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
Solution 1
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 Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
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.
How many moles of gas (to 1 decimal place, input value only), are contained in a 54.25 L vessel at a pressure of 173.6 kPa and temperature of 0.2 °C?
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.
A sample of an ideal gas has a volume of 0.00100 m3, a pressure of 4.50 atmospheres and 2.00 × 1023 particles. What is the temperature of the gas?
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.