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Sergio [31]
3 years ago
13

Consider the above reaction. If some CO2 were removed from the container, what would the reaction do in an attempt to replace th

e CO2?
Chemistry
1 answer:
faltersainse [42]3 years ago
4 0

Answer:

See explanation

Explanation:

The reaction to be considered is shown below;

H2CO3<------->CO2 + H2O

We know  that when a constraint such as a sudden change in concentration, pressure or temperature is imposed on  a reaction system in equilibrium, the system has to adjust itself by shifting in a particular direction in order to cancel the constraint.

Now, if we remove CO2, the equilibrium position must shift to the right by the decomposition of more H2CO3 to establish equilibrium again.

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Calculate the reaction quotient Qp for the following redox reaction: 14H+ + Cr2O72- + 6Cl- ----&gt; 2Cr3+ + 3Cl2 + 7H2O The reac
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Answer:

Value of Q_{p} for the given redox reaction is 1.0\times 10^{-8}

Explanation:

Redox reaction with states of species:

14H^{+}(aq.)+Cr_{2}O_{7}^{2-}(aq.)+6Cl^{-}(aq.)\rightarrow 2Cr^{3+}(aq.)+3Cl_{2}(g)+7H_{2}O(l)

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Q_{p}=\frac{[Cr^{3+}]^{2}.P_{Cl_{2}}^{3}}{[H^{+}]^{14}.[Cr_{2}O_{7}^{2-}].[Cl^{-}]^{6}}

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pH=-log[H^{+}]

So, [H^{+}]=10^{-pH}

Plug in all the given values in the equation of Q_{p}:

Q_{p}=\frac{(0.10)^{2}\times (0.010)^{3}}{(10^{-0.0})^{14}\times (1.0)\times (1.0)^{6}}=1.0\times 10^{-8}

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