Answer:
I think the answer is forest
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Answer:
The correct answer is B.
Explanation:
Heterogeneous equilibrium is that in which reagents and products are present in more than one phase.
When the reaction is carried out in a closed container, three equilibrium phases are present: solid magnesium oxide, solid magnesium sulfate and gaseous sulfur trioxide.
Hence, the equilibrium contant is given by:
![K=\frac{[MgSO_4]}{[MgO][SO_3]} =\frac{1}{[SO_3]}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BMgSO_4%5D%7D%7B%5BMgO%5D%5BSO_3%5D%7D%20%3D%5Cfrac%7B1%7D%7B%5BSO_3%5D%7D)
The concentrations in the equilibrium equation are the relationships of the real concentrations between the concentrations in the standard state. Since the standard state of a pure solid is the pure solid itself, the ratio of concentrations for a pure solid is equal to one.
Now, we analyse each statement:
I) As the reaction is endothermic (ΔH>0), increasing the temperature shifts the balance to the right because excess heat will be used to form more products.
II) Increasing the volume will decrease the concentration of SO₃, so Q>K and then this shifts the balance to the left.
III) As it is a heterogeneous balance, adding MgO will not affect the balance.
IV) Removing SO3 will decrease its concentration and therefore the reaction equilibrium will shift to the left.
Four option are provided as,
CH3CH2OCH2CH3
CH3CH2Cl
CH3CH2CH3
CH3OCH2CH2OCH3
CH3CH2Cl having 2 peaks of H NMR as 1st peak for quartet of 2 H and 2nd peak of triplet of 3 H and thus the ratio of both the peak is 2 :3 as the ratio indicates the number of hydrogen corresponds to each peak.