A generic gas, X, is placed in a sealed glass jar and decomposes to from gaseous Y and solid Z. How are these equilibrium quantities affected by the initial amount of X(g) placed in the container? Assume constant temperature. Changes if initial [X] changes Constant regardless of initial [X] mass of Z at equilibrium [Y] at equilibrium [Y]/[X] at equilibrium [X] at equilibrium [X]2/[Y] at equilibrium total pressure at equilibrium

The answer given by Casey12 is incorrect. The correct answer

is:

Changes if initial [x] changes: mass of Z at

equilibrium, [x] at equilibrium, [y] at equilibrium, [y]/[x] at

equilibrium and total pressure at equilibrium.

Constant regardless of inital [x]: [x]^2/[y] at

equilibrium

The decomposition reaction for the generic gas X is as follows The equilibrium constant for the reaction is as follows: Y1[Z As per the le chatelier principle, increase in reactant concentration will shift equilibrium towards right side. If concentration of X changes then concentration of Y and Z also changes to reach the equilibrium Mass of Z is directly proportional to the concentration of Z, so mass of Z changes if initial concentration changes If initial concentration of X changes then concentration of X at equilibrium also changes If concertation of X and Y changes, automatically changes At equilibrium, there is no change in the ratio of concentration of products to the reactants if initial concentration changes. Therefore, 1ที่ is constant with change in initial concentration of X

The total pressure of the system at equilibrium changes with initial concentration because as the concentration changes then number of moles also changes. If number of moles of X changes then total pressure of the system changes. Changes if initial [X changes Constant regardless of initial [X] Mass of Z at equilibrium Y at equilibrium X at equilibrium [Y/X] at equilibrium Total pressure at equilibrium [xF //Υ1 at equilibrium

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