At what Celsius temperature (in degrees Celsius) does 10.5 g of ammonia gas exert a pressure of 98.7 kPa in a 48.3 L container?
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in kPa)
V = volume (in Liters)
n = number of moles
R = ideal gas constant (8.31 L*kPa/mol*K)
T = temperature (in Kelvin)
First, we need to convert the given values to appropriate units:
10.5 g of ammonia gas = 10.5 g / 17.031 g/mol = 0.617 mol
Pressure = 98.7 kPa
Volume = 48.3 L
R = 8.31 L*kPa/mol*K
Now we can rearrange the ideal gas law equation to solve for T:
T = (P*V) / (n*R)
T = (98.7 kPa * 48.3 L) / (0.617 mol * 8.31 L*kPa/mol*K)
T = (4760.41 kPa*L) / (5.12417 L*kPa)
T = 930.23 K
To convert the temperature from Kelvin to Celsius, subtract 273.15:
T = 930.23 K - 273.15 = 657.08 degrees Celsius
Therefore, at 657.08 degrees Celsius, 10.5 g of ammonia gas would exert a pressure of 98.7 kPa in a 48.3 L container.