Home
Class 12
CHEMISTRY
Calculate standard enthalpy for the reac...

Calculate standard enthalpy for the reaction at 298K: `C_(2)H_(5)Cl(g)toC_(2)H_(4)(g)+HC l(g)`. Given: `DeltaH^(0)(C-H)=413kJ*mol^(-1),DeltaH^(0)(C-C)=346kJ*mol^(-1)`,
`DeltaH^(0)(C=C)=611kJ*mol^(-1),DeltaH^(0)(C-Cl)=339kJ*mol^(-1)`,
`DeltaH^(0)(H-Cl)=432kJ*mol^(-1)`.

Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    CHHAYA PUBLICATION|Exercise WARM UP EXERCISE|119 Videos

  • CHEMICAL THERMODYNAMICS

    CHHAYA PUBLICATION|Exercise QUESTION ANSWER ZONE FOR BOARD EXAMINATION (VERY SHORT ANSWER TYPE)|26 Videos

  • CHEMICAL KINETICS

    CHHAYA PUBLICATION|Exercise EXERCISE (NUMERICAL PROBLEMS)|37 Videos

  • CHEMISTRY IN EVERYDAY LIFE

    CHHAYA PUBLICATION|Exercise PRACTICE SET 15|15 Videos

Similar Questions

Explore conceptually related problems

Calculate the enthalpy for the reaction at 27^0C . C_2 H_5 Cl (s) rarr C H_4 (g) +HCl (g) , Delta H^0(C -C) = 350 kjmol ^(-1) H^0(C-H) = 410 Kjmol^(-)1 , Delta H(C = C) =600 kjmol^(-1) -Delta H^0(C-Cl) = 340^0k jmol^(-1) , Delta H^0(H-Cl) = 430 kjmol^(-1) .

Calculate the value of standard reaction enthalpy for the following reaction : C_2H_5Cl (g) rarr C_2H_4 (g) + HCl (g) at 298 K temperature.Given that DeltaH^@ (C-H) = 413 KJ mol^-1, DeltaH^@ (C-C) = 346 KJ mol^-1 ,DeltaH^@ (C=H) =611 KJ mol^-1, DeltaH^@ (C-CI) = 339 KJ mol^-1 DeltaH^@ (H-Cl) = 432 KJ- mol^-1 .

Determine the standard enthalpy of formation of isoprene(g) at 298K temperature. Given: at 298K, DeltaH^(0)(C-H)=413kJ*mol^(-1) DeltaH^(0)(H-H)=436kJ*mol^(-1) DeltaH^(0)(C-C)=346kJ*mol^(-1) , DeltaH^(0)(C=C)=611kJ*mol^(-1) , C("graphite, s")toC("graphite, g"), DeltaH^(0)=717kJ*mol^(-1)

Draw the Born-Haber cycle for the formation of LiF(s) from its elements and using this cycle calculate the lattice enthalpy of LiF(s). Given: DeltaH_(f)^(0)[LiF(s)]=-617kJ*mol^(-1) , DeltaH_(sub)=+161kJ*mol^(-1),DeltaH^(0)(F-F)=+159kJ*moL^(-1) , IE_(1)=+520kJ*mol^(-1),EA of F=-328kJ*mol^(-1) .

Calculate the DeltaG^0 for the reaction N_2(g) + O_2(g) * 2NO(g) Given DeltaH^0 =180.5 K.J , and DeltaS^0 = 15 J at 25^@C .

DeltaH value for the given reactions at 25^(@)C are- C_(3)H_(8)(g)to3C(s)+4H_(2)(g),DeltaH^(0)=103.8kJ*mol^(-1) 2H_(2)(g)+O_(2)(g) to 2H_(2)O(l),DeltaH^(0)=-571.6kJ*mol^(-1) C_(2)H_(6)(g)+(7)/(2)O_(2)(g)to2CO_(2)(g)+3H_(2)O(l),DeltaH^(0)=-1560kJ*mol^(-1) CH_(4)(g)+2O_(2)(g) to CO_(2)(g)+2H_(2)O(l),DeltaH^(0)=-890kJ*mol^(-1) C(s)+O_(2)(g) to CO_(2)(g),DeltaH^(0)=-393.5kJ*mol^(-1) Calculate DeltaH^(0) for the reaction at 25^(@)C C_(3)H_(8)(g)+H_(2)(g)toC_(2)H_(6)(g)+CH_(4)(g)

Diborane [B_(2)H_(6)(g)] is used as a very effective fuel for rockets. Calculate the heat of combustion of diborane for the following reaction: B_(2)H_(6)(g)+3O_(2)(g)toB_(2)O_(3)(g)+3H_(2)O(g) Given: (1) 2B(s)+(3)/(2)O_(2)(g)toB_(2)O_(3) (s),DeltaH^(0)=-1273kJ*mol^(-1) (2) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH^(0)=-285.8kJ*mol^(-1) . (3) H_(2)O(l)toH_(2)O(g),DeltaH^(0)=+44kJ*mol^(-1) (4) 2B(s)+3H_(2)(g) to B_(2)H_(6)(g),DeltaH^(0)=+36kJ*mol^(-1) .

Calculate the bond energy of O-H bond in H_(2)O(g) at the standard state from the following data: (1) H_(2)(g) to 2H(g),DeltaH^(0)=436kJ*mol^(-1) (2) (1)/(2)O_(2)(g)toO(g),DeltaH^(0)=249k*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(g),DeltaH_(f)^(0)[H_(2)O(g)]=-241.8kJ*mol^(-1) .

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: (1) CH_(3)OH(l)+(3)/(2)O_(2)(g)toCO_(2)(g)+2H_(2)O(l),Delta_(r)H^(0)=-726kJ*mol^(-1) (2) C(s)+O_(2)(g) to CO_(2)(g),Delta_(c)H^(0)=-393kJ*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),Delta_(f)H^(0)=-286kJ*mol^(-1) .

If (1)/(2)AtoB,DeltaH=+150kJ*mol^(-1),3B to 2C+D,DeltaH=-125kJ*mol^(-1),E+Ato2D,DeltaH=+350kJ*mol^(-1) then DeltaH of the reaction B+D to E+2C will be-