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3 years ago

Is air an element, compound or mixture? explain your answer

Chemistry

2 answers:

vfiekz [6]3 years ago

7 0

Mixture cuz it contains gases, water vapor, dust and microbes

emmainna [20.7K]3 years ago

3 0

It is a mixture because the compounds that make up air e.g. oxygen (o2), Carbon dioxide (co2) and the most important Nitrogen which is an element and makes up 78.09% of air are not chemically bound in the way that compounds are because they can be separated easily and there has been no change in state to any of the compounds or elements in air!hope this helpful!

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A 3.3 g sample of sodium hydrogen carbonate is added to a solution of acetic acid weighing 10.3 g. The two substances react, rel

Zanzabum

Answer:

1.73g of CO2.

Explanation:

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

NaHCO3 + CH3COOH → CH3COONa + H2O + CO2

Next we shall determine the masses of NaHCO3 and CH3COOH that reacted and the mass of CO2 produced from the balanced equation. This is illustrated below:

Molar mass of NaHCO3 = 23 + 1 + 12 + (16x3) = 84g/mol

Mass of NaHCO3 from the balanced equation = 1 x 84 = 84g

Molar mass of CH3COOH = 12 + (3x1) + 12 + 16 + 16 + 1 = 60g/mol

Mass of CH3COOH from the balanced equation = 1 x 60 = 60g

Molar mass of CO3 = 12 + (2x16) = 44g/mol

Mass of CO2 from the balanced equation = 1 x 44 = 44g

From the balanced equation above,

84g of NaHCO3 reacted with 60g of CH3COOH to produce 44g of CO2.

Next, we shall determine the limiting reactant of the reaction. This is illustrated below:

From the balanced equation above,

84g of NaHCO3 reacted with 60g of CH3COOH.

Therefore, 3.3g of NaHCO3 will react with = (3.3 x 60)/84 = 2.36g of CH3COOH.

From the above illustration, we can see that only 2.36g of CH3COOH out of 10.3g given reacted completely with 3.3g of NaHCO3. Therefore, NaHCO3 is the limiting reactant while CH3COOH is the excess reactant.

Finally, can determine the mass of CO2 produced during the reaction.

In this case the limiting reactant will be used because it will produce the mass yield of CO2 as all of it were used up in the reaction. The limiting reactant is NaHCO3 and the mass of CO2 produced is obtained as shown below:

From the balanced equation above,

84g of NaHCO3 reacted to produce 44g of CO2.

Therefore, 3.3g of NaHCO3 will react to produce = (3.3 x 44)/84 = 1.73g of CO2.

Therefore, 1.73g of CO2 is released during the reaction.

7 0

3 years ago

What’s a test you can give to show the difference between metal and gold

DENIUS [597]

Answer:

An Acid Test

An acid test is any qualitative chemical or metallurgical assay which uses acid ( most commonly), and historically, the use of a strong acid to distinguish gold from base metals.

Explanation:

I hope it helps

7 0

3 years ago

Suppose you begin with 1.50~g of the hydrate copper(II)sulfate · x-hydrate (CuSO4· x H2O), where x is an integer. After dehydrat

chubhunter [2.5K]

These are two questions and two answers.

Question 1.

Answer: x = 5

Explanation:

1) Data:

m₁ = 1.50 g

compound₁: CuSO₄· x H₂O

m₂ = 0.96g

compound₂ = CuSO₄

x = ? (round to the nearest integer)

2) Solution:

i) molar mass of CuSO₄ = 63.546g/mol + 32.065g/mol + 4×15.999g/mol = 159.607g/mol

ii) number of moles of CuSO₄

number of moles = mass in grams / molar mass = 1.50 g/ 159.607 g/mol = 0.006265 mol

iii) molar mass of H₂O = 18.015 g/mol

iv) mass of H₂O = 1.50g - 0.96g = 0.54g

v) number of moles of H₂O = mass in grams / molar mass = 0.54 g / 18.015 g/mol = 0.0300 mol

vi) Ratio moles H₂O / moles CuSO₄ = 0.0300 / 0.0062625 ≈ 5

∴ x = 5.

Question 2.

Answer: 5.5 g

1) Data:

compound₁ = KAl(SO₄)₂ · 12H₂O.

compound₂ = KAl(SO₄)₂

m₂ = 3.0 g KAl(SO₄)₂

m₁ = ? (two significant figures)

2) Solution:

i) molar mass of KAl(SO₄)₂ = 39.098g/mol + 26.982g/mol + 2×32.065g/mol + 8×15.999g/mol = 258.202

ii) number of moles of KAl(SO₄)₂ = mass in grams / molar mass = 3.0g / 258.202 = 0.011619 mol

iii) number of moles of H₂O = 12 × number of moles of KAl(SO₄)₂ = 12 × 0.011619*12 mol = 0.1394 moles

iv) mass of H₂O = number of moles × molar mass = 0.1394 moles × 18.015 g/mol = 2.5 g (rounded to two significant figures)

v) mass of the original compound = mass of KAl(SO₄)₂ + mass of H₂O = 5.5g

6 0

3 years ago

Ow well can you apply Charles’s law to this sample of gas that experiences changes in pressure and volume? Assume that pressure

Whitepunk [10]

I think it is A I believe

3 0

3 years ago

Read 2 more answers

How do I know what to do and can you help me because I really need it I am failing chemistry because it is too hard.

Arlecino [84]

Exothermic:

An Exothermic reaction is a chemical reaction that expels energy in the form of heat/light. Everything a Endothermic does not do. Pretty simple for this one

reactants → products + energy.

For future reference - Exo means release, thermic means heat.

Energy is a Reactant

_________________________________________________________

Endothermic:

An Endothermic reaction essentially is draining the heat energy from anything its its surroundings. Usually its just heat but can also be salt dissolving it water or ice melting. Another example would be frost on your windshield evaporating.

It is the exact opposite of an Exothermic reaction.

Energy is a Product

4 0

3 years ago