For a certain process, at 300. K, G = –14.1 kJ and H = –7.0 kJ. If the process is carried out reversibly, what is the amount of useful work that can be performed?
Ans: 14.1 kJ
15. Consider the reaction 2 NO2(g) N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and Gf NO2(g) = 51.3 kJ/mol, calculate G° at 298 K. kJ (b) Calculate G at 298 K if the partial pressures of NO2 and N2O4 are 0.35 atm and 1.60 atm, respectively. kJ 16. Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ (b) Calculate G at 298 K...
Given this balanced chemical reaction, 4 HCl(g) + O(g) →2 HO(l) + 2 Cl(g) H = -202.4 kJ (give answer in decimal notation, i.e. 234,000) a. How many J (joules) of heat are released when 2.50 moles of HCl react with excess oxygen gas? We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
NH4NO3 (s) NH4+ (aq) + NO3- (aq) H°f NH4NO3 (s) = -365.6 kJ/mol H°f NH4NO3 (aq) = -339.9 kJ/mol What is H°rxn? We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
h(k) = k mod 701 = 9 and 0 k 2000 , find two keys for which h(k) = 9 If k2= k1 +1 what can you say about h(k1) and h(k2) We were unable to transcribe this imageWe were unable to transcribe this image
A Reaction is given: ½Br2(l) --> Br(g) Ho = 112kJ/mol The bond enthalpy of Br-Br is 193 kJ/mol A. Formulate the vaporization process of 1 mol bromine Br2(l). B. Calculate the enthalpy of the vaporization process bromine. Show calculations C. Calculate the energy invested \ emitted by the evaporation of 3.2 gr of bromine. Show calculations. (Explain how you determined whether the energy is invested or emitted in this process). D.A Reaction is given: ½H2(g) + ½Br2(l) --> HBr(g) Ho...
The change in free energy of a certain process is equal to 4.000 kJ at 400.K and is equal to 2.000 kJ at 350.K. Assuming both the enthalpy and the entropy changes for the process are independent of temperature between 200.K and 400.K, determine the temperature in kelvin where this process occurs reversibly.
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3, 40 a 298 K. What is Delta G^Compositefunction for the following equilibrium? HA (aq) + H_2O(l) rightarrow leftarrow H_2O(aq) = A(aq) A) 7.95 kJ B) 30.8 kJ C) 11.4 kJ D) 19.4 kJ For a reversible phase change at constant temperature and pressure. A) Delta U = 0. B) Delta H = 0. C) w = 0 D) q = 0 E) Delta G...
do part f 7. Consider the following data: C2H6(g) -84.7 32.9 H2O(l) 285.9 -237.2 CO2(g) -393.5 -394.4 Ho kl/mole) a) Calculate the entropy change for the combustion of 1.0 mole of C,H,(g) at 25°C. b) Are the products more or less ordered than the reactants at 25 c) Is the reaction spontaneous at 25°C? d) Wh at is the maximum amount of useful work which can be obtained from the process at 25°C? e) If the process is carried out...
An experiment was performed to determine the Hsoln of the dissolution process of urea(CO(NH2)2(s)) in water. 95.91 grams of water was put in a calorimeter and 13.5 grams of solid urea was added. The initial temperature of Water is the same as that of urea. Below is a graph describing the temperature change over time of a process Dissolving the urea in the water. A. What is the change in temperature due to the dissolution of urea? B. Based on...
When a 5.12-g sample of solid sodium nitrate dissolves in 31.1 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 25.00 oC to 16.37 oC. Calculate H in kJ/mol NaNO3 for the solution process. NaNO3(s) Na+(aq) + NO3-(aq) The specific heat of water is 4.18 J/g-K. We were unable to transcribe this imageWe were unable to transcribe this imagethermometer stirrer coffee cups containing reaction mixture When a 5.12-g sample of solid sodium nitrate dissolves in...