Home
Class 11
CHEMISTRY
For the formation of ammonia the equilib...

For the formation of ammonia the equilibrium constant data at `673K` and `773 K`, respectively, are `1.64xx10^(-4)` and `1.44xx10^(-5)` respectively. Calculate heat of reaction `(R=8.314 J K^(-1) mol^(-1))`

Text Solution

Verified by Experts

The given data are:
`K_(1)=1.64xx10^(-4), T_(1)=673 K`
`K_(2)=1.44xx10^(-5), T_(2)=773 K`
Using van't Hoff equation,
`log(K_(P_(2))/K_(P_(1)))=(DeltaH)/(2.303R)((T_(2)-T_(1))/(T_(2)T_(1)))`
`:. log (1.44xx10^(-5))/(1.64xx10^(-4))=(DeltaH)/(8.314xx2.303)((773-673)/(773xx673))`
`-1.0565=(DeltaH)/(19.147)(100/520229)`
`:. DeltaH=(-1.0565xx19.147xx520229)/(100)`
`=-105216 J= -105.216 kJ`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

The equilibrium constants for the reaction Br_(2)hArr 2Br at 500 K and 700 K are 1xx10^(-10) and 1xx10^(-5) respectively. The reaction is:

For a reaction , Br_(2) hArr 2 Br, the equilibrium constant at 600K and 800 K are respectively 6.1 xx 10^(-12) and 1.0 xx 10^(-7) . What is the nature of the reaction?

The equilibrium constants for A_2 (g) hArr 2A(g) at 400 k and 600 k are 1xx 10^(-8) and 1 xx 10^(-2) respectively . The reaction is

The K_(a) for formic acid and acetic acid are 2.1 xx 10^(-4) and 1.1 xx 10^(-5) , respectively. Calculate relative strength of acids

The equilibrium constants for the reaction, A_2hArr2A A at 500K and 700K are 1xx10^(-10) and 1xx10^(-5) . The given reaction is

The rate constant of a reaction is 1.5 xx 10^(7)s^(-1) at 50^(@) C and 4.5 xx 10^(7)s^(-1) at 100^(@) C. Calculate the value of activation energy for the reaction (R=8.314 J K^(-1)mol^(-1))