Question

A sample of helium gas occupies 11.6L at 305K and 1.48atm. How many moles of

helium does the sample contain? Your answer will be in moles (do not enter into blank),
round to 2 places past the decimal.

Answer 1

Answer: 0.000602 moles of helium gas

Step-by-step explanation:

We can use the ideal gas law to solve this problem

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 in Kelvin.

First, we need to convert the given volume of 11.6 L to cubic meters:

V = 11.6 L = 0.0116 m^3

Next, we can plug in the given values:

PV = nRT

n = PV/RT

n = (1.48 atm) (0.0116 m^3) / [(0.08206 L atm/mol K) (305 K)]

n = 0.000602 moles of helium

Therefore, the sample contains 0.000602 moles of helium gas.