Consider the following reaction and the corresponding thermodynamic data to answer the next two problems.
CaCO3 (s) ( CaO (s) + CO2 (g) (Ho rxn = 179.2 kJ/mol; (So rxn = 160.2 J/mol K
What can be stated regarding the spontaneity of this chemical reaction?
a) This reaction is spontaneous at all temperatures.
b) This reaction is spontaneous above 894K and non-spontaneous below 894 K.
c) This reaction is spontaneous below 894 K and non-spontaneous above 894 K.
d) This reaction is spontaneous above 1119 K and non-spontaneous below 1119 K.
e) This reaction is spontaneous below 1119 K and non-spontaneous above 1119 K.
What is the value of the Gibbs Free Energy change, (Grxn for this reaction at 100 oC?
a) (Grxn = -5.96 x 104 kJ/mol b)
b) (Grxn = 119.4 kJ/mol c)
c) (Grxn = 163.2 kJ/mol
d) (Grxn = 195.2 kJ/mol e)
e) (Grxn = 239.0 kJ/mol
please please please show how to do the problems! i have an answer key but i am trying to prepare for a test and i dont understand.
Consider the following reaction and the corresponding thermodynamic data to answer the next two problems. CaCO3...
Please don't forgot to calculate the temperature at which the reaction switches . 1. Given the following information, calculate the standard Gibbs free energy of the reaction at 1455 K. State if the reaction is spontaneous or nonspontaneous followed by the temperature at which the reaction switches spontaneity if applicable CaCO3(s) → CaO(s) + CO2(g) Given: Δ"H = 179.2 kJ , Δ"S = 160.2 J/K
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 185.98 kJ/mol ΔS∘rxn 27.40 J/(mol⋅K) Calculate the temperature in Kelvin above which this reaction is spontaneous. Express your answer to 0 decimal places and in K.
part 1 answer is correct. Looking for #2 on this sheet with work please Verarbon dia Gibbs Free Energy & Predicting Spontaneity 1) The decomposition of calcium carbonate into calcium oxide and carbon dioxide (shown below) is not spontaneous at 298 K. CaCO (8) Cao(8) + Co.g) AH = +179 28 Using the data provided above, calculate the value of Great 298 K. 10- +160.29 179.2151005 AGO - DHOTOS I min hof amor AG° = 179200 Frei- 298(160.23imo) DGO=131460.45 sco=131.4605lmo...
Consider the reaction: 2NO(g) + Cl2(g) → 2NOCI(g) Given the following table of thermodynamic data, Substance NO (g) Cl2(g) NOCI (g) AH (kJ/mol) 90.3 0 sº (/mol.K) 210.7 223.0 51.7 261.6 Calculate Ahºrxn and AS rxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous.
Given the following reaction and thermodynamic data: A(g) - B(g AH = -42.3 kJ/mol; AS = -125.2 J/(mol*K) Is this reaction spontaneous or non-spontaneous? Select one: a. non-spontaneous. o b. spontaneous. c. more information is needed to determine.
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
Consider the reaction: 2NO(g) + Cl2(g) 2NOCl(g) Given the following table of thermodynamic data, Substance ∆Hfo (kJ/mol) So (J/molK) NO (g) 90.3 210.7 Cl2 (g) 0 223.0 NOCl (g) 51.7 261.6 Calculate ∆Horxn and ∆Sorxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous. Please show all work. Provide equations used. Please use correct significant figures and correct units in answers.
4. Consider the reaction 3 C (graphite)2 H2O (g) CH4 (g) 2 CO (g) The following data are needed (all are at 298 K): S(J mol K) AH(kJ mol AAG(kJ mol) compound C, graphite 0 5.740 Н.О (g) - 241.82 188.83 - 228.57 CH4 (g) 186.26 -74.81 - 50.72 СО (g) 197.67 - 137.17 - 110.53 a) Determine A,G° and K for this reaction at 298 K and comment on the spontaneity of this process b) If you find that...
A.) For the decomposition of barium carbonate, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the temperature in kelvins above which this reaction is spontaneous. B.) The thermodynamic values from part A will be useful as you work through part B ΔH∘rxn243.5kJ/mol ΔS∘rxn172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C: BaCO3(s)→BaO(s)+CO2(g)
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 179.97 kJ/mol ΔS∘rxn 22.99 J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 295.9 K: Whatever answer you get multiply by 1x1031 and enter that number to 4 decimal places.