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A Solution of Methanol and Water Has a Vapour Pressure

Question 119

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A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively.

A) $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.990, $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.010
B) $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.940, $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.060
C) $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.960, $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.040
D) $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.910, $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.090
E) $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.900, $A solution of methanol and water has a vapour pressure of 248 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively. A) = 0.990, = 0.010 B) = 0.940, = 0.060 C) = 0.960, = 0.040 D) = 0.910, = 0.090 E) = 0.900, = 0.100$ = 0.100

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