Answer: 55.7 kPa
Step-by-step explanation:
Given variables are:
Volume of gas (V) = 500.0mL
convert volume in milliliters to liters
(since 1000mL = 1L
500.0mL = 500.0/1000 = 0.5L)
Temperature (T) = 265°C
Convert temperature in celsius to Kelvin
(265°C + 273 = 538K)
Pressure (P) = ?
Number of mole (n) = 6.25 x 10^-3 moles
- Molar gas constant (R) is a constant with a value of 0.0821 atm dm3 K-1 mol-1
Then, apply ideal gas equation
pV = nRT
p x 0.5L = 6.25 x 10^-3 mole 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 = 0.55 atm
The pressure in atmosphere is 0.55. So, convert it to kilopascal (kPa)
Since 1 atm = 101.325 kPa
0.55 atm = Z
cross multiply
Z x 1 atm = 101.325 kPa x 0.55 atm
Z = (101.325 kPa x 0.55 atm) / 1 atm
Z = 55.7 kpa
Thus, the pressure of the gas is 55.7 kilopascals