4. a. Consider the data below for the reaction H2Ou) = H2O() - Plot a graph and determine AH and AS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 000

4. a. Consider the data below for the reaction H2Ou) = H2O() - Plot a graph and determine AH and AS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 000

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 85QAP: Which of the following quantities can be taken to be independent of temperature? independent of...

See similar textbooks

Similar questions

For the process H2O(l)H2O(g) at 298 K and 1.0 atm, H is more positive than E by 2.5 kJ/mol. What does the 2.5 kJ/mol quantity represent?
A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour. Given the following data, determine Hf for the hydrocarbon: Hreaction=2044.5KJ/molhydrocarbonHf(CO2)=393.5KJ/molHf(H2O)=242KJ/mol Density of CO2 and H2O product mixture at 1.00 atm, 200.c = 0.751g/L. The density of the hydrocarbon is less than the density of Kr at the same conditions.
In the laboratory, hydrogen chloride (HCl(g)) and ammonia (NH3(g)) often escape from bottles of their solutions and react to form the ammonium chloride (NH4Cl(s)), the white glaze often seen on glassware. Assuming that the number of moles of each gas that escapes into the room is the same, what is the maximum partial pressure of HCl and NH3 in the laboratory at room temperature? (Hint: The partial pressures will be equal and are at their maximum value when at equilibrium.)
a. Consider the data below for the reaction H2O(l) ⇌ H2O(g) . Plot a graph and determine ΔH and ΔS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 90.0 525.8 Explain how the boiling point temperature of H2O(l) (at sea level) can be accurately determined from the data in a.? c. For the reaction in a., ΔE is less than ΔH. Explain.
a.Consider the data below for the reaction H2O(l) ⇌ H2O(g) . Plot a graph and determine ΔH and ΔS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 90.0 525.8
Consider the data provided for the following rxn: H2O(l)⇌ H2O(g) a. Plot a graph and determine the ∆H and ∆S for the reaction. describe how they influence the spontaneity of the reaction as a function of temperature. T(°C): 0.0, 10.0, 20.0, 25.0, 30.0, 40.0, 60.0, 70.0, 90.0 P(torr): 4.579, 9.209, 17.53, 23.76, 31.82, 55.32, 149.4, 233.7, 525.8 b. explain how the boiling temperature of H2O(l) (at sea level) can be accurately determined from the data in a? c. for the reaction in a, ∆E is less than ∆H. Explain why.
Consider the data below for the reaction H2O (l) = H2O (g). Plot a graph and determine deltaH and deltaS for the reaction. Describe how they influence the penitent of the reaction as a function of temperature. Data: T (degree Celsius) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 90.0 525.8 Explain how the boiling point temperature of H2O(l) (at sea level) can be accurately determined from the above data?
The thermal decomposition of ethylene occurs in manyindustrial contexts, for example, during ethylene transit inpipelines, formation of polyethylene, drying of the gas, and sep-arating it from impurities. The decomposition reaction is CH₂=CH₂(g)→CH₄(g)+C(graphite) .Assume that the decomposition begins at 10°C and 50.0 atm with agas density of 0.215 g/mL and the temperature increases by 950 K.What is the final pressure of the confined gas (ignore the vol-ume of graphite and use the van der Waals equation)?
A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.
A 10.0L can at 20ᵒC has a pressure of .90atm, what pressure will it have in a hot car that is 50ᵒC?
A series of reactions carried out in separate containers at a constant volume and a constant pressure. For each reaction, what is the ratio of the final temperature to the intial temperature? (enter answers as simplified ratios) 1) Cl2(g) +H2(g) --> 2HCl(g) 2) CH4 +2O2(g) --> CO2(g) + 2H2O(g) 3) S(g) + H2(g) --> H2S(g) 4) C2H4(g) + 3O2(g) --> 2CO2(g) + 2H2O(g)
Calculate the degree of decomposition of n2O4 to NO2(g) at 0.49 bar total pressure and 300K. If the temperature increases to 600C, how does the degree of decomposition change (increase-decrease) and why?