Calculate the change in pressure ( in atm) when 2 mole of `NO` and `16 g O _(2)` in `6.25` litre originally at `27^(@)C` react to produce the maximum quantity of `NO_(2)` possible according to the equation.
`( ` Take `R=(1)/(12)` ltr. Atm`//`mol K `)`
`2NO(g)+O_(2)(g) hArr 2NO_(2)(g)`

Calculate the change in pressure when 1.04 mole of NO and 20.0gO_(2) in a 20.0L vessel originally at 27^(@)C react to produce maximum quantity of NO_(2(g)) according to reaction 2NO_((g)) +O_(2(g))rarr2NO_(2(g)) .

2 moles of NO(g) and 16 gm of O_(2)(g) were mixed in a 6.25 litre vessel at 27^(@)C temperature to produce maximum amount of NO_(2)(g) 2NO(g)+O_(2)(g)rarr2NO_(2)(g) ("Use" :R=(1)/(12) "L-atm mol"^(-1)K^(-1)) Calculate change in pressure (in atm) due to this reaction.

Density of dry air ( only N_(2) and O_(2)) is 1.24g litre^(-1) at 760 m m and 300 K . Find the partial pressure of N_(2) gas in aire. ( Take R=(1)/(12) litre litre atm // mol K, mol. Wt. of N_(2) =28)

Density of dry air ( only N_(2) and O_(2)) is 1.24g litre^(-1) at 760 m m and 300 K . Find the partial pressure of N_(2) gas in aire. ( Take R=(1)/(12) litre litre atm // mol K, mol. Wt. of N_(2) =28)

Calculate the mass of sucrose C_(12)H_(22)O_(11)(s) produced by mixture 78 g of C(s) , 11 g of H_(2)(g) & 67.2 litres of O_(2)(g) at 0^(@)C and 1 atm according to given reaction (unbalanced)?

What volume of gas will be formed at 523 K and 1 atm pressure by the explosive decomposition of 5 g of the ammonium nitrate, according to the given equation? 2NH_(4)NO_(3)(s)=2N_(2)(g)+O_(2)(g)+4H_(2)O(g)

N_(2)O_(3) dissociates into NO and NO_(2) . At equilibrium pressure of 3 atm , all three gases were found to have equal number of moles in a vessel. In another vessel, equimolormixture of N_(2)O_(3), NO and NO_(2) are taken at the same temperature but at an initial pressure of 9 atm then find the partial pressure of NO_(2) (in atm ) at equilibrium in second vessel! N_(2)O_(3)(g) hArr NO(g) + NO_(2) (g)