Home
Class 11
CHEMISTRY
The enthalpy change for the reaction N2(...

The enthalpy change for the reaction N2(g) + 3 H2(g) → 2 NH3(g) is -91.8 kJ at 298 K. Calculate the enthalpy of formation of ammonia?

Text Solution

Verified by Experts

The correct Answer is:
a
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level 1 (Q.93 To Q.122)|1 Videos

  • CHEMICAL EQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level 2|1 Videos

  • ATOMIC STUCTURE

    NARENDRA AWASTHI|Exercise level 2|1 Videos

  • DILUTE SOLUTION

    NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos

Similar Questions

Explore conceptually related problems

Heat change for a reaction N_(2)(g) + 3H_(2) (g) to 2NH_(3)(g) is - 92.2 kj/mol. Calculate the heat of formation of one mole of a ammonia.

For a reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))

Calculate the enthalpy change in the reaction, 4NH_(3) + 3O_(2) to 2N_(2) + 6H_(2) O at 298 K,given that the enthalpy of formation at 298 K for NH_(3) and H_(2)O are - 46.0 and - 286.0 KJ mol^(-1) respectively.

The enthaply change (Delta H) for reaction, N_(2) (g) + 3H_(2)(g) to 2NH_(3) (g) is 92.38 kj at 298 K. What is Delta U at 298 K ?

The enthalpy change for the transiton of liquid water to steam is 40.8 kj mol^(-1) at 373 K. Calculate the entropy change for the process.

Calculate the enthaply change in the reaction, CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O (i)The enthalpy change of formation of CH_(4) (g), CO_(2)(g) and H_(2)O (i) are - 74.8 kj mol^(-1), -393.5 KJ mol^(-1) and - 286 KJ mol^(-1) respectively.

The enthalpy change for the reaction, C_(2)H_(6)(g)rarr2C(g)+6H(g) is X kJ. The bond energy of C-H bond is :

The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of formation of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

Calculate the enthalpy change for the reaction H_(2)(g) + Cl_(2)(g) to 2HCl(g) . The bond enthalpy of H - H, Cl - Cl and H - Cl ar 437, 244 and 433 kj mol^(-1) respectively.

Equilibrium constant, K_(C ) for the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) at 500 K is 0.061 At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^(-1)N_(2), 2.0 "mol L"^(-1) H_(2) , 0.5 mol L^(-1) NH_(3) . Is the reaction at equilibrium ? If not, in which direction does the reaction tends to proceed to reach equilibirum ?