Home
Class 11
CHEMISTRY
On the basis of following equations the ...

On the basis of following equations the heat of dimerisation of `NO_(2)` will be
(i) `N_(2)+2O_(2)rarr2NO_(2) " "DeltaH=67.9 kJ`
(ii) `N_(2)+2O_(2)rarrN_(2)O_(4) " "DeltaH=09.3 kJ`

A

`+77.2kJ`

B

`-77.2kJ`

C

`-58.6kJ`

D

`+58.6kJ`

Text Solution

Verified by Experts

The correct Answer is:
C
So Heat of dimerisation of `2NO_(2) rarr N_(2)O_(4)` ...(iii)
Given
`2NO_(2) rarr N_(2) + 2O_(2) Delta H= -67.9kJ` ....(i)
`N_(2)O_(4) rarr N_(2) + 2O_(2) Delta H= -09.3 kJ` ...(ii)
On subtracting equation (ii) from (i) we will get equation (iii)
`2NO_(2)- N_(2)O_(4) rarr 0`
`2NO_(2) rarr N_(2)O_(4)` ..(iii)
So Heat of dimerisation of `NO_(2)= -67.9- (-09.3)kJ= -67.9+ 9.3= -58.6kJ`
Promotional Banner

Similar Questions

Explore conceptually related problems

S( rhombic ) + O_(2) rarr SO_(2)," " DeltaH=-297.5kJ S( monoclini ) + O_(2) rarr SO_(2), " "DeltaH=-300kJ This date indicates :

Using Le-Chatelier's principle, predict which conditions of termperature and pressure would give high yield of products in the following reactions: (i) CO_2(g) + H_2(g) hArr H_2O(g) + CO(g) " " DeltaH =+41 kJ (ii) 2SO_2(g) + O_2(g) hArr 2SO_3(g) " " DeltaH =-198 kJ (iii) N_2(g)+O_2(g) hArr 2NO(g) " " DeltaH =175 kJ

Calculate the standard enthalpy of reaction for the following reaction using the listed enthalpies of reaction : 3Co(s)+2O_(2)(g)rarrCo_(3)O_(4)(s) 2 Co(s)+O_(2)(g)rarr2CoO(s)," "DeltaH_(1)^(@)=-475.8 kJ 6CoO(s)+O_(2)(g)rarr2Co_(3)O_(4)(s),DeltaH_(2)^(@)=-355.0 kJ

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)

Calculate the heat of combustion of benzene form the following data: a. 6C(s) +3H_(2)(g) rarr C_(6)H_(6)(l), DeltaH = 49.0 kJ b. H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l), DeltaH =- 285.8 kJ c. C(s) +O_(2) (g) rarr CO_(2)(g), DeltaH =- 389.3 kJ

Calculate the heat of formation of n butane from the followinf data: a. 2C_(4)H_(10)(g) +13O_(2)(g) rarr 8CO_(2)(g) +10H_(2)O(l), DeltaH = - 5757.2 kJ b. C(s) +O_(2) (g)rarrCO_(2)(g), DeltaH =- 405.4 kJ c. 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l), DeltaH =- 572.4 kJ

Calculate the heat of combustion (in KJ) of methane from the following data (i) C ("graphite")+2H_(2)(g) rarr CH_(4) (g), DeltaH=-74.8 kJ (ii) C ("graphite")+O_(2) (g) rarr CO_(2) (g), DeltaH=-393.5 kJ (iii) H_(2(g))+1//2O_(2(g)) rarr H_(2)O_((l)), DeltaH=-286.2 kJ .