calculate the volume occupied by 7g of N2 gas at 27 degree c and 750mm Hg pressure
p v = n r t ... v = n r t / p
make sure the r value has the correct units
To calculate the volume occupied by 7g of N2 gas at 27 degrees Celsius and 750 mmHg pressure, you can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
To start, you need to convert grams of N2 gas to moles. The molar mass of N2 is 28 g/mol. Therefore, dividing the given mass by the molar mass will give you the number of moles:
n = mass / molar mass
n = 7g / 28 g/mol
n = 0.25 mol
Next, you will need to convert the temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature:
T = 27°C + 273.15
T = 300.15 K
Now you have all the values needed to calculate the volume. The gas constant, R, is 0.0821 L.atm/(mol.K) for pressure in atm and volume in liters. However, since you are given the pressure in mmHg, you need to convert it to atm by dividing it by 760:
P = 750 mmHg / 760 mmHg/atm
P = 0.987 atm
Now you can plug in the values into the equation and solve for the volume:
PV = nRT
V = (nRT) / P
V = (0.25 mol * 0.987 atm * 300.15 K) / 0.987 atm
V ≈ 74.6 L
Therefore, the volume occupied by 7g of N2 gas at 27 degrees Celsius and 750 mmHg pressure is approximately 74.6 liters.
As we know that PV =nR T .................(1)eqn.
First of all, we will find n =given mass / molar mass
Then, put values in equation no. (1)
Make sure about value of R
Answer will be 6.239litres