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Nastasia [14]
2 years ago
10

Aqueous hydrogen chloride reacts with oxygen gas to form chlorine gas and liquid water.Express your answer as a balanced chemica

l equation. Identify all of the phases in your answer
Chemistry
2 answers:
zhenek [66]2 years ago
8 0

4HCl (aq) + O₂ (g) ⇒ 2Cl₂ (g) + 2H₂O (l)

<h3>Further explanation </h3>

Equalization of chemical reactions can be done using variables. Steps in equalizing the reaction equation:

  • 1. gives a coefficient on substances involved in the equation of reaction such as a, b, or c, etc.
  • 2. make an equation based on the similarity of the number of atoms where the number of atoms = coefficient × index (subscript) between reactant and product
  • 3. Select the coefficient of the substance with the most complex chemical formula equal to 1

For gas combustion reaction which is a reaction of hydrocarbons with oxygen produces CO₂ and H₂O (water vapor). can use steps:

Balancing C, H and the last O

Reaction :

HCl (aq) + O₂ (g) ⇒ Cl₂ (g) + H₂O (l)

Suppose we give a coefficient of 1 for HCl

HCl (aq) + aO₂ (g) ⇒ bCl₂ (g) + cH₂O (l)

number of Homs: left 1, right 2c -> 2c = 1-> c = 1/2

number of Cloms: left 1, right 2b ---> 2b = 1 ----> b = 1/2

number of O atoms: left 2a, right c ---> 2a = c ---> 2a = 1/2 ---> a = 1/4

the reaction coefficient becomes:

\rm HCl(aq)+\dfrac{1}{4}O_2(g)\Rightarrow \dfrac{1}{2}Cl_2(g)+\dfrac{1}{2}H_2O(l)\times 4\\\\4HCl(aq)+O_2(g)\Rightarrow 2Cl_2(g)+2H_2O(l)

<h3>Learn more </h3>

the combustion of octane in gasoline

brainly.com/question/8175791

brainly.com/question/897044

hydrogen and excess oxygen

brainly.com/question/1405182

ddd [48]2 years ago
5 0

Answer: 4 HCl (g) + O₂ (g) → 2 Cl₂ (g) + 2 H₂O (l)

Explanation:

4 moles of hydrogen chloride (note that it is in the gaseous phase, otherwise it would be hydrochloric acid) react with 1 mole of oxygen gas to form 2 moles of chlorine gas and 2 moles of liquid water.

To conform with  the law of conservation of mass, the equation must be balanced, this means that there must be the same number of each type of atom  on both sides of the arrow.

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kobusy [5.1K]
B, 51 mL of mystery solution
4 0
3 years ago
Just need help with these two questions
kvasek [131]
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8 0
2 years ago
What volume is occupied by 8.7 g of chlorine gas, Cl2, at 23°C and 1.15 atm pressure
Harrizon [31]

Answer:

V = 5.17L

Explanation:

Mass of gas = 8.7g

T = 23°C = (23 + 273.15)K = 296.15K

P = 1.15 atm

V = ?

R = 0.082atm.L / mol.K

From ideal gas equation

PV = nRT

P = pressure of the gas

V = volume of the gas

n = no. Of moles

R = ideal gas constant

T = temperature of the gas

no of moles = mass / molar mass

Molar mass of Chlorine = 35.5g / mol

No. Of moles = 8.7 / 35.5

No. Of moles = 0.245 moles

PV = nRT

V = nRT / P

V = (0.245 * 0.082 * 296.15) / 1.15

V = 5.9496 / 1.15

V = 5.17L

The volume of the gas is 5.17L

4 0
3 years ago
The bacteria can chemically combine nitrogen with hydrogen to form ammonia (NH3). This combining process is called nitrogen fixa
nikklg [1K]

Answer:

bacteria

Explanation:

they are decomposers. they decompose dead material by fixing nitrogen

7 0
3 years ago
How many grams of ammonia (NH3) can be produced by the synthesis of excess hydrogen gas (H2) and 253.8 grams of nitrogen gas (N2
kogti [31]

Answer:

308.2 g of NH₃.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

3H₂ + N₂ —> 2NH₃

Next, we shall determine the mass of N₂ that reacted and the mass of NH₃ produced from the balanced equation. This can be obtained as follow:

Molar mass of N₂ = 2 × 14 = 28 g/mol

Mass of N₂ from the balanced equation = 1 × 28 = 28 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3 = 17 g/mol

Mass of NH₃ from the balanced equation = 2 × 17 = 34 g

Summary:

From the balanced equation above,

28 g of N₂ reacted to produce 34 g of NH₃.

Finally, we shall determine the mass of NH₃ produced by the reaction of 253.8 g of N₂. This can be obtained as illustrated below:

From the balanced equation above,

28 g of N₂ reacted to produce 34 g of NH₃.

Therefore, 253.8 g of N₂ will react to produce = (253.8 × 34)/28 = 308.2 g of NH₃.

Thus, 308.2 g of NH₃ were obtained from the reaction.

8 0
2 years ago
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