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
Question
- At what temperature will 0.654 mol of neon gas occupy 12.30 L at 1.95 atm?*1 point264 K314 K389 K447 K
Solution
To solve this problem, we can use the ideal gas law equation, which is PV = nRT.
Here, P = pressure = 1.95 atm V = volume = 12.30 L n = number of moles = 0.654 mol R = ideal gas constant = 0.0821 L.atm/K.mol (since the pressure is given in atm and volume in L) T = temperature = ?
We need to find the temperature, so we rearrange the equation to solve for T:
T = PV / nR
Substitute the given values into the equation:
T = (1.95 atm * 12.30 L) / (0.654 mol * 0.0821 L.atm/K.mol)
Calculate the above expression to find the temperature. The answer should be in Kelvin.
Similar Questions
How many moles of neon (Ne) gas have a volume of 4.5 L and a pressure of 2.1 atm at 302 K?(The universal gas constant is 0.0821 L•atm/mol•K.)A.2.6 molB.0.38 molC.230 molD.0.086 mol
A 0.25 mol sample of neon gas at 18 °C and 0.799 atm is heated to 49 °C. The new gas pressure is 1.11 atm. What is the change in volume of the neon gas?
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.
If 21.5 mol of Ne gas occupies 105.8 L, how many mol of Ne would occupy 549.8 L under the same temperature and pressure? Record your answer in scientific notation using 3 significant figures.
Write the ideal gas equation and give the units for each term. Calculate the temperature in oC when 2.50 moles of argon occupy 25.0 L at 1.20 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.