Question

In: Chemistry

What are the values of q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following constant...

What are the values of q, w, ΔU, ΔH, ΔS, ΔS_surr, and ΔS_univ for the following constant pressure process for a system containing 0.137 moles of CH₃OH ?

CH₃OH(g, 122.0 ºC, 1.00 atm) ⟶ CH₃OH(l, 29.0 ºC, 1.00 atm)

Assume that CH₃OH(g) behaves as an ideal gas and the volume of CH₃OH(l) is much less than that of CH₃OH(g). Also, assume that the temperature of the surroundings is 29.0 ºC.

Data:

Molar heat capacity for CH₃OH(g), C_p,m = 44.1 J K⁻¹ mol⁻¹

Molar heat capacity for CH₃OH(l), C_p,m = 81.1 J K⁻¹ mol⁻¹

Enthalpy of vaporization, Δ_vapH = 35.2 kJ mol⁻¹ at 64.7 ºC and 1.00 atm

Enter answers that are accurate to three (3) or more significant figures.

q = ____________ J

w = ____________ J

ΔU = ____________ J

ΔH = ____________ J

ΔS = ____________ J K⁻¹

ΔS_surr = ____________ J K⁻¹

ΔS_univ = ____________ J K⁻¹

Expert Solution

queen_honey_blossom answered 10 months ago

Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn=...

Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 258 J/K , T= 294 K B. ΔH∘rxn= 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K C. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K . D. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 545 K . Predict whether or not the reaction in part A will be spontaneous. Predict whether or not the reaction in part...

Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn=...

Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 296 K Will this be spontaneous or not spontaneous? b) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 762 K Will this be spontaeous or not spontaneous? c) ΔH∘rxn= 87 kJ , ΔSrxn=− 146 J/K , T= 296 K will this be spontaneous or not spontaneous? d) ΔH∘rxn=− 87 kJ , ΔSrxn= 146 J/K ,...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Predict whether or not each...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Predict whether or not each reaction will be spontaneous. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 261 J/K , T= 294 K ΔSuniv = ??? (J/K) ΔH∘rxn= 118 kJ , ΔS∘rxn=− 261 J/K , T= 294 K . ΔSuniv = ??? (J/K) ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 261 J/K , T= 294 K . ΔSuniv = ??? (J/K) ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 261 J/K , T= 565 K . ΔSuniv...

Calculate w, q, ΔH, and ΔU for the process in which 1.78 moles of water undergoes...

Calculate w, q, ΔH, and ΔU for the process in which 1.78 moles of water undergoes the transition H2O(l,373K)→H2O(g,610.K) at 1 bar of pressure. The volume of liquid water at 373 K is 1.89×10−5 m3 mol−1 and the molar volume of steam at 373 K and 610. K is 3.03 and 5.06 ×10−2 m3 mol−1, respectively. For steam, CP,m can be considered constant over the temperature interval of interest at 33.58 J mol−1 K−1. Assume that the molar enthalpy of...

Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K...

Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K for the reaction below. Enter all values to the 0.1 place. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔS° ΔH° ΔG°

Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs...

Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs free energy change for the production of following metallic elements from their ore sources: (a) 2ZnO(s) 2Zn(s) + O2(g) (b) 2CaO(s) 2Ca(s) + O2(g) (c) 2Al2O3(s) 4Al(s) + 3O2(g) (d) 2MgO(s) 2Mg(s) + O2(g)

Classify the following phase changes by the signs of the system's ΔH and ΔS.

From the following combinations of ΔH and ΔS, predict if a process will be spontaneous at...

From the following combinations of ΔH and ΔS, predict if a process will be spontaneous at a high or low temperature: (a) both ΔH and ΔS are negative, (b) ΔH is negative and ΔSis positive, (c) both ΔH and ΔS are positive, (d) ΔH is positive and ΔS is negative.

Which of the following processes are spontaneous? For each process also indicate whether ΔS, ΔSsurr,and ΔSuniv,...

Which of the following processes are spontaneous? For each process also indicate whether ΔS, ΔSsurr,and ΔSuniv, are positive, negative or zero: a. The freezing of supercooled liquid water at −3°C and 1 bar. b. The freezing of liquid water at 0°C and 1 bar by removing a small amount of heat. c. The adiabatic expansion of a van der Waals gas into a vacuum. d. The reversible isothermal compression of an ideal gas

For a reaction with ΔH∘=−24 kcal/mol and ΔS∘=0.07 kcalmol−1K−1, calculate the equilibrium constant at: (1.) 30...

For a reaction with ΔH∘=−24 kcal/mol and ΔS∘=0.07 kcalmol−1K−1, calculate the equilibrium constant at: (1.) 30 ∘C and (2.) 150 ∘C.