Home
Class 11
CHEMISTRY
One mole of nitrogen is mixed with three...

One mole of nitrogen is mixed with three moles of hydrogen in a 4 litre container. If 0.25 per cent of nitrogen is converted into ammonia by the following reaction
` N_2(g) +3H_2 hArr 2NH_3(g)`
calculate the equilibrium constant of the reaction in concentration units. What will be the value of K for the following reaction?
` (1)/(2) N_2 (g) + (3)/(2) H_2 hArr NH_3 (g)`

Text Solution

Verified by Experts

The correct Answer is:
A, C
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Subjective type|1 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives (True/False)|4 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

In the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) the value of the equilibrium constant depends on

In the reaction N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g) , the value of the equlibrium constant depends on

1 mol of N_(2) is mixed with 3 mol of H_(2) in a litre container. If 50% of N_(2) is converted into ammonia by the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , then the total number of moles of gas at the equilibrium are

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 litre vessel. 20% of nitrogen is converted into NH_(3) . Then K_(C) for the (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)hArr NH_(3) is

For the reversible reaction N_2(g) +3H_2(g) hArr 2NH_3(g) +"Heat" The equilibrium shifts in forward directions.

The value of the equilibrium constant K for the reaction H_2(g) +I_2(g) hArr 2Hl(g) " is " 48 " at " 717 K. Find out the value of K for the following reaction at Hl(g) hArr (1)/(2) H_2(g) + (1)/(2) I_2(g)

What is concentration quotient ? Write concentration quotients for the the following reactions: N_2(g) + 3H_2(g) hArr 2NH_3(g)

For the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g), DeltaH=?

For the reversible reaction N_(2) (g) +3H_(2) (g) hArr 2NH_(3) (g) + " Heat" The equilibrium shifts in forward direction

For the reaction, N_2[g] + 3H_2[g] hArr 2NH_3[g] , Delta H = …

Knowledge Check

  • In the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) the value of the equilibrium constant depends on

    A
    volume of the reaction vessel
    B
    total pressure of the system
    C
    the initial concentration of nitrogen and hydrogen
    D
    the temperature

  • For the reversible reaction N_2(g) +3H_2(g) hArr 2NH_3(g) +"Heat" The equilibrium shifts in forward directions.

    A
    by increasing the concentration of `NH_3 (g)`
    B
    by decreasing the pressure
    C
    by decreasing the concentration of `N_2(g) and H_2(g)`
    D
    by increasing pressure and decreasing temperature

  • For the reaction, N_2[g] + 3H_2[g] hArr 2NH_3[g] , Delta H = …

    A
    `DeltaU - 2RT`
    B
    `DeltaU + 2RT`
    C
    `DeltaU + RT`
    D
    `DeltaU - RT`.