The amount of gas that occupies 36.52 L at 68.0 °C and 672 mm Hg is ________ mol.
A)127
B)1.15
C)878
D)24.4
E)12.7

Question

Quizplus · Accepted Answer

We need to use the ideal gas law which is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin by adding 273.15. So, T = 68.0 + 273.15 = 341.15 K.

Next, we need to convert the pressure from mm Hg to atm. 1 atm = 760 mm Hg, so 672 mm Hg = 672/760 atm = 0.8842 atm.

Now, we can rearrange the ideal gas law to solve for n:

n = PV/RT

n = (0.8842 atm)(36.52 L)/(0.0821 L·atm/mol·K)(341.15 K)

n = 1.15 mol

Therefore, the answer is choice B.

The Amount of Gas That Occupies 36