At what temperature (in K) would 2.10 mol of N2 gas have a pressure of 1.25 atm in a 22.1 L tank? (R = 0.0821 L·atm/mol·K.
Question
At what temperature (in K) would 2.10 mol of N2 gas have a pressure of 1.25 atm in a 22.1 L tank? (R = 0.0821 L·atm/mol·K.
Solution
To solve this problem, we can use the ideal gas law equation, which is:
PV = nRT
Where: P = pressure V = volume n = number of moles R = ideal gas constant T = temperature
We are asked to find the temperature (T), so we rearrange the equation to solve for T:
T = PV / nR
Now we can substitute the given values into the equation:
T = (1.25 atm * 22.1 L) / (2.10 mol * 0.0821 L·atm/mol·K)
Now, calculate the value:
T = 27.75 / 0.17241
T = 160.9 K
So, the temperature of the gas would be approximately 161 K.
Similar Questions
What is the pressure of 5.0 mol nitrogen (N2) gas in a 2.0 L container at 268 K?(The universal gas constant is 0.0821 L•atm/mol•K.)A.0.018 atmB.8.8 atmC.55 atmD.220 atmSUBMITarrow_backPREVIOUS
A quantity of 2.00 mol of an ideal gas is maintained at a temperature of 127ûC in a containerof volume 0.083 m3 . What is the pressure of the gas?
What is the volume of 0.98 mol oxygen (O2) gas at 275 K and a pressure of 2.0 atm?(The universal gas constant is 0.0821 L•atm/mol•K.)A.44 LB.11 LC.46 LD.0.090 L
40. At what temperature will 0.654 mol of neon gas occupy 12.30 L at 1.95 atm?*1 point264 K314 K389 K447 K
A 1.0 L container is filled with gas at 2.5 atm. Later the gas is transferred into a larger 3.0 L container. Determine the pressure of the gas in the larger container if the temperature of the gas also changed from 350 K to 298 K.Question 4Select one:a.2.1 atmb.0.71 atmc.0.98 atmd.0.83 atm
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.