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TEA [102]
3 years ago
8

Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of the pressures exert

ed independently by each gas in the mixture. True False
Chemistry
1 answer:
Damm [24]3 years ago
5 0

Answer: The given statement is true.

Explanation:

According to the Dalton's law, total pressure of a mixture of gases that do not react with each other is equal to the partial pressure exerted by each gas.

The relationship is as follows.

          p_{total} = \sum_{i=1}^{n} p_{i}

or,        p_{total} = p_{1} + p_{2} + p_{3} + p_{4} + ......... + p_{n}

where,  p_{1}, p_{2}, p_{3} ....... = partial pressure of individual gases present in the mixture

Also, relation between partial pressure and mole fraction is as follows.

                 p_{i} = p_{total} \times x_{i}

where,      x_{i} = mole fraction

Thus, we can conclude that the statement Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of the pressures exerted independently by each gas in the mixture, is true.              

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Option C.

<h3><u>Explanation:</u></h3>

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Here in this diagram, we can see that the points A and B are the north pole and the part in northern hemisphere respectively which aren't facing the sun directly, whereas C and D are facing the sun. Thus the southern hemisphere is experiencing summer and the northern hemisphere the winter.

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2 years ago
During an endothermic phase change, what happens to the potential energy and the kinetic energy?
Dovator [93]
The correct answer should be that Potential energy increases, and kinetic energy increases, since they both increase as the temperature changes.
7 0
2 years ago
Read 2 more answers
What is the molar mass, in grams, of a mole of an element equal to?
insens350 [35]

Answer:

B. the atomic weight of the element

Explanation:

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5 0
3 years ago
What is the density of a substance that has a mass of 453g and a volume of 224mL?
Savatey [412]
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3 years ago
Urea, CH4N2O (s), is manufactured from NH3 (g) and CO2 (g). H2O (l) is another product of this reaction. An experiment is starte
Katarina [22]

Answer:

a. 4.41 g of Urea

b. 1.5 g of Urea

Explanation:

To start the problem, we define the reaction:

2NH₃ (g) +  CO₂ (g) → CH₄N₂O (s)  +  H₂O(l)

We only have mass of ammonia, so we assume the carbon dioxide is in excess and ammonia is the limiting reactant:

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Formula is (Yield produced / Theoretical yield) . 100 → Percent yield

3 0
3 years ago
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