Calculate the volume occuiped by 7g of nitrogen gas at 27degree centigrade and 750 mm of Hg pressure?
assuming the gas is ideal, we can use the ideal gas law:
PV = nRT
where
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant = 0.0821 L-atm/mol-K
T = temperature (in K)
note that n = mass given / molar mass. The molar mass of nitrogen (diatomic gas) is equal to 28 g/mol. Also, K = C + 273 and 1 atm = 760 mm Hg.
substituting,
(750/760)*(V) = (7/28)*(0.0821)*(27+273)
now solve for V. units in liters.
hope this helps~ :)
7.8litres
To calculate the volume occupied by a gas, we can use the ideal gas law equation: PV = nRT.
Here's how you can calculate the volume:
Step 1: Convert the given temperature to Kelvin.
To convert from Celsius to Kelvin, add 273.15 to the given temperature.
27 degrees Celsius + 273.15 = 300.15 Kelvin
Step 2: Convert the given pressure to atm.
1 atm = 760 mmHg, so we divide 750 mmHg by 760 mmHg/atm.
750 mmHg / 760 mmHg/atm = 0.98684 atm
Step 3: Calculate the number of moles of nitrogen gas.
We can use the molar mass of nitrogen gas to find the number of moles. The molar mass of nitrogen (N2) is approximately 28 g/mol.
Number of moles = Given mass / Molar mass
Number of moles = 7 g / 28 g/mol = 0.25 mol
Step 4: Plug the values into the ideal gas law equation.
PV = nRT
Substituting the given values:
(0.98684 atm) * V = (0.25 mol) * (0.0821 L atm/mol K) * (300.15 K)
Step 5: Solve for V (volume).
V = (0.25 mol * 0.0821 L atm/mol K * 300.15 K) / 0.98684 atm
V ≈ 6.298 L
Therefore, the volume occupied by 7g of nitrogen gas at 27 degrees Celsius and 750 mmHg of pressure is approximately 6.298 liters.