Question

A automobile piston at a pressure of 3.2 atm has a volume of

1.5mL. How many moles of gas will the piston contain at 345 K?

Answer 1

Answer and Explanation:

To find the number of moles of gas in the piston, we can use the ideal gas law equation:

PV = nRT

Where:

P = pressure (in atm)

V = volume (in liters)

n = number of moles

R = ideal gas constant (0.0821 L·atm/mol·K)

T = temperature (in Kelvin)

First, let's convert the volume from milliliters to liters:

Volume = 1.5 mL = 1.5 mL * (1 L / 1000 mL)

Volume = 0.0015 L

Next, let's substitute the given values into the ideal gas law equation:

3.2 atm * 0.0015 L = n * 0.0821 L·atm/mol·K * 345 K

Now, let's solve for n (number of moles):

n = (3.2 atm * 0.0015 L) / (0.0821 L·atm/mol·K * 345 K)

n ≈ 0.000136 mol

Therefore, the piston contains approximately 0.000136 moles of gas.