How much pressure would 0.8 moles of a gas at 370K exert if it occupied 17.3L of space
2 answers:
Answer:
1.40 atm is the pressure for the gas
Explanation:
An easy problem to solve with the Ideal Gases Law:
P . V = n . R .T
T° = 370K
V = 17.3L
n = 0.8 mol
Let's replace data → P . 17.3L = 0.8mol . 0.082L.atm/mol.K . 370K
P = (0.8mol . 0.082L.atm/mol.K . 370K) / 17.3L = 1.40 atm
Answer:
The pressure is 1.40 atm
Explanation:
Step 1: Data given
Number of moles = 0.8 moles
Temperature = 370 K
volume = 17.3 L
Step 2: Calculate the pressure
p*V = n*R*T
⇒ with p = the pressure = TO BE DETERMINED
⇒with V = the volume = 17.3 L
⇒with n = the number of moles of gas = 0.8 moles
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 370 K
p = (n*R*T)/V
p = (0.8 * 0.08206 * 370) / 17.3 L
p = 1.40 atm
The pressure is 1.40 atm
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