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6. Consider an ideal gas mixture composed of diatomic oxygen, carbon dioxide, and diatomic nitrogen with partial pressures of: 1) 35 kPa; 2) 25 kPa; and 3) 40 kPa, respectively. (A) Calculate the mass fraction (of all three components) (B) Calculate the mole fraction (of all three components) (C) Calculate the apparent Molar Mass (D) Calculate the ratio of specific heat at 300 K for the mixture

6. Consider an ideal gas mixture composed of diatomic oxygen, carbon dioxide, and diatomic nitrogen with partial pressures of: 1) 35 kPa; 2) 25 kPa; and 3) 40 kPa, respectively. (A) Calculate the mass fraction (of all three components) (B) Calculate the mole fraction (of all three components) (C) Calculate the apparent Molar Mass (D) Calculate the ratio of specific heat at 300 K for the mixture

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6. Consider an ideal gas mixture composed of diatomic oxygen, carbon dioxide, and diatomic nitrogen with partial pressures of: 1) 35 kPa; 2) 25 kPa; and 3) 40 kPa, respectively. (A) Calculate the mass fraction (of all three components) (B) Calculate the mole fraction (of all three components) (C) Calculate the apparent Molar Mass (D) Calculate the ratio of specific heat at 300 K for the mixture
Transcribed Image Text:6. Consider an ideal gas mixture composed of diatomic oxygen, carbon dioxide, and diatomic nitrogen with partial pressures of: 1) 35 kPa; 2) 25 kPa; and 3) 40 kPa, respectively. (A) Calculate the mass fraction (of all three components) (B) Calculate the mole fraction (of all three components) (C) Calculate the apparent Molar Mass (D) Calculate the ratio of specific heat at 300 K for the mixture
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