A sample of krypton gas in a container of volume 1.90 L exerts a pressure of 0.553 atm at 21 Celsius. How many moles of gas are present?

0.044 mole

Explanation:

Data obtained from the question include:

V (volume) = 1.90 L

P (pressure) = 0.553 atm

T (temperature) = 21°C = 21 + 273 = 294K

R (gas constant) = 0.082atm. L/Kmol

n (number of mole of krypton) = ?

Using the ideal gas equation PV = nRT, the number of mole of krypton can obtained as illustrated below:

PV = nRT

n = PV / RT

n = (0.553 x 1.9) / (0.082x294)

n = 0.044 mole

Therefore, 0.044 mole of krypton is present in the container.

pv = nRT

n = PV/RT

n = 0.553*1.90/0.0821*294

n=1.0507/24.1374

n=0.0435mol