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According to Dalton's law the total pressure of the mixture of gases is equal to
- a)greater of the partial pressures of all
- b)average of the partial pressure of all
- c)sum of the partial pressures of all
- d)sum of the partial pressure of all divided by average molecular weight
- e)atmospheric pressure.
Correct answer is option 'C'. Can you explain this answer?
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According to Dalton's law the total pressure of the mixture of gas...
Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
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According to Dalton's law the total pressure of the mixture of gas...
Dalton's law states that the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of each individual gas in the mixture. In other words, the total pressure exerted by a mixture of gases is the sum of the pressures that each gas would exert if it alone occupied the same volume at the same temperature.
Let's break down the answer and explain it in detail:
Dalton's Law:
Dalton's law is based on the concept that gases behave independently of each other in a mixture. According to this law, the total pressure exerted by a mixture of gases is equal to the sum of the pressures exerted by each individual gas, assuming ideal gas behavior.
Partial Pressure:
Partial pressure is the pressure exerted by a single gas in a mixture, assuming it occupies the same volume at the same temperature as the mixture. It is proportional to the mole fraction of that gas in the mixture. Mathematically, the partial pressure of a gas can be calculated using the following equation:
Partial Pressure = Total Pressure * Mole Fraction
Total Pressure of the Mixture:
The total pressure of a mixture of gases is the overall pressure exerted by the entire mixture. It is the sum of the partial pressures of each gas in the mixture. Therefore, option 'C' is correct, as it states that the total pressure of the mixture is equal to the sum of the partial pressures of all gases.
Explanation:
When multiple gases are present in a mixture, each gas exerts its own pressure based on its concentration and temperature. The total pressure of the mixture is the sum of these individual pressures. This can be understood by considering a container divided into multiple compartments, each containing a different gas. The pressure exerted by each gas in its respective compartment is the partial pressure. The combined pressure of all compartments is the total pressure of the mixture.
Example:
Let's consider a mixture of two gases, A and B, in a container. If the partial pressure of gas A is PA and the partial pressure of gas B is PB, then the total pressure of the mixture would be PA + PB.
In conclusion, Dalton's law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas in the mixture. Therefore, option 'C' is the correct answer.
Let's break down the answer and explain it in detail:
Dalton's Law:
Dalton's law is based on the concept that gases behave independently of each other in a mixture. According to this law, the total pressure exerted by a mixture of gases is equal to the sum of the pressures exerted by each individual gas, assuming ideal gas behavior.
Partial Pressure:
Partial pressure is the pressure exerted by a single gas in a mixture, assuming it occupies the same volume at the same temperature as the mixture. It is proportional to the mole fraction of that gas in the mixture. Mathematically, the partial pressure of a gas can be calculated using the following equation:
Partial Pressure = Total Pressure * Mole Fraction
Total Pressure of the Mixture:
The total pressure of a mixture of gases is the overall pressure exerted by the entire mixture. It is the sum of the partial pressures of each gas in the mixture. Therefore, option 'C' is correct, as it states that the total pressure of the mixture is equal to the sum of the partial pressures of all gases.
Explanation:
When multiple gases are present in a mixture, each gas exerts its own pressure based on its concentration and temperature. The total pressure of the mixture is the sum of these individual pressures. This can be understood by considering a container divided into multiple compartments, each containing a different gas. The pressure exerted by each gas in its respective compartment is the partial pressure. The combined pressure of all compartments is the total pressure of the mixture.
Example:
Let's consider a mixture of two gases, A and B, in a container. If the partial pressure of gas A is PA and the partial pressure of gas B is PB, then the total pressure of the mixture would be PA + PB.
In conclusion, Dalton's law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas in the mixture. Therefore, option 'C' is the correct answer.
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According to Dalton's law the total pressure of the mixture of gas...
C
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According to Dalton's law the total pressure of the mixture of gases is equal toa)greater of the partial pressures of allb)average of the partial pressure of allc)sum of the partial pressures of alld)sum of the partial pressure of all divided by average molecular weighte)atmospheric pressure.Correct answer is option 'C'. Can you explain this answer?
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