Home
Class 11
CHEMISTRY
Consider the reaction X(g) hArr Y(g)+Z...

Consider the reaction
`X(g) hArr Y(g)+Z(g)`
When the system is at equilibrium at `100^(@)`, the concentrations are found to be `[X]=0.2 M, [Y]=[Z]=0.4 M`
a. If the pressure of the container is suddenly halved at `100^(@)C`, find equilibrium concentration.
b. If the pressure of the container is suddenly doubled at `100^(@)C`, find the equilibrium concentration

Text Solution

AI Generated Solution

To solve the problem step-by-step, we will analyze the equilibrium reaction and how changes in pressure affect the concentrations of the reactants and products. ### Given Reaction: \[ X(g) \rightleftharpoons Y(g) + Z(g) \] ### Initial Concentrations at Equilibrium: - \([X] = 0.2 \, M\) - \([Y] = 0.4 \, M\) ...
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

Consider the reaction: A(g) hArr B(g)+C(g) When the system is at equilibrium at 200^(@)C , the concentrations are found to be: [A]=0.20 M, [B]=0.30 M, [C]=0.30 M a. If the volume of the container is suddenly doubled at 200^(@)C , find the equilibrium concentrations. b. If the volume of the container is suddenly halved (instead of being doubled in part (i) at 200^(@)C , find the equilibrium concentrations.

Consider the imaginary equilibrium 4A(g)+5B(g)hArr 4X(g)+6Y(g) , The unit of equilibrium constant K_(C) is

In the system X+2Y⇌Z, the equilibrium concentrations are, [X]=0.06 mol L −1 ,[Y]=0.12 mol L −1 ,[Z]=0.216 mol L −1 . Find the equilibrium constant of the reaction.

For the reaction, 2SO_(2(g))+O_(2(g))hArr2SO_(3(g)) What is K_(c) when the equilibrium concentration of [SO_(2)]=0.60M,[O_(2)]=0.82Mand[SO_(3)]=1.90M ?

For the reaction, A(g)+2B(g)hArr2C(g) one mole of A and 1.5 mol of B are taken in a 2.0 L vessel. At equilibrium, the concentration of C was found to be 0.35 M. The equilibrium constant (K_(c)) of the reaction would be

The reaction, 2A(g) + B(g)hArr3C(g) + D(g) is begun with the concentration of A and B both at an intial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

For the reaction H_(2)(g) + I_(2)(g)hArr2HI(g) at 721 K the value of equilibrium constant (K_(c)) is 50. When the equilibrium concentration of both is 0.5 M, the value of K_(p) under the same condtions will be

For , A + B hArr C. the equilibrium concentration of A and B at a temperäture are 15 mol lit^(-1) When volume is doubled the reaction has equilibrium concentration of A as 10 mol lit^(-1) then

In the system X+2YhArrZ , the equilibrium concentration are, [X]=0.06" mol L"^(-1),[Y]=0.12" mol L"^(-1) , [Z]=0.216" mol L"^(-1) . Find the equilibrium constant of the reaction.

For a reversible reaction: X+2Y rarr 2Z , the equilibrium concentrations of X, Y and Z are 0.32, 0.40 and 0.35 moles L^(-1) respectively at 25^(@)C . a. If unitially the system contained only X and Y and then reached the state of equilibrium, what were the initial concentrations of X and Y . b. If at the start only X and Z were present, what were the initial concentrations?