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2 years ago

Consider the following reaction: 2 Bi(s) + 3 Cl2(g) → 2 BiCl3(s)

1 answer:

5 0

Taking into account the reaction stoichiometry, 1.119 grams of chlorine gas are required to produce 3.32 grams of bismuth chloride is produced.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 Bi + 3 Cl₂ → 2 BiCl₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Bi: 2 moles
Cl₂: 3 moles
BiCl₃: 2 moles

The molar mass of the compounds is:

Bi: 209 g/mole
Cl₂: 70.90 g/mole
BiCl₃: 315.45 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

Bi: 2 moles ×209 g/mole=418 g

Cl₂: 3 moles ×70.90 g/mole= 212.7 g

BiCl₃: 2 moles ×315.45 g/mole= 630.9 g

<h3>Mass of Cl₂ required</h3>

The following rule of three can be applied: If by reaction stoichiometry 630.9 grams of BiCl₃ are formed by 212.7 grams of Cl₂, 3.32 grams of BiCl₃ are formed by how much mass of Cl₂?

$mass of Cl_{2} =\frac{3.32 grams of BiCl_{3}x212.7 grams of Cl_{2} }{630.9 grams of BiCl_{3}}$

<u><em>mass of Cl₂= 1.119 grams</em></u>

Finally, 1.119 grams of chlorine gas are required to produce 3.32 grams of bismuth chloride is produced.

Learn more about the reaction stoichiometry:

<u>brainly.com/question/24741074</u>

<u>brainly.com/question/24653699</u>

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Find the amount of heat energy needed to convert 400 grams of ice at -38°C to steam at 160°C.

Marianna [84]

The amount of heat energy needed to convert 400 g of ice at -38 °C to steam at 160 °C is 1.28×10⁶ J (Option D)

<h3>How to determine the heat required change the temperature from –38 °C to 0 °C </h3>

Mass (M) = 400 g = 400 / 1000 = 0.4 Kg
Initial temperature (T₁) = –25 °C
Final temperature (T₂) = 0 °
Change in temperature (ΔT) = 0 – (–38) = 38 °C
Specific heat capacity (C) = 2050 J/(kg·°C)
Heat (Q₁) =?

Q = MCΔT

Q₁ = 0.4 × 2050 × 38

Q₁ = 31160 J

<h3>How to determine the heat required to melt the ice at 0 °C</h3>

Mass (m) = 0.4 Kg
Latent heat of fusion (L) = 334 KJ/Kg = 334 × 1000 = 334000 J/Kg
Heat (Q₂) =?

Q = mL

Q₂ = 0.4 × 334000

Q₂ = 133600 J

<h3>How to determine the heat required to change the temperature from 0 °C to 100 °C </h3>

Mass (M) = 0.4 Kg
Initial temperature (T₁) = 0 °C
Final temperature (T₂) = 100 °C
Change in temperature (ΔT) = 100 – 0 = 100 °C
Specific heat capacity (C) = 4180 J/(kg·°C)
Heat (Q₃) =?

Q = MCΔT

Q₃ = 0.4 × 4180 × 100

Q₃ = 167200 J

<h3>How to determine the heat required to vaporize the water at 100 °C</h3>

Mass (m) = 0.4 Kg
Latent heat of vaporisation (Hv) = 2260 KJ/Kg = 2260 × 1000 = 2260000 J/Kg
Heat (Q₄) =?

Q = mHv

Q₄ = 0.4 × 2260000

Q₄ = 904000 J

<h3>How to determine the heat required to change the temperature from 100 °C to 160 °C </h3>

Mass (M) = 0.4 Kg
Initial temperature (T₁) = 100 °C
Final temperature (T₂) = 160 °C
Change in temperature (ΔT) = 160 – 100 = 60 °C
Specific heat capacity (C) = 1996 J/(kg·°C)
Heat (Q₅) =?

Q = MCΔT

Q₅ = 0.4 × 1996 × 60

Q₅ = 47904 J

<h3>How to determine the heat required to change the temperature from –38 °C to 160 °C</h3>

Heat for –38 °C to 0°C (Q₁) = 31160 J
Heat for melting (Q₂) = 133600 J
Heat for 0 °C to 100 °C (Q₃) = 167200 J
Heat for vaporization (Q₄) = 904000 J
Heat for 100 °C to 160 °C (Q₅) = 47904 J
Heat for –38 °C to 160 °C (Qₜ) =?

