Agas collected from a reaction has a mass of 1.211 g and occupies a volume of 0.677 l. the temperature in the laboratory is 296 k, and the air pressure is 0.987 atm. calculate the molar mass of the gas.

a) 23.7 g/mol
b) 44.0 g/mol
c) 58.5 g/mol
d) 82.3 g/mol

B) 44.0 g/mol

Explanation:

To solve this problem we use the law of ideal gases, according to which ,

PV = nRT

where P, V, n and T are the pressure, volume, moles and temperature of the gas in question while R is the constant gas (0.082057 atm L / mol K)

The molar mass (MM) of a substance is given by

MM = m / n

where m is the mass of the substance. So,

n = m / MM

Substituting in the ideal gas equation we have

PV = () RT  →  MM =

→ MM =

→ MM = 44.0 g/mol

B) 44.0 g/mol

Explanation:

To solve this problem we use the law of ideal gases, according to which ,

PV = nRT

where P, V, n and T are the pressure, volume, moles and temperature of the gas in question while R is the constant gas (0.082057 atm L / mol K)

The molar mass (MM) of a substance is given by

MM = m / n

where m is the mass of the substance. So,

n = m / MM

Substituting in the ideal gas equation we have

PV = () RT  →  MM =

→ MM =

→ MM = 44.0 g/mol

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

i think its 100

i hope this !