Find K for 2A = B + 3C Reaction in a 1 L Container

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In a reaction involving 0.5 moles of A, 1 mole of B, and 2 moles of C in a 1 L container, the equilibrium shows 0.6 moles of A. This indicates that 0.1 moles of A have been formed during the reaction. To find the changes in moles of B and C, the stoichiometry of the reaction must be considered, where each mole of A corresponds to specific amounts of B and C. By applying this stoichiometric relationship, the concentrations of B and C can be calculated. Understanding these relationships is crucial for determining the equilibrium constant K for the reaction 2A = B + 3C.
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we mix 0.5 moles of A
1 mole of B
2 moles of C
in a one litter container

after it blances we find 0.6 moles of A
find K for
=(is a sign where two arrows go in different directions)
2A =B+3c
 
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1. How many moles of A have been formed?
2. How can you use this to find how many moles of B and C have been used?
 
1. 0.6 moles
2.
(0.5/1 +1/1+2/1)=output
 
1. No, you are mistaken. You started with 0.5 moles and ended up with 0.6 moles. 0.1 moles have been formed.

2. Look at the reaction. How many moles of B or C correspond to 1 mole of A? Then use this information and find the concentrations of B and C.
 
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