Which one of the following pairs of gases contain the same number of molecules?
8 g of \(CO_{2}\) and 8 g of \(N_{2}\)
18 g of \(NO_{2}\) and 15 g \(SO_{2}\)
64 g of \(O_{2}\) and 56 g of \(N_{2}\)
32 g of \(O_{2}\) and 32 g of \(N_{2}\)

A gaseous mixture contains CO_(2) (g) and N_(2)O(g) in 2:5 ratio by mass. The ratio of the number of molecules of CO_(2)(g) and N_(2)O(g) is:

A vessel of volume 4 litres contains a mixture of 8g of O_(2), 14g of N_(2) and 22 g of CO_(2) at 27^(0)C . The pressure exerted by the mixture is

A gaseous mixture contains 1 g of H_(2) , 4 g of He , 7 g of N_(2) and 8 g of O_(2) . The gas having the highest partial pressure is :-

With the following infromations, determine standard Gibb's free energy of formation of N_(2)O_(4)(g). (1)/(2)N_(2)(g) + (1)/(2)O_(2)(g) rarr NO(g) " "DeltaG^(@)=86.6 KJ " ""….."(i) NO(g) + (1)/(2)O_(2)(g) rarr NO_(2)(g) " "DeltaG_(@) =34.82 KJ " ""....."(ii) 2NO_(2)(g) rarr N_(2)O_(4)(g) " G= 5.77 ""....."(iii)

2.8 g of N_(2) 0.40 g of H_(2) and 6.4 g of O_(2) are placed in a container of 1.0 L capacity at 27^(@) C. The total pressure in the container is

The total pressure of a gaseous mixture of 2.8 g N_(2) , 3.2 g O_(2) , and 0.5 g H_(2) is 4.5 atm . Calculate the partial pressure of each gas.