0.2 mole of A and 0.4 mile of B were reacted at a certain temperature and allowed to come to equilibrium . A+B---2AB The equilibrium mixture contained 0.1 mole of A, find Kc if volume of the container was 2 dm^3?
I'll show my explanation in steps for your understanding
- First set balance the equation
- Now write the equilibrium constant for the reaction
- Calculate the molarities
- Set up an ICE table
- Solve for the equilibrium amounts of B and AB
Reaction will proceed towards left
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Kc = [AB]² / [A][B] Kc = (0.1 mol / 2 dm³)² / [(0.2 mol - 0.1 mol) / 2 dm³][(0.4 mol - 0.1 mol) / 2 dm³]
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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