Answer :

To find the temperature of the helium gas, we can use the Ideal Gas Law equation, which is:

[tex]\[ PV = nRT \][/tex]

Where:
- [tex]\( P \)[/tex] is the pressure in atmospheres (atm).
- [tex]\( V \)[/tex] is the volume in liters (L).
- [tex]\( n \)[/tex] is the number of moles.
- [tex]\( R \)[/tex] is the ideal gas constant ([tex]\( R = 0.0821 \)[/tex] L·atm/mol·K).
- [tex]\( T \)[/tex] is the temperature in Kelvin (K).

Here are the steps to find the temperature:

1. Find the number of moles of helium ([tex]\( n \)[/tex]):

First, we need to calculate the number of moles of helium using its mass and molar mass.

- The given mass of helium is 3.05 grams.
- The molar mass of helium is approximately 4.00 g/mol.

Use the formula for moles:

[tex]\[
n = \frac{\text{mass}}{\text{molar mass}} = \frac{3.05 \, \text{g}}{4.00 \, \text{g/mol}} = 0.7625 \, \text{mol}
\][/tex]

2. Plug in the known values into the Ideal Gas Law to solve for [tex]\( T \)[/tex]:

Given:
- Pressure ([tex]\( P \)[/tex]) = 1.70 atm
- Volume ([tex]\( V \)[/tex]) = 14.1 L
- Number of moles ([tex]\( n \)[/tex]) = 0.7625 mol
- Ideal gas constant ([tex]\( R \)[/tex]) = 0.0821 L·atm/mol·K

Rearrange the formula to solve for [tex]\( T \)[/tex]:

[tex]\[
T = \frac{PV}{nR} = \frac{1.70 \, \text{atm} \times 14.1 \, \text{L}}{0.7625 \, \text{mol} \times 0.0821 \, \text{L·atm/mol·K}}
\][/tex]

3. Calculate the temperature ([tex]\( T \)[/tex]):

[tex]\[
T \approx 382.9 \, \text{K}
\][/tex]

So, the temperature of the helium gas under the given conditions is approximately 382.9 Kelvin.

Thank you for reading the article What is the temperature of 3 05 g of helium gas at a pressure of 1 70 atm and a volume of 14 1 L. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!

Rewritten by : Jeany

Other Questions