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3 years ago

1. For each of the following, convert the word equation into a formula equation, BUT do not balance! (4 pts each = 12 pts)

Chemistry

1 answer:

daser333 [38]3 years ago

4 0

Answer:

1a) BaClO₃(s) → BaCl₂(g) + O₂(g)

1b) Cl₂(g) + K₃N(s) → N₂(g) + KCl(s)

1c) Na₃N(aq) + Al(BrO₃)₃(aq) → AlN(s) + Na(BrO₃)₃(aq)

2a) Calcium hydroxide and hydrogen gas

2b) Tin(II) silicate and Lead(IV) permanganate

2c) Magnesium oxide and water

2d) No product

2e) Mercury and iodine

2f) Calcium chloride and iodine

2g) Strontium phosphite and cesium nitride

2h) Carbon dioxide, water, and sulfur dioxide

2i) Iron oxide(III) and carbon dioxide

2j) Magnesium acetate and hydrogen gas

2k) Calcium iodide

Explanation:

1. For each of the following, convert the word equation into a formula equation, BUT do not balance!

a) Barium chlorate → Barium chloride + Oxygen

1. Chemical formulas

Barium chlorate:

It is a salt: an ionic compound.
Barium has oxidation state +2
Chlorate is the ion ClO₃⁻
Swap the oxidation numbers to write the subscripts: 2 goes to ClO₃ and 1 goes to Ba
Chemical formula Ba(ClO₃)₂
It is solid: Ba(ClO₃)₂(s)

Barium chloride:

It is a salt: an ionic compount
Barium has oxidation state +2
Chlorine is in oxidation state -1
Swap the numbers to write the subscripts: 2 goes to Cl and 1 goes to Ba
BaCl₂
It is solid BaCl₂(s)

Oxygen:

It is a diatomic gas molecule
O₂(g)

2. Write the unbalanced molecular equation:

BaClO₃(s) → BaCl₂(s) + O₂(g)

b) Chlorine + Potassium nitride → Nitrogen + Potassium chloride

1. Chemical formulas

Chlorine:

It is a diatomic gas molecule
Cl₂(g)

Potassum nitride

It is a salt

Potassium has oxidation state +1
Nitrogen is with oxidation state +3
Swap the oxidation states
K₃N
It is solid: K₃N(s)

Nitrogen:

It is a diatomic gas
N₂(g)

Potassium chloride

It is a salt (ionic compound)
Potassium has oxidation state +1
Chlorine is in oxidation state -1
Swap the oxidation numbers
KCl
It is solid: KCl(s)

2. Write the unbalanced molecular equation

Cl₂(g) + K₃N(s) → N₂(g) + KCl(s)

c) Sodium nitride + Aluminum bromate → Aluminum nitride + Sodium bromate

1. Chemical formulas

Sodium nitride

It is a salt (ionic compound)
Sodium has oxidation state +1
Nitrogen is with oxidation state -3
Swap the oxidation numbers
Na₃N
It is in aqueous solution
Na₃N (aq)

Aluminum bromate

Salt
Aluminum has oxidation state +3
Bromate is the ion BrO₃⁻
Swap the oxidation states
Al(BrO₃)₃ (aq)

Aluminum nitride

Both Al and N have oxidation state 3, which simply
AlN(s). It is not soluble in water.

Sodium bromate

Na(BrO₃)₃ (aq)

2. Write the unbalanced molecular equation

Na₃N(aq) + Al(BrO₃)₃(aq) → AlN(s) + Na(BrO₃)₃(aq)

<h2>This is a long answer with more than 5,000 charaters; thus, I have to add the rest of the explanations on a separate file.</h2><h2></h2><h2>The attached file contains the complete answer.</h2>

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What is the percentage yield of O2 if 12.3 g of KClO3 (molar mass 123 g) is decomposed to produce 3.2 g of O2 (molar mass 32 g)

My name is Ann [436]

Answer:

The percentage yield of O2 is 66.7%

Explanation:

Reaction for decomposition of potassium chlorate is:

2KClO₃ → 2KCl + 3O₂

The products are potassium chloride and oxygen.

Let's find out the moles of chlorate.

Mass / Molar mass = Moles

12.3 g / 123 g/mol = 0.1 mol

So ratio is 2:3, 2 moles of chlorate produce 3 mol of oxygen.

Then, 0.1 mol of chlorate may produce (0.1 .3)/ 2 = 0.15 moles

Let's convert the moles of produced oxygen, as to find out the theoretical yield.

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To calculate the percentage yield, the formula is

(Produced Yield / Theoretical yield) . 100 =

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A metallurgist has one alloy containing 21% aluminum and another containing 42% aluminum. how many pounds of each alloy must he

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Answer is: 7.8 lb of 21% aluminum and 33.2 ib of 42% aluminum.

ω₁ = 21% ÷ 100% = 0.21.
ω₂ = 42% ÷ 100% = 0.42.
ω₃ = 38% ÷ 100% = 0.38.
m₁ = ?.

m₂ = ?.
m₃ = m₁ + m₂.
m₃ = 41 pounds.

m₁ = 41 lb - m₂.
ω₁ · m₁ + ω₂ ·m₂ = ω₃ · m₃.

0.21 · (41 lb - m₂) + 0.42 · m₂ = 0.38 · 41 lb.

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3 years ago