A 0.286g sample of carbon dioxide, CO2, has a volume of 585mL and a pressure of 495mmHg . What is the temperature, in kelvins and degrees Celsius, of the gas?

Use PV = nRT.

P = 495 mm; convert to atm.
V = 585 mL; convert to L.
n = g/molar mass = 0.286/44 = ?
R = you know
T = kelvin. Substitute and solve for T in kelvin, the
K = 273 + C to calculate C.

When I've done the equation I've gotten 713.971 K for the first part. What have I done wrong?

Probably nothing. Using 44 for the molar mass of CO2 I obtained 714.3 K. You may have punched in a wrong digit somewhere.

For n I have 0.286/44 = 0.00650
Using 44.01 for the molar mass gave me 714.5 K.

thanks for your help

287

To find the temperature of the gas, you can use the ideal gas law equation, which is given by:

PV = nRT

Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Ideal gas constant
T = Temperature of the gas in Kelvin

The ideal gas constant, R, can be found in various unit values. In this case, we will use R = 0.0821 L.atm/mol.K.

We can rearrange the equation to solve for temperature, T:

T = PV / nR

First, let's determine the number of moles (n) of the gas using the sample mass and molecular weight. The molecular weight of carbon dioxide (CO2) is 44.01 g/mol.

n = Mass / Molecular weight
n = 0.286 g / 44.01 g/mol

n ≈ 0.0065 mol

Now we can substitute the values into the equation:

T = (495 mmHg) * (0.585 L) / (0.0065 mol * 0.0821 L.atm/mol.K)

Simplifying the equation:

T ≈ 367 K

To convert the temperature from Kelvin (K) to degrees Celsius (°C), you can use the following formula:

°C = K - 273

Therefore:

°C ≈ 367 - 273
°C ≈ 94°C

So, the temperature of the gas is approximately 94°C or 367 Kelvin.