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Calculate the pressure of 0.76 moles of methane that occupies 2800 cm3 at a temperature of 290 K.A. 2664.82 PaB. 654.12 kPaC. 0.654 kPaD. 60.97 Pa

User Ennabah
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1 Answer

12 votes
12 votes

Step-by-step explanation:

We have to find the pressure of a 0.76 moles sample of methane that occupies 2800 cm³ at a temperature of 290 K. We can use the ideal gas law to find it.

P * V = n * R * T

P = n * R * T/V

Where P is the pressure in atm, n is the number of moles, R is the ideal gas constant (0.082 atm*L/(mol*K), T is the temperature in K and V is the volume in L. We already know those values:

P = ?

n = 0.76 moles

R = 0.082 atm*L/(mol*K)

T = 290 K

V = 2800 cm³ * 1 L/(1000 cm³)

V = 2.800 L

We can replace these values into the equation and get the answer to our problem.

P * V = n * R * T

P = n * R * T/V

P = 0.76 moles * 0.082 atm*L/(mol*K) * 290 K/(2.8 L)

P = 6.45 atm

Finally we have to convert the answer to Pa.

101325 Pa = 1 atm

P = 6.45 atm * 101325 Pa/(1 atm)

P = 653546 Pa = 653546 Pa * 1 kPa/(1000 Pa)

P = 654 kPa

Answer: B. 654.12 kPa

User SuperManSL
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