Calculate the pressure of 0.55 mol NH3 gas in a 2.00 L vessel at 25 celsius, using ideal gas law.
To calculate the pressure of NH3 gas using the ideal gas law, we can use the formula:
PV = nRT
Where:
P is the pressure of the gas,
V is the volume of the vessel,
n is the number of moles of the gas,
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15 to the given temperature:
T = 25°C + 273.15 = 298.15 K
Now we can substitute the given values into the formula:
P * 2.00 L = 0.55 mol * 0.0821 L·atm/(mol·K) * 298.15 K
Now let's solve for P:
P = (0.55 mol * 0.0821 L·atm/(mol·K) * 298.15 K) / 2.00 L
P = 0.3358 atm
Therefore, the pressure of 0.55 mol of NH3 gas in a 2.00 L vessel at 25°C is approximately 0.3358 atm.
To calculate the pressure of NH3 gas using the ideal gas law, we can use the formula:
PV = nRT
Where:
P = pressure (in units of atm)
V = volume (in units of liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L.atm/(mol.K))
T = temperature (in units of Kelvin)
First, we need to convert the temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. So, 25°C + 273.15 = 298.15 K.
Now we have all the necessary values to calculate the pressure:
P = (nRT) / V
P = (0.55 mol * 0.0821 L.atm/(mol.K) * 298.15 K) / 2.00 L
Simplifying the equation:
P = (0.55 * 0.0821 * 298.15) / 2.00
P ≈ 9.09 atm
Therefore, the pressure of 0.55 mol of NH3 gas in a 2.00 L vessel at 25°C (298.15 K) is approximately 9.09 atm.