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1 year ago

Calculate the density of oxygen, O2 , under each of the following conditions:

Chemistry

1 answer:

sdas [7]1 year ago

4 0

The density of oxygen, O2 , under each of the following conditions:

STP 1.00 atm and 20.0°C is 1.78 g/L.

<h3>What is the density of a substance?</h3>

Density is the ratio of mass and volume of a substance.

The density of oxygen under the given conditions is calculated as follows:

STP = standard temperature and pressure.

standard pressure = 1 atm pressure

standard temperature = 25°C

Volume of 1 mole of a gas at STP = 22.4 L/mol

Thus, 1 mole of O2 occupies the volume , V = 22.4 L/mol

Volume of oxygen at 20°C is calculated using:

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 22.4 * 20/25

V₂ = 17.92

Hence;

density = 32 g/17.92

Density = 1.78 g/L

In conclusion, density is ratio of mass and volume.

Learn more about density at: brainly.com/question/952755

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The Law of _____states that substances combine in predictable proportions and that excess reactants remain unchanged.

RideAnS [48]

Answer: definite proportions.

Explanation:

1) The definite proportions law states that compounds will always have the same kind of atoms (elements) in the same mass proportion (ratios).

2) For example, a molecule of water will alwys have the same mass ratio of hydrogen atoms to oxygen atoms. That is what permits to obtain the chemical formula of the water molecule as H₂O.

The mass of the two hydrogen atoms will be in a fixed ratio respect to the mass of the oxygen atoms.

Then, if you have one reactant in less proportion than the other, respect to the ratio stated by the chemical formula of water, the former will react completely (it is the limiting reactant) with the corresponding (proportional) mass of the later. Then there will be an excess of the later reactant which will not react (will remain unchanged).

The reactants can only react in the proportion defined by the chemical formulas of the final products.

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3 years ago

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For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts.

Nesterboy [21]

Answer:

0.712 mol of NO₂ are formed .

Explanation:

For the reaction , given in the question ,

2 N₂O₅ ( g ) → 4 NO₂ ( g ) + O₂ ( g )

From the above balanced reaction ,

2 mol of N₂O₅ reacts to give 4 mol of NO₂

Applying unitary method ,

1 mol of N₂O₅ reacts to give 4 / 2 mol of NO₂

From the question , 0.356 mol of N₂O₅ are reacted ,

now, using the above equation , to calculate the moles of the NO₂ , as follow -

Since ,

1 mol of N₂O₅ reacts to give 4 / 2 mol of NO₂

0.356 mol of N₂O₅ reacts to give 4 / 2 * 0.356 mol of NO₂

Calculating ,

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3 years ago

.7 liters of CO represents how many molecules?

Ronch [10]

Answer:

1.88 × 10²² Molecules of CO

Explanation:

At STP for an ideal gas,

Volume = Mole × 22.4 L/mol

Or,

Mole = Volume / 22.4 L/mol

Mole = 0.7 L / 22.4 L/mol

Mole = 0.03125 moles

Now,

No. of Molecules = Moles × 6.022 × 10²³ Molecules/mol

No. of Molecules = 0.03125 × 6.022 × 10²³ Molecules/mol

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Andre45 [30]

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NemiM [27]

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3 years ago

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