A vessel of volume 5 litres contains `1.4 g` of `N_2` and `0.4 g` of He at `1500 K`. If `30 %` of the nitrogen molecules are dissociated into atoms then find the gas pressure.

A vessel of volume V = 5 litre contains 1.4 g nitrogen and 0.4g of He at 1500K . If 30% of the nitrogen molecules are disassociated into atoms then the gas pressure becomes (N)/(8)xx10^(5)N//m^(2) . Find N (Assume T constant). [R = (25)/(3)J//molK]

A vessel of volume V = 5 litre contains 1.4 g nitrogen and 0.4g of He at 1500K . If 30% of the nitrogen molecules are disassociated into atoms then the gas pressure becomes (N)/(8)xx10^(5)N//m^(2) . Find N (Assume T constant). [R = (25)/(3)J//molK]

A vessel of volume 5 litre contains 1.4 g of nitrogen at a temperature 1800K. The pressure of the gas is 30% of its molecules are dissociated into atoms at this temperature is:

A vessel of volume 5 litre contain 1.4 g of nitrogen at a temperature 1800 K. The pressure of the gas if 30% of its molecules are dissociated into atoms at this temperature is

A vessel of volume , V = 5.0 litre contains 1.4 g of nitrogen at a temperature T = 1800 K . Find the pressure of the gas if 30% of its molecules are dissociated into atoms into atmos at this temperature.

A vessel of volume V = 5.0 litre contains 1.4 gm of nitrogen at temperature T = 1800 K. Find the pressure of the gas if 30% of its molecule are dissociated into atom at this temperature.

A 5 L vessel contain 2.8 g of N_2 when heated to 1800 K, 30% molecules are dissociated into atoms

A 5-L vessel contains 1.4 g of nitrogen. When heated to 1800 K, 30% of molecules are dissociated into atoms. Calculate the pressure of the gas at 1800 K.