Question

I really need help for this chemistry question. Steps and how it was worked out would be helpful!

Answer 1

Data:
V (volume) = 500.0 mL = 0.5 L
T (temperature) = 15.00ºC
(converting in Kelvin) → TK = TC + 273 → TK = 15 + 273 = 288 K
P (pressure) = 736.0 mmHg
R (constant) = 62.363 (mmHg*L/mol*K)
m (mass) = 2.688 g
M (Molar Mass) = ? (g/mol)

Formula: General Gas Equation

`P*V = n*R*T \to \boxed{P*V = (m)/(M) *R*T}`

Solving:

`P*V = (m)/(M) *R*T`

`736*0.5 = (2.688)/(M) *62.363*288`

`368 = (2.688)/(M) *17960.544`
Product of extremes equals product of means:

`368*M = 2.688*17960.544`

`368M = 48277.94227`

`M = (48277.94227)/(368)`

`M = 131.1900605\to \boxed{\boxed{M \approx 131.2\:g/mol}}`

Therefore: The gas found to have such a molar mass is xenon gas