(a)
Interpretation:
The pressure of the vapors of benzene is to be calculated under the given conditions.
Concept Introduction :
The ideal gas equation is the expression that relates different measurable properties of a gas. The expression is given as:
where,
P = Pressure of the gas
V = Volume of the container in which the gas is occupied
R = Ideal gas constant = 0.0821 L atm/ mol K
n = number of moles of the gas = Mass of gas / Molecular mass of gas
T = Absolute temperature of the gas i.e., temperature on Kelvin scale
(b)
Interpretation:
The pressure calculated in part (a) are to be compared with the equilibrium pressures of benzene.
Concept Introduction :
If the pressure of vapors is more than the equilibrium pressure, it indicates that the liquid has undergone condensation.
(c)
Interpretation:
The pressure of benzene vapors inside the flask is to be calculated at 50 0C and 60 0C.
Concept Introduction : When a liquid is present in a closed container, it starts to form vapors above the liquid surface. A stage is reached when the liquid and vapors are present in equilibrium with each other.
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Chapter 9 Solutions
Chemistry: Principles and Reactions
- Suppose you have 600.0 grams of room temperature water (20.0 degrees Celsius) in a thermos. You drop 90.0 grams of ice at 0.00 degrees Celsius into the thermos and shut the lid.(a) What is the equilibrium temperature of the system? (b) How much ice is left (in grams)? Provide a step-by-step explanation for how you arrived at your solution as though you were teaching a student to solve this type of problem.arrow_forward3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBr is -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number.…arrow_forward3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBris -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number. (c) Would you expect this compound to be soluble in water? Why/Why not? Calculate anything you need in order to figure this out, and explain your answer.arrow_forward
- 5. (a) The melting point of ammonia (NH3) is higher than that of methane (CH4) and yet these molecules have comparable molecular mass. Why does NH3 have a higher melting point than CH4? Explain in terms of intermolecular forces. (b) Predict the solubility of HF, HCl and Cl2 in water and explain your answer.arrow_forwardAt 20.0 °C, the vapor pressure of cyclohexane, a nonpolar hydrocarbon, is 66.9 torr and that of toluene, a hydrocarbon related to benzene, is 21.1 torr. Calculate the expected vapor pressure of a mixture of cyclohexane and toluene that consists of 124 grams of each liquid. Ptotal= torrarrow_forwardAcetonitrile, CH3CN, has a vapor pressure of 88.8 torr at 25.0 ̊C. If 9.22 mL of liquid acetonitrile (MCH3CN = 41.05 g/mol, dCH3CN = 0.786 g/mL) is placed into a sealed 5.25 L container at 25.0 ̊C and allowed to reach equilibrium. What would the value of [grams of CH3CN(g)/ grams of CH3CN(l)] in the container be at equilibrium?.arrow_forward
- Consider the following reaction: Zn + 2HCl(aq) (s) ---> ZnCl2 (aq) + H2(g) Zinc metal is added to hydrochloric acid to generate hydrogen gas and is collected over a liquid whose vapor pressure is the same as that of pure water at 20.0°C (18 torr). The volume of the mixture is 1.7 L, and its total pressure is 0.792 atm. Determine the number of moles of hydrogen gas present in the sample.arrow_forwardCalculate the change in the chemical potential of liquid water and water vapor when the pressure is increased from 1.0 atm to 10 atm at 100°C. Discuss the effect of the pressure increase on the equilibrium between the liquid water and the water vapor. Assume that water vapor behaves perfectly and the density of water is 1 g/cm3.arrow_forward(a) Temperature dependence of the vapor pressure of ethylene log p (mm Hg) = - 834.13 / T + 1.75 log T - 8.375 x 10-3 T + 5.3234 , which gives the temperature dependence of the molar enthalpy of vaporization derive the equation. (b) Calculate the molar enthalpy of evaporation at -103.9 oC, the normal boiling point of ethylene. Note: Use the equation that gives the temperature dependence of ΔHvap= a + bT + cT2+ ….enthalpy.arrow_forward
- Part A What is the value of A-G for the reaction MCI, 6 H₂O(s) MCL, (s) + 6 H₂O(g) - when the pressure of water vapour is 28.7 mbar? Express your answer as an integer with the appropriate units. A.G= Value μA Submit Request Answer Part B A.G' = What is the value of A,C? Express your answer with the appropriate units. μA Units Value Units ? Submit Previous Answers Request Answer Un input for part B ? X Incorrect; Try Again; 5 attempts remainingarrow_forwardNaphthalene undergoes sublimation: C10H3(s)C10Halg). In a closed container at 800.0 K, the equilibrium vapor pressure is 0.70 torr. What is the value of K? Type your answer.arrow_forwardA mixture with a total mass of 1.67 g contains sucrose and ethyl alcohol. This mixture is reacted with acidic aqueous potassium dichromate. 2.36 L CO₂ (g) coming from the reaction accumulates on water at 35 ˚C and has a pressure of 0.48 atm. If the vapor pressure of the water at this temperature is 42.20 mmHg, what is the percentage by mass of C₆H₁₂O₆ in the mixture? (C₆H₁₂O₆, 342.30 g mol⁻¹ and C₂H₆O, 46.07 g mol⁻¹) C₆H₁₂O₆ (aq) + Cr₂O₇²⁻ (aq) → CO₂ (g) + Cr⁺ᶾ (aq) (unbalanced) C₂H₆O (aq) + Cr₂O₇²⁻ (aq) → CO₂ (g) + Cr⁺ᶾ (aq) (balanced)arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning