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3 years ago

Classify each of the following possible reactions according to whether a precipitate will form or will not form.

Chemistry

1 answer:

elena-14-01-66 [18.8K]3 years ago

8 0

Answer:

Reactions, 2, 3 and 5 make precipitates

Explanation:

1. The halogens always make aqueous salts with elements from group 1

2. Phosphate anion can make insoluble salts, the same as carbonate.

3. Nitrate anion always make aqueous salts

4. Sulfate anion makes aqueous salts except with Ag⁺, Pb⁺² and group 2

1. KI(aq) + NaCl(aq) → KCl(aq) + NaI(aq)

2. 2Na₃PO₄ (aq) + 3CoCl₂(aq) → 6NaCl(aq) + Co₃(PO₄)₂(s) ↓

3. Na₂CO₃ (aq) + CuCl₂ (aq) → 2NaCl (aq) + CuCO₃ (s) ↓

4. 2LiNO₃ (aq) + Na₂SO₄ (aq) → Li₂SO₄ (aq) + 2NaNO₃(aq)

5. CrCl₂ (aq) + Li₂CO₃ (aq) → 2LiCl (aq) + Cr₂(CO₃)₂ (s) ↓

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Answer:

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Galvanized nails are iron nails that have been plated with zinc to prevent rusting. The relevant reaction is

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Answer:

1.18 × 10⁷ c

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Explanation:

Let's consider the reduction of Zn²⁺.

Zn²⁺(aq) + 2 e⁻ ⇒ Zn(s)

How many coulombs of charge are needed to produce 61.2 mol of solid zinc?

We can establish the following relations:

When 2 moles of electrons circulate, 1 mol of Zn is produced.
1 mole of electrons have a charge of 96468 c (Faraday's constant).

Then, for 61.2 mol of Zn:

$61.2molZn.\frac{2mole^{-} }{1molZn} .\frac{96468c}{1mole^{-}} =1.18 \times 10^{7} c$

Identify the anode and cathode when plating an iron nail with zinc.

The anode is where the oxidation takes place and the cathode is where the reduction takes place.

Anode (oxidation): Fe(s) ⇒ Fe²⁺(aq) + 2 e⁻

Cathode (reduction): Zn²⁺(aq) + 2 e⁻ ⇒ Zn(s)

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3 years ago

Give the word and chemical equations (including state symbols) for the reaction of potassium and water

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Answer:

Zinc is Zn and Magnesium is Mg

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3 years ago

Predict which of the following changes will cause the volume of the balloon to increase or decrease assuming that the temperatur

IrinaVladis [17]

Answer:

1. a

2. a

3. b

4. c

Explanation:

The STP is the Standard conditions of Temperature and Pressure, in these conditions, T = 0°C and P = 1 atm. By the ideal gas law,

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

We can observe that pressure and volume are indirect proportional, so when one increase, the other decrease. so:

1. The pressure decreases from 1.15 atm to STP, 1 atm, thus the volume increases.

2. The pressure decreases from STP, 1 atm, to 0.5 atm, thus the volume increases.

3. The pressure increases from STP, 1 atm, to 1.25 atm, thus the volume decreases.

4. The pressure remains constant at 1 atm, thus the volume is unchanged.

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