# Question #38860

##### 1 Answer

The answer is **B)**

#### Explanation:

The idea here is that you need to convert everything to *grams*.

You already know that one of the samples contains **gram atoms** of nitrogen. Now, a *gram atom* is used to denote the mass of a substance that contains **atoms**.

Note that **Avogadro's constant**, represents the *definition of a mole*.

Simply put, a gram atom is the mass of a substance that contains **mole** of atoms. In this case, **gram atoms** of nitrogen will be equivalent to **moles** of elemental nitrogen.

This means that the mass of the first sample will be

#2 color(red)(cancel(color(black)("moles N"))) * "14 g"/(1color(red)(cancel(color(black)("mole N")))) = "28 g"#

Keep in mind that the *relative atomic mass* is actually **equivalent** to its **molar mass**. So if nitrogen is said to have a relative atomic mass of **molar mass** will be equal to

The relative atomic mass of silver is said to be equal to **mole** of silver atoms has a mass of

Now, a sample of any ideal gas that is being kept at a pressure of **exactly** **mole** of gas and occupies

This implies that you're dealing with **mole** of oxygen gas, *molar mass* of

#M_ ("M O"_2) = 2 xx "16 g mol"^(-1) = "32 g mol"^(-1)#

You can thus say that the sample of oxygen gas has a mass of

Finally, **mole** of carbon.

This means that the last sample will contain **mole** of carbon and have a mass of

Therefore, you will have

#"108 g Ag" > "32 g O"_2 > "28 g N" > "12 g C"#