A gaseous product of a reaction is collected at 280K and 0.95 atm. Given R = 0.0821L atm what is the molar mass of the gas, in grams per mole, if 5.49 g of gas occupies 4.92 L? (1 point)

24 g/mol

27 g/mol

0.04 g/mol

133 g/mol

27 g/mol

Explanation:

We'll use this formula: PV = nRT

P = Pressure (0.95)

V = Volume (4.92)

n = moles (?)

R = Constant (0.0821)

T = Temperature in kelvins (280)

(0.95)(4.92) = n(0.0821)(280)

4.674 = 22.988n

Divide both sides by 22.988

4.674/22.988 = 22.988n/22.988

n = 0.20332347

Or just round it to 0.2

This means are 0.2 moles

Divide the grams by moles

5.49/0.2 = 27.45

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.