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3 years ago

Is burning physical or chemical change?

Chemistry

2 answers:

Tanya [424]3 years ago

7 0

Answer:

a chemical change

Explanation:

lighting a match is a chemical change. chemical reactions cause chemical change. in a chemical reaction two or more substances, called the reactants, form different substances called products. hope this helped :)

LUCKY_DIMON [66]3 years ago

3 0

Answer:

Burning is a chemical process.

Explanation:

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What volume (in L) of carbon dioxide will be produced from the reaction of 37.4 L of oxygen?

Anna [14]

Answer:

21.4 L

Explanation:

Given data:

Volume of carbon dioxide produced = ?

Volume of oxygen = 37.4 L

Solution:

Chemical equation:

2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

It is known that,

1 mole = 22.414 L

There are 7 moles of oxygen = 7×22.414 = 156.9 L

There are 4 moles of carbon dioxide = 4×22.414 = 89.66 L

Now we will compare:

O₂ : CO₂

156.9 : 89.66

37.4 : 89.66/156.9×37.4 = 21.4 L

So from 37.4 L of oxygen 21.4 L of carbon dioxide is produced.

3 0

3 years ago

An organic one of these will usually contain carbon and hydrogen.

Oksanka [162]

The answer will be A

7 0

3 years ago

Read 2 more answers

Help!!!

kupik [55]

Answer:

1. 0.82 gram of Ag+

2. 4.79 g of Ag₂O₃S

Explanation:

From the given information:

Total amount of Ag₂O₃S = 2.24 grams

Atomic mass of Ag+ =107.86 g/mole

molar mass of Ag₂O₃S = 295.8 g/mole

∴

The mass of the Silver (Ag) in grams is:

$= Total\ amount \ of \ Ag^+ \times \dfrac{107.86 \ g/mol}{295.8 \ g/mol}$

$=2.24 \times \dfrac{107.86 \ g/mol}{295.8 \ g/mol}$

= 0.82 gram of Ag+

Here, the total amount of Ag₂O₃S = unknown

Atomic mass of Ag+ = 107.86 g/mole

molar mass of Ag₂O₃S = 295.8 g/mole

amount of Ag+ = 1.75 g

∴

The mass of Ag₂O₃S = $Total \ amount \ of \ Ag^+ \times \dfrac{295.8 \ g/mol}{107.86\ g/mol}$

$=1.75 \times \dfrac{295.8 \ g/mol}{107.86\ g/mol}$

= 4.79 g of Ag₂O₃S

4 0

3 years ago

The following data was collected when a reaction was performed experimentally in the laboratory.

Lera25 [3.4K]

Answer:

Mass = 279.23 g

Explanation:

Given data:

Number of moles of Fe₂O₃ = 3 mol

Number of moles of Al = 5 mol

Maximum amount of iron produced by reaction = ?

Solution:

Chemical equation:

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe

Now we will compare the moles of iron with Al and iron oxide.

Fe₂O₃ : Fe

1 : 2

3 : 2×3 = 6 mol

Al : Fe

2 : 2

5 : 5 mol

The number of moles of iron produced by Al are less so Al is limiting reacting and it will limit the amount of iron so maximum number of iron produced are 5 moles.

Mass of iron:

Mass = number of moles × molar mass

Mass = 5 mol × 55.845 g/mol

Mass = 279.23 g

3 0

3 years ago

Which of the following equilibrium expressions corresponds to a heterogeneous equilibrium?(a) Kc =[NH4+][OH−][NH3](b) Kc =[H+][C

Alex777 [14]

Answer:

c. $Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}$

d. $Kc = [Ba^{2+}][F^{-}]^2$

Explanation:

An heterogeneous equilibrium is defined as a system whose reactants, products, or both are in more than one phase.

Also, you must know in an equilibrium constant you don't take solids or pure liquids. Thus:

a. $Kc = \frac{[NH_{4}^+][OH^-]}{[NH_3]}}$

The reaction must be: NH₃(aq) + H₂O(l) ⇆ NH₄⁺(aq) + OH⁻(aq) All reactants are in the same phase.

b. $Kc = \frac{[H^+][C_2H_3O_{2}^-]}{[HC_2H_3O_2]}}$

The reaction must be: HC₂H₃O₂(aq) ⇄ H⁺(aq) + C₂H₃O₂⁻(aq) All reactants are in the same phase.

c. $Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}$

The reaction must be: 2NH₃(aq) + AgCl(s) ⇄ Ag(NH₃)₂⁺(aq) + Cl⁻(aq)

Reactants aren´t in the same phase. Heterogeneous equilibrium

d. $Kc = [Ba^{2+}][F^{-}]^2$

The reaction must be: BaF₂(s) ⇆ Ba²⁺(aq) + 2F⁻(aq)

Reactants aren´t in the same phase. Heterogeneous equilibrium

I hope it helps!

6 0

4 years ago

Is burning physical or chemical change?￼

Is burning physical or chemical change?