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

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.