Answer:
molar mass = 16.03 g/mol.
Yes, the mentioned gas is methane.
Explanation:
- We can use the general law of ideal gas: <em>PV = nRT</em>.
where, P is the pressure of the gas in atm (P = 1.0 atm, at STP).
V is the volume of the gas in L (V = 2.0 L).
n is the no. of moles of the gas in mol (n = ??? mol).
R is the general gas constant (R = 0.0821 L.atm/mol.K),
T is the temperature of the gas in K (T = 273 K, at STP).
∴ n = PV/RT = (1.0 atm)(2.0 L)/(0.0821 L.atm/mol.K)(273 K) = 0.08923 mol.
∵ n = mass/molar mass
<em>∴ molar mass = mass/n</em> = (1.43 g)/(0.08923 mol) = <em>16.03 g/mol.</em>
∵ molar mass of methane (CH₄) = 16.0 g/mol.
<em>So, the mentioned gas is methane.</em>
