How many moles of chloroform, CHCl^3, are required to fill a 253-ml flask at 100.0 degrees Celsuis and 940 torr?
Use PV = nRT
T must be in kelvin.
To find out how many moles of chloroform (CHCl3) are required to fill a 253 mL flask at 100.0 degrees Celsius and 940 torr, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
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 temperature from Celsius to Kelvin:
T = (100.0 + 273.15) K
T = 373.15 K
Next, let's convert the given volume from milliliters to liters:
V = 253 mL
V = 253 mL * (1 L/1000 mL)
V = 0.253 L
Now we can plug in the values into the ideal gas law equation:
PV = nRT
n = (PV) / (RT)
n = (940 torr * 0.253 L) / (0.0821 L·atm/mol·K * 373.15 K)
Let's calculate the value:
n = (237.82) / (30.616)
n ≈ 7.7642 moles
Therefore, approximately 7.7642 moles of chloroform (CHCl3) are required to fill a 253 mL flask at 100.0 degrees Celsius and 940 torr.
To find the number of moles of chloroform (CHCl3) required to fill a 253-ml flask at a specific temperature and pressure, we need to use the ideal gas law equation:
PV = nRT
Where:
P is the pressure in atmospheres
V is the volume in liters
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, let's convert the given volume from mL to liters:
253 mL = 0.253 L
Next, we need to convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T = 100.0 + 273.15 = 373.15 K
Now, we can calculate the number of moles using the ideal gas law equation. However, we need to convert the given pressure from torr to atm:
1 atm = 760 torr
940 torr = 940/760 atm ≈ 1.237 atm
Now, we can substitute the values into the ideal gas law equation:
(1.237 atm) * (0.253 L) = n * (0.0821 L·atm/(mol·K)) * (373.15 K)
Simplifying the equation:
0.3131 = 30.636515 * n
Now, isolate n by dividing both sides by 30.636515:
n ≈ 0.3131 / 30.636515
Calculating the value:
n ≈ 0.0102 moles
Therefore, approximately 0.0102 moles of chloroform (CHCl3) are required to fill the 253-ml flask at a temperature of 100.0 degrees Celsius and a pressure of 940 torr.
Ideal law
0.0099 mol