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Alex_Xolod [135]
3 years ago
9

The equilibrium expression for a reaction is `"K"_("eq") = ("[H"^+"]"^6)/("[Bi"^(2+)"]"^2["H"_2"S"]^3)` Which of the following c

ould be the reaction?
A.
6H+(aq) + BiS(s) 2Bi2+(aq) + 3H2S(g)

B.
2Bi2+(aq) + 3H2S(aq) Bi2S3(s) + 6H+(aq)

C.
6H+(aq) + Bi2S3(s) 2Bi2+(aq) + 3H2S(g)

D.
2Bi2+(aq) + 3H2S(aq) Bi2S3(aq) + 6H+(aq)
Chemistry
2 answers:
Nata [24]3 years ago
4 0

Option B is correct

K = Kp /Kr

The given equation indicating, the product containing 6 moles of proton whereas the reactant contains 2 mole of bismuth and 3 mole of hydrogen sulphide.

Hence, in reaction B there are 2 mole of bismuth and 3 mole of hydrogen sulphide reacting to produce 6 moles of proton. whereas the concentration of Bi2S3 is not considered as it is present in solid phase.

natima [27]3 years ago
3 0

Answer:

2Bi2+(aq) + 3H2S(aq)↔ Bi2S3(s) + 6H+(aq)

Explanation:

In general for a hypothetical reaction:

x(Reactants) ↔ y(Products)

the equilibrium constant, Keq is given by the ratio of the products to that of the reactants raised to the appropriate coefficients.

Keq = \frac{[Products]^{y} }{[Reactants]^{x} }

The given Keq is:

Keq = \frac{[H+]^{6}}{[Bi2+]^{2} [H2S]^{3} }

This implies that the reactants are: H2S (aq) and Bi2+(aq)

Products are: H+(aq)

Therefore the reaction with the appropriate coefficients would be:

2Bi2+(aq) + 3H2S(aq)↔ Bi2S3(s) + 6H+(aq)

Since the activity of solids = 1, Bi2S3 is not included in Keq

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5 0
1 year ago
To find the atomic mass of a particular atom you need to know
Andreyy89
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It is know as the normal force.


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Which of the following elements has 3 electrons in the outermost d orbital?
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Answer:

A

Explanation:

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Valency of B is −2 as it will gain 2 electrons to attain stability and combine with other atom.

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(Refer to Image)

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3 0
3 years ago
Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 3.56 mol of m
pishuonlain [190]
<h3>Answer:</h3>

43.27 g Mg

<h3>Explanation:</h3>

The balanced equation for the reaction between magnesium metal and hydrochloric acid is;

Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

From the equation;

1 mole of magnesium reacts with 2 moles of HCl

We are given;

3.56 moles of Mg and 3.56 moles of HCl

Using the mole ratio;

3.56 moles of Mg would react with 7.12 moles of HCl, and

3.56 moles of HCl would react with 1.78 moles of Mg

Therefore;

The amount of magnesium was in excess;

Moles of Mg left = 3.56 moles - 1.78 moles

                         = 1.78 moles

But; 1 mole of Mg = 24.305 g/mol

Therefore;

Mass of magnesium left = 1.78 moles × 24.305 g/mol

                                        = 43.2629 g

                                        = 43.27 g

Thus, the mass of magnesium that remained after the reaction is 43.27 g

4 0
3 years ago
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