Calculate the volume occupied by 5.25 g of nitrogen at 26*c [temperature] and 74.2 cm of pressure.?

PV = nRT

PV=nrT

V= nrT/ P

n = 5.25/14 (mass of nitrogen)
= 0.375
R = 0.0821
T = 27+273 = 299
P = 74.2 cm x 10 = 742mm of pressure

V=nRT/P

ANS=> 0.012 dm3

ChuLbuLi has erred.

mass N is 14. mass N2 is 28; therefore,
n = 5.25/28 = ?
P must be in atmosphere if you use R as 0.08206 L*atm/mol*K.
P = 74.6 cm/76.0 cm = ? atm.

This answer wrong . And stop making fool of students , if you don't know anything . The correct answer is 4.71 litres

Kapil Saini , IITian (IIT Bombay)

To calculate the volume occupied by the nitrogen, we can use the ideal gas law equation:

PV = nRT

Where:
P is the pressure of the gas in atmospheres (atm)
V is the volume of the gas in liters (L)
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 (K)

First, we need to convert the given temperature from degrees Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature.

T = 26°C + 273.15 = 299.15 K

Next, we need to calculate the number of moles of nitrogen using its mass and molar mass.

The molar mass of nitrogen (N₂) is 28 g/mol.

Using the molar mass, we can calculate the number of moles:

n = mass / molar mass
n = 5.25 g / 28 g/mol

Now we have all the required values to calculate the volume.

V = (nRT) / P
V = (5.25 g / 28 g/mol) * (0.0821 L·atm/(mol·K)) * (299.15 K) / 74.2 atm

Calculating the expression:

V = (5.25 * 0.0821 * 299.15) / (28 * 74.2) L

Finally, we can solve for V:

V ≈ 0.645 L

Therefore, the volume occupied by 5.25 g of nitrogen at 26°C and 74.2 cm of pressure is approximately 0.645 liters.