Question

If 0.250 mole of neon gas has a volume of 1520 mL at a pressure of 325 mmHg, what will be its

temperature in kelvins and in degrees Celsius? Show the rearranged ideal gas law solving for T. Cancel
units in work.

Answer 1

Step-by-step explanation:

We can use the ideal gas law to solve for the temperature of the neon gas:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

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

V = 1520 mL = 1.52 L

Next, let's rearrange the ideal gas law to solve for T:

T = PV/nR

Now we can plug in the values and solve:

T = (325 mmHg)(1 atm/760 mmHg)(1.52 L)/(0.250 mol)(0.0821 L·atm/(mol·K))

T = 89.6 K

To convert to degrees Celsius, we subtract 273.15:

T = 89.6 K - 273.15 = -183.6 °C

Therefore, the temperature of the neon gas is 89.6 K or -183.6 °C.