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