Question

One mole of an ideal gas at 1.00 atm and 0.00°C occupies 22.4 L. How many molecules of an ideal gas are in one cm^3 under these conditions?a. 28.9 b. 22 400 c. 2.69 × 1019 d. 6.02 × 1023

Answer 1

Given:

Atm = 1.00 atm

Temperature = 0.00°C

Amount of gas = 1 mole which occupues 22.4 L

Let;s find the number of molecules of an ideal gas are in one cm^3 under these conditions.

We have:

1 mole of ideal gas = 22.4 L

This is called the molar volume of gas.

To find the amount of molecules, apply the avogrado's constant:

Number of molecules in 1 mol = 6.023 x 10²³

Hence, for 1 cm³, we have:

`\text{ No. of molecules in 1 cm}^3=(6.023*10^(23))/(22.4*10^3)`

Solving further:

`\text{ No. of molecules in 1 cm}^3=(6.023*10^(23))/(22.4*10^3)=2.69*10^(19)mol/cm^3`

Therefore, the amount of molecules of an ideal gas in one cm^3 under these conditions is:

2.69 x 10¹⁹ mol/cm^3

ANSWER:

C. 2.69 x 10¹⁹