Home
Class 11
CHEMISTRY
If the bond energies of H-H, Br-Br and H...

If the bond energies of H-H, Br-Br and HBr are `433, 192 and 364 kJ mol^(-1)` respectively, then `DeltaH^@` for the reaction :
`H_(2(g)) + Br_(2(g)) rarr 2HBr_((g))` is

A

`-261kJ`

B

`+103kJ`

C

`+261kJ`

D

`-103kJ`

Text Solution

Verified by Experts

The correct Answer is:
D
Promotional Banner

Similar Questions

Explore conceptually related problems

Given that bond energies of N=N,H-H and N-H bonds as 945, 436 and 391 kJ/ mol respectively ,the enthalpy of the reaction N_(2)(g)+3H_(2)(g)+to2NH_(3)(g), is

In the reaction 2Br^(-) + X_(2) rarr Br_(2) + 2X^(-) , X_(2) is

Given Delta H_r ^@ for CO_2(g) , CO_(g) and H_2O(g) are -393.5, -110.5 and -241.8 KJ mol^-1 respectively. The Delta H_r^@ (in KJ mol^-1] for the reaction CO_2(g) + H_2(g) rightarrow CO_(g) + H_2O(g) is

If the standard molar enthalpy of formation of SO _(2 (g)) and SO _(3(g)) is - 296 . 82 kJ mol ^(-1) and -395 . 72 kJ mol ^(-1) respectively, then enthalpy change for the reaction in kJ mol ^(-1) , SO _(2 (g)) + (1)/(2) O _(2 (g)) to SO _(3(g)) , is

Heat of formation of 2 moles of NH_(3)(g) " is" -90 kJ l bond energies of H-H and N-H bonds are 435 kJ and 390 kJ mol^(-1) respectively. The value of the bond energy of N -= N is (1000- (x^(2) + x +25)) kJ/mol What is x ?

Heat of formation of water and heats of combustion of ethylene and acetylene are respectively 286, -1410 and -1299 kJ mol^(-1) , Calculate the heat of the reaction, C_2H_(2(g)) + H_(2(g)) to C_(2)H_(4(g)) .

The standard enthalpies of formation of H_(2)O_(2(l)) and H_(2)O_((l)) are -187.8kJ "mole"^(-1) and -285.8 kJ "mole"^(-1) respectively. The DeltaH^(0) for the decomposition of one mole of H_(2)O_(2(l)) " to" H_(2)O_((l)) and O_(2(g)) is

If DeltaH_(f)^(0) " for" H_(2)O_(2(l)) and H_(2)O_((l)) " are " -188 kJ mol^(-1) and -286 kJ mol^(-1) , what will be the enthalpy change of the reaction 2H_(2)O_(2(l)) rarr 2H_(2)O_((l)) + O_(2(g)) = ?