Home
Class 12
CHEMISTRY
Heat of solution of BaCl(2).2H(2)O=200 k...

Heat of solution of `BaCl_(2).2H_(2)O=200 kJ mol^(-1)`
Heat of hydration of `BaCl_(2)=-150 kJ mol^(-1)`
Hence heat of solution of `BaCl_(2)` is

A

350 kJ

B

50 kJ

C

`-350 kJ`

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
B
`BaClcdot 2H_2O + aq to BacL_(2)(aq) DeltaH_(1) = 200 kJmol^(-1)` ....... (i)
`BaCl_(2) + aq to Bacl_(2) cdot 2 H_(2)O Delta H_(2) = -150 kJ mol^(-1)…..(ii)`
Adding equation (i) and (ii)
`DeltaH_(3) = DeltaH_(1) + DeltaH_(2)`
Heat of solution of `Bacl_(2) = 200 + (-500) = 50 kJ`
Promotional Banner

Similar Questions

Explore conceptually related problems

Lattice energy of NaCl_((s)) is -788kJ mol^(-1) and enthalpy of hydration is -784kJ mol^(-1) . Calculate the heat of solution of NaCl_((s)) .

Enthalpies of solution of BaCI_(2). 2H_(2)O and BaCI_(2) are 8.8 and -20.6 kJ mol^(-1) respectively.Calculate the heat of hydration of BaCI_(2). 2H_(2)O

The heat of solution of BaCl_(2) .2H_(2) O_((s)) and anhydrous BaCl_(2(s)) are 8.37" kJ mol"^(–1) and –20.62" kJ mol"^( –1) respectively then heat of hydration of BaCl_(2(s)) will be :-

Enthalpies of solution of BaCl_(2)(s) and BaCl_(2).2H_(2)O(s) are -20 kJ//"mole" and 8.0kJ//"mole" respectively. Calculate heat of hydration of BaCl_(2)(s) .

If the heats of formation of C_(2)H_(2) and C_(6)H_(6) are 230 kJ mol^(-1) and 85 kJ mol^(-1) respectively, the DeltaH value for the trimerisation of C_(2)H_(2) is

The heat of solution of one mole of Na_2SO_4.10H_2O is -78.7 kJ ,and that of dehydration , -81.6 kJ. The heat of solution (kJ) of anhydrous sodium sulphate is

The stadard heats of formation of NO_(2)(g) and N_(2)O_(4) (g) are 33.5 and 8.4 kJ mol^(-1) respectively. The heat of dimerisation of NO_(2) in kJ is