Qₜ = Q₁ + Q₂ + Q₃ + Q₄ + Q₅

Qₜ = 31160 + 133600 + 167200 + 904000 + 47904

Qₜ = 1.28×10⁶ J

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2 years ago

How are the following aspects of a reaction affected by the addition of a catalyst? 1) activation energy of the reverse reaction

snow_tiger [21]

These are four questions and four answers.

Answers:

1) activation energy of the reverse reaction

b. Decreased

2) Rate of the forward reaction

a. Increased

3) Rate of the reverse reaction

a. Increased

4) Activation energy of the forward reaction

b. decreased

Explanation:

<em>Activarion energy</em> is the energy required by the reactants to form the intermediate transition state and become products.

<em>Catalysts</em> are substances that change the path of the chemical reactions, lowering the activation energy, and thus speeding up the rate of the reactions, since the products can reach the new lower activation energy faster.

The equilibrium reactions are the chemical process in which two reactions, the <em>forward and the reverese reactions</em>, occur simultaneously and at the same rate. The equlibrium reactions may be represented by:

A ⇄ B

Where A → B is the direct or forward reaction, and A ← B is the reverse reaction (note the inversed arrow, from right to left).

For the direct reaction A represents the reactants and B represents the products. On the other hand, B represents the reactants and A represents the reactants of the reverse reaction and A. This, is A is the reactant of the forward reaction and the product of the reverse reaction, while B is the reactant of the reverse reaction and the product of the forward reaction.

Since, <em>the addition of a catalyst</em> lowers the activation energy of the process, the new activation energy is lower for both the forward and the reverse reaction, meaning that:

1. <em>The activation energy of the reverse reaction is decreased</em> (option b. of the first question)

2.<em> The rate of the forward reaction is increased</em> (option a. of the second question)

3. <em>The rate of the reverse reaction is increased</em> (option a. of the third question).

4. <em>Activation energy of the forward reaction is decreased</em> (option b. of the fourth question).

In summary, the addition of a catalyst decreases the activation energy for both forward and reverse reactions, and increases the rate of both forward and reverse reactions.

3 0

3 years ago

Read 2 more answers

After heating the solution, you decant the liquid and wash the remaining solid with distilled water. What you are removing by th

solniwko [45]

Answer:

The solvent

Explanation:

After the solid is recoverd by decanting the liquid, some solvent particles may still adhere to the solid.

In order to remove the solvent that may have adhered to the solid completely , the solid is washed before it is now dried.

7 0

3 years ago

Given the reaction below, if 0.00345 g of carbon dioxide is used up, how many grams of water will be produced?

zimovet [89]

From the stoichiometry of the reaction, 1.4 * 10^-3 g is produced.

<h3>What mass of water is produced?</h3>

The equation of the reaction is written as; CO2 + 2LiOH → Li2CO3 + H2O. This can help us to apply the principle of stoichiometry here.

Thus;

Number of moles of CO2 = 0.00345 g/44 g/mol = 7.8 * 10^-5 moles

If 1 mole of CO2 produced 1 mole of water

7.8 * 10^-5 moles of CO2 produced 7.8 * 10^-5 moles of water

Mass of water produced = 7.8 * 10^-5 moles * 18 g/mol = 1.4 * 10^-3 g

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2 years ago

The PH solution of NH3 of 0.950molar solution is 11.612. find the Kb

Vaselesa [24]

Answer:

1.8 x 10⁻⁵

Explanation:

NH3(aq) + H2O(l) ⇄ NH4⁺(aq) + OH⁻(aq)

I 0.95 0 0

C -x +x +x

E 0.95-x x x

Kb= [NH₄⁺] [OH⁻] / ( NH₃) = x²/ (0.95-x )

P(OH) = 14-PH = 14-11.612 = 2.388

(OH)⁻¹ = 10⁻²°³⁸⁸ = 4.09 x 10⁻³ = x

Kb = (4.09 x 10⁻³)²/ (0.95-4.09 x 10⁻³)

= 1.8 x 10⁻⁵

8 0

3 years ago