Identify the products formed in this Brønsted-Lowry reaction. HCO−3+HBrO↽−−⇀acid+base
1 answer:
Answer:
Explanation:
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In this case, according to the Brønsted-Lowry theory of acids, it is possible to realize that HBrO acts as the Brønsted-Lowry acid as it has a free hydrogen to give away to HCO₃⁻ which acts as the Brønsted-Lowry base able to accept the incoming hydrogen; therefore, the Brønsted-Lowry reaction is:
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Explanation:
Answer:
At equilibrium, the concentration of is going to be 0.30M
Explanation:
We first need the reaction.
With the information given we can assume that is:
+
⇄ 2
If there is placed 0.600 moles of NO in a 1.0-L vessel, we have a initial concentration of 0.60 M NO; and no nor
present. Immediately,
and
are going to be produced until equilibrium is reached.
By the ICE (initial, change, equilibrium) analysis:
I: []=0 ; [
]= 0 ; [
]=0.60M
C: []=+x ; [
]= +x ; [
]=-2x
E: []=0+x ; [
]= 0+x ; [
]=0.60-2x
Now we can use the constant information:
=
=
=
At equilibrium, the concentration of is going to be 0.30M