3. Trouton's rule a. Estimate the molar enthalpy of vaporization, AvapHm, of formic acid using Trouton's rule. The normal boiling point of formic acid is 100.8 °C and its chemical formula is CH₂O₂.
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- At 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa. Use this information to estimate the enthalpy of vaporization for ethanol.Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).The vapor pressure of ethanol is 24.1 Torr at 10C and 44.0 Torr at 20C. Calculate the enthalpy of vaporization of ethanol over this temperature range.
- Consider the following equilibrium: 2 HI (g) 4 H2 (g) + 12 (g) Kp at 1000 K is equal to 29.1. Calculate the value of Kc at this temperature.C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalystAt 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53-3 kPa. Use this information to estimate the enthalpy of vaporization for ethanol. OkJ/mol
- A 65.0 g piece of gold at 650 K is dropped into 162 g of H2O(l) at 298 K in an insulated container at 1 bar pressure. CP,m for Au and H2O at 298 K are 25.4 and 75.3 J⋅K−1⋅mol−1, respectively. Calculate the temperature of the system once equilibrium has been reached. Assume that CP,m for Au and H2O are constant at their values for 298 K throughout the temperature range of interest.1. Which, if any of the following, constitute a closed system?(a) A sealed container in which a chemical reaction occurs.(b) A dog.(c) An open beaker in the lab, in which a reaction occurs.(d) A mixture of gases inside a sealed impenetrable balloon. 2. What is the definition of an isolated system? How could you approximate anisolated system in the lab?Calculate the vapor pressure of ethnaol at 25 Celsius. Assume the thermodynamic values are independent of temperature
- Calculate the enthalpy of vaporization of SO2 at –25°C if the same at its boiling point (i.e. –10°C) be 5950 cal mol–1. Given for SO2, molar heat capacities in liquid and vapor phase are 206 cal K–1 mol–1 and 9.3 cal K–1 mol–1 respectively.A geochemist in the field takes a small sample of the crystals of mineral compound X from a rock pool lined with more crystals of X. He notes the temperature of the pool, 17.° C, and caps the sample carefully. Back in the lab, the geochemist dissolves the crystals in 4.00 L of distilled water. He then filters this solution and evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 0.080 kg. Using only the information above, can you calculate the solubility of X in water at 17.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. O yes O no 0 0 x10 ロ・ロ x 3 00 5Calculate the value of K, for the equation C(s) + CO, (g) =2 CO(g) Kp = given that at a certain temperature C(s) + 2 H,O(g) F CO,(g) + 2H,(g) = H, (g) + CO, (g)=H,O(g) + CO(g) Kp2 = 0.695 Kp