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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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A solid, pure substance containing just carbon and hydrogen is found to contain 35.8g of carbon and 3.72 g of hydrogen. how many
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Answer:

            4.36 g of Carbon

Solution:

Step 1: Calculate the %age of Carbon in given Solid as;

                        Mass of Carbon  =  35.8 g

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                        %age of Carbon  =  (35.8 g ÷ 39.52 g) × 100

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Step 2: Calculate grams of Carbon in 4.82 g of given solid as;

                        Mass of Carbon  =  4.82 g × (90.58 ÷ 100)

                        Mass of Carbon  =  4.36 g

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