If 0.500 mol of a nonvolatile non electrolyte are dissolved in 3.20 mol of what

Question

If 0.500 mol of a nonvolatile non electrolyte are dissolved in 3.20 mol of what is the VAPOR pressure P_H_sO of the resulting solution? The vapor pressure of pure water is 23.8 ton at 25 Degree C. Express your answer numerically in torr Incorrect, Try Again;6 attempts remaining Solutions containing volatile solutes In solutions composed of two liquids(A and B), each liquid contributes to the total vapor pressure above the solution.T he total vapor pressure is the sum of the partial pressures of the components: P_total= P_A+P_B=N_AP_A degree +X_B P_B degree where P_A degree and P_B degree are the vapor pressures of pure A and B respectively. A solution is composed of 1.70 mol cyclohexane (P_cy degree= 97.6 torr) and 2.10 mol acelone. (P_ae degree = 229.5 torr). What is the total vapor pressure P_total above this solution?

Explanation / Answer

part A )

solute moles = n1 = 0.500

solvent moles = n2 = 3.20

mole fraction of solute = 0.5 / 0.5 + 3.20 = 0.135

Po - Ps / Po = mole fraction of solute

23.8 - Ps / 23.8 = 0.135

Ps = 20.58

PH2O = 20.58 torr

part B)

Ptotal = PA XA + PBXB

= 97.6 x 1.70 + 229.5 x 2.10

= 647.9 torr

total vapour pressure of the solution = 647.9 torr

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