Home
Class 11
CHEMISTRY
What is % dissociation of H(2)S if 1 "mo...

What is `%` dissociation of `H_(2)S` if `1` "mole" of `H_(2)S` is introduced into a `1.10 L` vessel at `1000 K`? `K_(c)` for the reaction
` `2H_(2)S(g) hArr 2H_(2)(g)+S_(2)(g)` is `1xx10^(-6)

Text Solution

AI Generated Solution

To find the percentage dissociation of \( H_2S \) in the given reaction, we can follow these steps: ### Step 1: Write the balanced chemical equation The decomposition of hydrogen sulfide can be represented as: \[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \] ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 7.2|40 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

Calculate the precentage dissociation of H_(2)S(g) if 0.1 mol of H_(2)S is kept in a 0.5 L vessel at 1000 K . The value of K_(c ) for the reaction 2H_(2)ShArr2H_(2)(g)+S_(2)(g) is 1.0xx10^(-7).

Calculate the percent dissociation of H_(2)S(g) if 0.1 mol of H_(2)S is kept in 0.4 L vessel at 1000 K . For the reaction: 2H_(2)S(g) hArr 2H_(2)(g)+S(g) The value of K_(c ) is 1.0xx10^(-6)

What is the unit of K_(p) for the reaction ? CS_(2)(g)+4H_(2)(g)hArrCH_(4)(g)+2H_(2)S(g)

A mixture of 1.57 mol of N_(2), 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

A mixture of 1.57 mol of N_(2), 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

Write the equilibrium constant of the reaction C(s)+H_(2)O(g)hArrCO(g)+H_(2)(g)

If 0.2 mol of H_(2)(g) and 2.0 mol of S(s) are mixed in a 1.0 L vessel at 90^(@)C , the partial pressure of H_(2)S(g) formed according to the reaction H_(2)(g)+S(s)hArr H_(2)S(g),K_(p) at 363K=6.78xx10^(-2) would be

A mixture of 2 moles of N_2,2.0 moles of H_2 and 10.0 moles of NH_3 is introduced into a 20.0 L reaction vessel at 500 K . At this temperature, equilibrium constant K_c is 1.7 xx 10^2 , for the reaction N_2(g) +3H_2(g) hArr 2NH_3(g) (i) is the reaction mixture at equilibrium ? (ii) if not, what is the direction of the reaction ?

What is DeltaG^(ɵ) for the following reaction? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g), K_(p)=4.42xx10^(4) at 25^(@)C

What is DeltaG^(ɵ) for the following reaction? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g), K_(p)=4.42xx10^(4) at 25^(@)C