Question

How many moles of helium are required to fill a 5.10 L ballon to a pressure of 1.1 atm at 22 Kelvin? Show your work to receive full credit.

Answer 1

Answer:

n = 3.1 moles

Explanation:

Given that,

The volume of a balloon, V = 5.1 L

Pressure, P = 1.1 atm

Temperature, T = 22 K

We need to find the number of moles are required to fill the balloon. We know that,

Gas law, PV = nRT

Where

R is gas constant, R = 0.08206 L-atm/mol-K

So,

$n=\dfrac{PV}{RT}\\\\n=\dfrac{1.1\times 5.1}{0.08206 \times 22}\\\\n=3.1$

So, there are 3.1 moles of helium are required.

Answer 2

The moles of helium are required to fill a 5.10 L ballon to a pressure of 1.1 atm at 22 Kelvin is 3.1 moles.

How we calculate moles?

Moles of gases will be calculated by using the ideal gas equation as:

PV = nRT, where

P = pressure of gas = 1.1 atm

V = volume of gas = 5.10 L

R = universal gas constant = 0.08206 L-atm/mol-K

T = temperature of gas = 22K

n = moles of gas?

On putting all these values in the above equation and calculate for the value of n as:
n = 1.1 × 5.10 / 0.082 × 22 = 3.1 moles

Hence, the required moles is 3.1 moles.

To know more about ideal gas equation, visit the below link:
https://brainly.com/question/25290815