If a mixture of CO_2 and O_2 occupies a volume of 1 m63 at a temperature of 28 d

Question

If a mixture of CO_2 and O_2 occupies a volume of 1 m63 at a temperature of 28 degree C and is at a pressure of 1.5 atm (equal) to the sum of partial pressures of the two gases), then O_2 alone in the mixture is at a temperature of ____ degree C. A 14 B. 56 C. 28 D. depends on mole fraction of O_2 E. depends on CO_2 temperature F. How do I know? Ask O_2. If a mixture of 1 kg of CO_2 and 2 kg of O_2 occupies a volume of 3 m63 at a temperature of 28 degree C and is at a pressure of 1.5 atm (equal to the sum of partial pressures of the two gases), then CO_2 alone in the mixture occupies a volume of ____ m^3 A. 1 B. 2 C. 3 D. depends on mole fraction of CO_2 E. depends on CO_2 mass F. How do I know? Ask CO_2. If a gas mixture consists of 1 kg of CO_2 and 2 kg of OO_2, the mass of the mixture is 3 kg. A. 1 B. 1.5 C. 2 D. 3 E. whatever is If a gas mixture consists of 1 mole of CH_4 and 2 moles of O_2 the number of moles of the mixture is: A. 1 B. 1.5 C. 2 D. 3 E. whatever it is Mass fraction of gas a in a mixture of gases is A. the ratio of mass of gas A to the total mixture mass B. the difference of the total mixture mass and the sum of masses of the remaining gases C. the average of masses of all the gases in the mixture D. it depends on the volumes occupied by the gases in the mixture Molar mass of a gas mixture can be calculated as: A. the average of molar masses of all the gases in the mixture B. the sum of mass-weighted average of each gas in the mixture C. the sum of molar masses of all the gases in the mixture D. none of the above A gas mixture at a temperature of 28 degree C and a pressure of 1.5 atm has 1 kg of N_2 (occupies a partial volume of a m^3) and 2 kg of O_2 (occupies a partial volume of b m^3). The volume occupied by this gas mixture is C m63 A. a-b B. a + b C. (a + b)/2 D. (a - b)2 e. [(1 kg middot a) + (2 kg middot b)] (1 + 2)kg If a mixture of CH_4 and C_3H_8 occupies a volume of 1 m63 (equal to the sum of partial volumes of the two gases) at a temperature of 28 degree C and at a pressure of 1.5 atm, then CH)4 alone in the mixture is at a temperature of C degree C. A. 14 B. 56 C. 28 D. depends on mole fraction of CH_4 e. room temperature

Explanation / Answer

1) Volume of the mixture of gases, V = 1 m3

Temperature of the gas mixture = 28C

Total pressure of the system = 1.5 atm.

Since the system temperature is 28C, both the gases will be at the same temperature, 28C. Otherwise, cooling of the gas mixture will take place and that is clearly not a case here. Hence, the O2 alone will be at a temperature of 28C.

Ans: (C) 28

2) The volume occupied by CO2 will depend on the mole fraction of CO2 as well as the density of the gas mixture. Hence (D) is the correct answer.

Ans: (D)

3) The total mass of the gas mixture is the sum total of the masses of the components present. Hence the total mass of the gas mixture = (1 + 2) kg = 3 kg.

Ans: (D) 3

4) The number of moles present in a gaseous mixture is the sum of the moles of each gas present. Hence, the total number of moles present in the mixture = (1 + 2) mole = 3 mole.

Ans: (D) 3

5) Mass fraction of a gas A in a mixture of gases is obtained by dividing the mass of A by the total mass of the gas mixture. Hence, (A) is the correct answer.

Ans: (A)

6) Molar mass of a gas mixture is not simply the sum of the molar masses of the gases. Infact, it is not even an average of the molar masses of the gases present in the mixture. A best approximation is to multiply the percentage of each gas in the mixture by their individual molar masses to arrive at the sum-weighted mass fraction. Hence, (B) is the right answer.

Ans: (B)

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