I need help. ASAP! Look at the picture below. (5)

A solution may contain Ag+, Pb2+, and/or Hg22+. A white precipitate forms when 6 M HCl is added. The precipitate is partially so

omeli [17]

Answer:

All three are present

Explanation:

Addition of 6 M HCl would form precipitates of all the three cations, since the chlorides of these cations are insoluble: $AgCl (s), PbCl_2 (s), Hg_2Cl_2 (s)$ .

Firstly, the solid produced is partially soluble in hot water. Remember that out of all the three solids, lead(II) choride is the most soluble. It would easily completely dissolve in hot water. This is how we separate it from the remaining precipitate. Therefore, we know that we have lead(II) cations present, as the two remaining chlorides are insoluble even at high temperatures.
Secondly, addition of liquid ammonia would form a precipitate with silver: $AgCl (s) + 2 NH_3 (aq) + H_2O (l)\rightarrow [Ag(NH_3)_2]OH (s) + HCl (aq)$ ; Silver hydroxide at higher temperatures decomposes into black silver oxide: $2 [Ag(NH_3)_2]OH (s)\rightarrow Ag_2O (s) + H_2O (l) + 4 NH_3 (g)$ .
Thirdly, we also know we have $Hg_2^{2+}$ in the mixture, since addition of potassium chromate produces a yellow precipitate: $Hg_2^{2+} (aq) + CrO_4^{2-} (aq)\rightarrow Hg_2CrO_4 (s)$ . The latter precipitate is yellow.

3 0

4 years ago

At a particular temperature, an equilibrium mixture the reaction below was found to contain 0.171 atm of I2, 0.166 atm of Cl2 an

maw [93]

Answer: 3390

Explanation:

Since this problem already gives is the equilibrium values, all we have to do is to plug them into the formula for $K_{p}$ .

$K_{p} =\frac{[ICl]^2}{[I_{2}][Cl_{2}] }$

$K_{p} =\frac{(9.81)^2}{(0.171)(0.166)} =3390$

7 0

3 years ago

Help pleaseeeeeeee //////:))))))))))))

Mademuasel [1]

Chose 3 you know this because you will need heat..

7 0

3 years ago

What was helium used for in the past?

yawa3891 [41]

Helium used to be used in hot air balloons. Then, when the Hindenburg exploded, annexed file, they realized that hydrogen was not only lighter, but it also was less flammable.

6 0

3 years ago

Read 2 more answers

The water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g) is used industrially to produce hydrogen. The reaction enthalpy is ΔH∘=−4

Pani-rosa [81]

Answer:

The answers are in the explanation

Explanation:

A. For the reaction:

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g); ΔH°=−41kJ.

As the reaction is exothermic ( ΔH°<0), you need to use low temperature to increase the equilibrium yield of hydrogen -LeChatelier's principle-.

We would use low temperature. For an exothermic reaction such as this, decreasing temperature increases the value of K and the amount of products at equilibrium.

B.

c. No. We cannot increase the equilibrium yield of hydrogen by controlling the pressure of this reaction.

It is possible to increase the equilibrium yield of reaction by controlling the amount of reactants added. As reactants and products are gases, the pressure of the reaction will not change the amount of reactants or products in the equilibrium.

I hope it helps!

8 0

3 years ago