What is the density (in g/L) of methane (CH₄) at 25°C and 1.2 atm of pressure? The value of R = 0.0821 L atm mol^-1 K^-1.

Question

Quizplus · Accepted Answer

We can use the ideal gas law to find the density of methane:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. We want to find the density, which is the mass per unit volume, so we can rearrange the equation to:

P = (n/V)RT

The density is then given by:

density = mass/volume = (n × molar mass)/V

where the molar mass of methane is 16.04 g/mol.

So, we need to find the number of moles and the volume of the gas. We can use the ideal gas law again to find the volume:

V = nRT/P

Plugging in the given values, we get:

V = (1 mol × 0.0821 L atm mol^-1K^-1 × 298 K)/1.2 atm = 2.05 L

Now we can find the number of moles:

n = PV/RT = (1.2 atm × 2.05 L)/(0.0821 L atm mol^-1K^-1 × 298 K) = 0.0581 mol

Finally, we can calculate the density:

density = (0.0581 mol × 16.04 g/mol)/2.05 L = 0.787 g/L

Therefore, the answer is C.

What Is the Density (In G/L) of Methane (CH4) at 25°C

What Is the Density (In G/L) of Methane (CH₄) at 25°C