Question

Suppose a piston automatically adjusts to maintain a gas at a constant pressure of 5.80 atm . For the initial conditions, consider 0.04 mol of helium at a temperature of 240.00 K . This gas occupies a volume of 0.14 L under those conditions. What volume will the gas occupy if the number of moles is increased to 0.07 mol (n2) from the initial conditions?

Answer 1

Answer: the new volume will be 0.245L

Explanation:Please see attachment for explanation

Answer 2

Answer:

The volume will be 238 mL or 0.238 L

Explanation:

Step 1: Data given

Pressure = constant = 5.80 atm

The initial moles of helium = 0.04 moles

Temperature = 240.00 K

Volume = 0.14L

The number of moles increases to 0.07 moles

Step 2: Calculate the new volume

p*V = n*R*T

V = (n*R*T)/p

⇒ with n = the number of moles = 0.07 moles

⇒ with R = the gas constant = 0.08206 L*atm/mol*K

⇒ with T = the temperature = 240.00 K

⇒ with p = the pressure = 5.80 atm

V = (0.07 * 0.08206 * 240.00) / 5.80

V = 0.238 L = 238 mL

The volume will be 238 mL or 0.238 L