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mestny [16]
3 years ago
13

Which of the following is not a result when a change to an equilibrium system is applied? (2 points)

Chemistry
2 answers:
Ray Of Light [21]3 years ago
8 0
It should be increasing the rate of the forward reaction will cause a shift to the left because the external stress, which is the increase in rate, will cause the reaction to be unbalanced, and to reach equilibrium it needs to shift to the right.
Ksju [112]3 years ago
6 0

Answer: Option (2) is the correct answer.

Explanation:

According to LeChatelier principle, any change in the equilibrium of a chemical reaction will result in shifting of equilibrium which is opposing the change.

Therefore, when we increase the rate of the reverse reaction that is, we move towards left side then this will actually cause a shift to the right hand side which is opposing the change.

Thus, we can conclude that increasing the rate of the reverse reaction will cause a shift to the left is not a result when a change to an equilibrium system is applied.

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Type the correct answer in the box. Express your answer to three significant figures.
VladimirAG [237]

<u>Given:</u>

Mass of calcium nitrate (Ca(NO3)2) = 96.1 g

<u>To determine:</u>

Theoretical yield of calcium phosphate, Ca3(PO4)2

<u>Explanation:</u>

Balanced Chemical reaction-

3Ca(NO3)2 + 2Na3PO4 → 6NaNO3 + Ca3(PO4)2

Based on the reaction stoichiometry:

3 moles of Ca(NO3)2 produces 1 mole of Ca3(PO4)2

Now,

Given mass of Ca(NO3)2 =  96.1 g

Molar mass of Ca(NO3)2 =  164 g/mol

# moles of ca(NO3)2 = 96.1/164 = 0.5859 moles

Therefore, # moles of Ca3(PO4)2 produced = 0.0589 * 1/3 = 0.0196 moles

Molar mass of Ca3(PO4)2 = 310 g/mol

Mass of Ca3(PO4)2 produced = 0.0196 * 310 = 6.076 g

Ans: Theoretical yield of Ca3(PO4)2 = 6.08 g



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