Bond dissociation energy of XY- X2 and Y2 all diatomic molecules are in the ratio of 1-1-0-5 and - Hf of XY is -100 kJ mol -1- The bond dissociation energy of X2 is 100x- Find the value of x-

The correct option is B 4 1 / 2 X_2 + 1 / 2 Y_2 ⟶ XY; nbsp; nbsp;Δ H = 100 nbsp;kJ Let the bond dissociation energy of X_2 , Y_2 and ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Enthalpy

Bond dissocia...

Question

Bond dissociation energy of $X Y$ , $X_{2}$ and $Y_{2}$ (all diatomic molecules) are in the ratio of $1 : 1 : 0.5$ and $Δ H_{f}$ of $X Y$ is $- 100 k J m o l^{- 1}$ . The bond dissociation energy of $X_{2}$ is $100 x$ . Find the value of x.

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 4
$\frac{1}{2} X_{2} + \frac{1}{2} Y_{2} ⟶ X Y; Δ H = - 100 k J$
Let the bond dissociation energy of $X_{2}$ , $Y_{2}$ and $X Y$ be
$a : \frac{a}{2} : a (t h e g i v e n r a t i o) k J m o l^{- 1}$ , respectively.
$∴$ $\frac{a}{2} + \frac{a}{4} - a = - 100$
$∴ a = 400$
$100 x = 400$
$x = 4$

Suggest Corrections

Similar questions

Q. If the bond dissociation energies of

X Y, X_{2}

and

Y_{2}

(all diatomic molecules) are in the ratio of

1 : 1 : 0.5

and

Δ H_{f}

for the formation of

X Y

- 200 k J {m o l}^{- 1}

, the bond dissociation energy of

X_{2}

will be:

Q. If the bond dissociation energy of

X Y, X_{2}, Y_{2}

(all are gaseous diatomic molecules) are in the ratio of 1:1:0.5 and enthalpy for the formation of

X Y

is -200kJ/mol. The bond dissociation energy of

X_{2}

will be:

Q. If the bond dissociation energies of

X Y, X_{2}

and

Y_{2}

(all diatomic molecules) are in the ratio of 1 : 1 : 0.5 and

Δ_{f} H

for the formation of

X Y

- 200 kJ/mol

, the bond dissociation energy of

X_{2}

will be:

Q. The bond dissociation energies of

X_{2}

Y_{2}

and

X Y

are in the ratio of 1 : 0.5 : 1.

△ H

for the formation of

X Y

is –200 kJ

m o l^{- 1}

. The bond dissociation energy of

X_{2}

will be

Q. The bond dissociation energies of

X_{2}, Y_{2}

and

X Y

are in the ratio of

1 : 0.5 : 1

Δ H

for the formation of

X Y

- 200 k J m o l^{- 1}

. The bond dissociation energy of

X_{2}

will be:

Join BYJU'S Learning Program

Bond dissociation energy of XY,X2 and Y2 (all diatomic molecules) are in the ratio of 1:1:0.5 and ΔHf of XY is −100kJmol−1. The bond dissociation energy of X2 is 100x. Find the value of x.

The correct option is B 412X2+12Y2⟶XY;ΔH=−100kJLet the bond dissociation energy of X2, Y2 and XY be a:a2:a(thegivenratio)kJmol−1, respectively.∴ a2+a4−a=−100∴a=400100x=400x=4

Bond dissociation energy of $X Y$ , $X_{2}$ and $Y_{2}$ (all diatomic molecules) are in the ratio of $1 : 1 : 0.5$ and $Δ H_{f}$ of $X Y$ is $- 100 k J m o l^{- 1}$ . The bond dissociation energy of $X_{2}$ is $100 x$ . Find the value of x.