates. What mass of AgCl is produced from 75.0 g

$$\mathrm { AgNO } _ { 3 } ?$$

Acetylene gas,

$$\mathrm { C } _ { 2 } \mathrm { H } _ { 2 }$$

is produced as a result of the following reaction:

$$\mathrm { CaC } _ { 2 } ( s ) + 2 \mathrm { H } _ { 2 } \mathrm { O } ( l ) \longrightarrow \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } ( \mathrm { g } ) + \mathrm { Ca } ( \mathrm { OH } ) _ { 2 } ( a q )$$

. a. If 32.0 g

$$\mathrm { CaC } _ { 2 }$$

are consumed in this reaction, how many moles of

$$\mathrm { H } _ { 2 } \mathrm { O }$$

are needed? b. How many moles of each product would form?

Which law would you use to compare CO and $\mathrm{CO}_{2}$? Explain. Without doing any calculations, determine which of the two compounds has the highest percent by mass of oxygen in the compound.

Consider the combustion of carbon monoxide (CO) in oxygen gas:

$$2\mathrm{CO}(g)+\mathrm{O_2}(g)\rightarrow2\mathrm{CO_2}(g)$$

Starting with 3.60 moles of CO, calculate the number of moles of

$$\mathrm{CO_2}$$

produced if there is enough oxygen gas to react with all the CO.