Answer: 55.9 kilopascals
Step-by-step explanation:
Given that:
Volume of gas (V) = 500.0mL
[convert 500.0 mL to liters
If 1000 mL = 1 liter
500.0 mL = 500.0/1000 = 0.5 liters]
Temperature of gas (T) = 265°C
Convert 265°C to Kelvin by adding 273
(265°C + 273 = 538K)
Pressure of gas (P) = ?
Number of moles (n) = 6.25 × 10^-3 mol
Molar gas constant (R) is a constant with a value of 0.0821 atm L K-1 mol-1
To get pressure, apply ideal gas equation
pV = nRT
p x 0.5L = 6.25 × 10^-3 mol x 0.0821 atm L K-1 mol-1 x 538K
0.5L•p = 0.276 atm L
Divide both sides by 0.5L
0.5L•p / 0.5L = 0.276 atm L / 0.5L
p = 0.552 atm
Since pressure is required in kilopascal, convert 0.552 atm to kilopascal
If 1 atm = 101.325 kPa
0..552 atm = Z
cross multiply
Z x 1 atm = 0.552 atm x 101.325 kPa
Z x 1 atm = 55.9 atm•kPa
Z = 55.9 atm•kPa / 1 atm
Z = 55.9 kPa
Thus, the pressure of the gas in kilopascals is 55.9 kPa