Chlorine gas, CL2 is used to purify water. How many moles of chlorine gas are in a 7.00L tank if gas has a pressure of 865mmHg anf temp of 24 degree celcius?
Chlorine gas, Cl, is used to purify water.How many moles of chlorine gas are in a 7.00 L tank if the gas has a pressure of 865 mmhg and a temperature of 24 C
To calculate the number of moles of chlorine gas (Cl2) in a 7.00L tank, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin
First, let's convert the given pressure from mmHg to atm:
1 atm = 760 mmHg
Convert mmHg to atm:
865 mmHg / 760 mmHg/atm = 1.14 atm
Next, convert the given temperature from Celsius to Kelvin:
Temperature in Kelvin = Temperature in Celsius + 273.15
T = 24°C + 273.15 = 297.15 K
Now, we can plug in the values into the ideal gas law equation:
PV = nRT
(1.14 atm)(7.00L) = n(0.0821 L·atm/mol·K)(297.15 K)
n = (1.14 atm * 7.00L) / (0.0821 L·atm/mol·K * 297.15 K)
n ≈ 0.27 moles
Therefore, there are approximately 0.27 moles of chlorine gas (Cl2) in the 7.00L tank.
To determine the number of moles of chlorine gas in the tank, we need to use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure in atmospheres
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin
First, let's convert the given pressure from mmHg to atm:
1 atm = 760 mmHg
Pressure (P) = 865 mmHg × (1 atm/760 mmHg) = 1.137 atm
Next, let's convert the given temperature from Celsius to Kelvin:
Temperature (T) = 24 °C + 273.15 = 297.15 K
Now we can rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
n = (1.137 atm) × (7.00 L) / (0.0821 L·atm/(mol·K)) × (297.15 K)
Calculating the expression, we get:
n ≈ 0.342 moles
Therefore, there are approximately 0.342 moles of chlorine gas in the 7.00L tank.