How many moles are contained in a 4.67-L sample of gas at 30°C and 199 kPa?

A. 1.7 mol
B. 11.8 mol
C. 0.37 mol
D. 3.7 mol

I guessed D, but I'm not sure.

PV = nRT. Solve for n.

To find the number of moles of gas in a given sample, we can use the ideal gas law equation: 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, we need to convert the temperature from Celsius to Kelvin by adding 273.15. So, 30°C + 273.15 = 303.15 K.

Next, we need to convert the pressure from kilopascals (kPa) to atmospheres (atm) since the ideal gas constant (R) is usually expressed in terms of atm. There are 101.325 kPa in 1 atm, so 199 kPa ÷ 101.325 = 1.968 atm.

Now, we can plug in the values into the ideal gas law equation:

PV = nRT

(1.968 atm) * (4.67 L) = n * (0.0821 L·atm/mol·K) * (303.15 K)

9.16656 atm·L = n * 24.918015 L·atm/mol·K

n = (9.16656 atm·L) / (24.918015 L·atm/mol·K)

n = 0.3685 mol

So, there are approximately 0.37 moles of gas in the 4.67-L sample.

The correct answer is C. 0.37 mol.