Question

1. What pressure (in kPa) is required to contain 0.15 moles of N, gas in a 4.2 Lcontainer at a temperature of 23.0°C?

Answer 1

`89.17\text{ kPa}`

Step-by-step explanation:

Here, we want to get the required pressure in kPa

We start by writing the ideal gas equation

We have that as:

`PV\text{ = nRT}`

where P is the pressure we want to calculate

V is the volume which is 4.2 L

n is the number of moles which is 0.15

T is the temperature which we will convert to Kelvin by adding 273K:

We have that as 273 + 23 = 300K

R is the molar gas constant which is 0.0821 L.atm/mol.K

Substituting the values, we have it that:

`P\text{ = }(nRT)/(V)\text{ = }\frac{0.15\text{ }*0.0821*300}{4.2}\text{ = 0.88 atm}`

Finally, we convert the pressure in atm to pressure in kPa

To do this, we multiply the atm value by 101.325

We have that as:

`0.88\text{ }*\text{ 101.325 = 89.17 kPa}`