A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 1.79 g/mL, 1.8
1 answer:
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Answer : The concentration of at equilibrium is 0.9332 M
Solution : Given,
Concentration of and
at equilibrium = 0.200 M
Concentration of and
at equilibrium = 0.500 M
First we have to calculate the value of equilibrium constant.
The given equilibrium reaction is,
The expression of will be,
Now we have to calculate the final concentration of NO.
The given equilibrium reaction is,
Initially 0.200 0.200 0
.800
At equilibrium (0.200-x) (0.200-x) (0.800+2x)
The expression of will be,
By solving the term x, we get
From the values of 'x' we conclude that, x = 2.6 can not more than initial concentration. So, the value of 'x' which is equal to 2.6 is not consider.
And the negative value of 'x' shows that the equilibrium shifts towards the left side (reactants side).
Thus, the concentration of at equilibrium = (0.800+2x) = 0.800 + 2(0.0666) = 0.9332 M
Therefore, the concentration of at equilibrium is 0.9332 M
Answer:
Use the x method, cross over each charge.
Explanation:
and
the +1 and -1 cancel each other out, so it will be KBr