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1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction?
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1 mole of x and Y are allowed to react in a 2 litre container when equ...
**Calculation of Equilibrium Constant**
To calculate the equilibrium constant for the given reaction, we need to use the concentration of Z at equilibrium and the stoichiometric coefficients of the reactants and products.
**Given Data**
- 1 mole of X and Y are allowed to react.
- The reaction is: 2X + Y = Z
- The volume of the container is 2 litres.
- The concentration of Z at equilibrium is 0.2 M.
**Step-by-Step Solution**
**Step 1: Write the Balanced Chemical Equation**
2X + Y = Z
**Step 2: Write the Equilibrium Expression**
Kc = [Z] / ([X]^2 [Y])
**Step 3: Determine the Concentrations**
- The initial concentration of X and Y is 1 mole/2 L = 0.5 M.
- Let the equilibrium concentration of X and Y be x M.
- At equilibrium, the concentration of Z is 0.2 M.
**Step 4: Substitute the Values in the Equilibrium Expression**
Kc = [Z] / ([X]^2 [Y])
Kc = (0.2) / (x^2 * (0.5 - x))
**Step 5: Solve for x**
At equilibrium, the number of moles of Z formed is equal to the number of moles of X and Y consumed. Therefore,
2x = [Z] * 2 L
2x = 0.2 * 2
x = 0.1 M
**Step 6: Substitute the Value of x in the Equilibrium Constant Expression**
Kc = (0.2) / (0.1)^2 * (0.5 - 0.1)
Kc = 8 M^-1
**Step 7: Interpret the Result**
The equilibrium constant for the given reaction is 8 M^-1. This means that at equilibrium, the concentration of Z is 8 times greater than the concentration of X and Y. The equilibrium lies to the right, indicating that the forward reaction is favored.
To calculate the equilibrium constant for the given reaction, we need to use the concentration of Z at equilibrium and the stoichiometric coefficients of the reactants and products.
**Given Data**
- 1 mole of X and Y are allowed to react.
- The reaction is: 2X + Y = Z
- The volume of the container is 2 litres.
- The concentration of Z at equilibrium is 0.2 M.
**Step-by-Step Solution**
**Step 1: Write the Balanced Chemical Equation**
2X + Y = Z
**Step 2: Write the Equilibrium Expression**
Kc = [Z] / ([X]^2 [Y])
**Step 3: Determine the Concentrations**
- The initial concentration of X and Y is 1 mole/2 L = 0.5 M.
- Let the equilibrium concentration of X and Y be x M.
- At equilibrium, the concentration of Z is 0.2 M.
**Step 4: Substitute the Values in the Equilibrium Expression**
Kc = [Z] / ([X]^2 [Y])
Kc = (0.2) / (x^2 * (0.5 - x))
**Step 5: Solve for x**
At equilibrium, the number of moles of Z formed is equal to the number of moles of X and Y consumed. Therefore,
2x = [Z] * 2 L
2x = 0.2 * 2
x = 0.1 M
**Step 6: Substitute the Value of x in the Equilibrium Constant Expression**
Kc = (0.2) / (0.1)^2 * (0.5 - 0.1)
Kc = 8 M^-1
**Step 7: Interpret the Result**
The equilibrium constant for the given reaction is 8 M^-1. This means that at equilibrium, the concentration of Z is 8 times greater than the concentration of X and Y. The equilibrium lies to the right, indicating that the forward reaction is favored.
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1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction?
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1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction?.
1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1 mole of x and Y are allowed to react in a 2 litre container when equilibrium is reached the following reaction occur 2x Y=Z. If the concentration of Z is .2M calculate the equilibrium constant for this reaction?.
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