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2 NO (9) 1. (2 pts) Use the following experimental data to write a Rate Law...
Use Hess' law and the data below to calculate AG, in kJ, for the following reaction: NO(g) + O (9) NO2 (g), AG° = ? 2 03 (9) - 3 O2 (g), AG° = +489.6 kJ 02 (9) 20 (9), AGⓇ = +463.4 kJ NO(g) + O2 (9) - NO2 (g) + O2 (g), AG° = -199.5 kJ QUESTION 14 Calculate AG for the following reaction, in kJ, at 0 °C under the following non-standard conditions shown below. 2 Hgo...
Given the values of K shown below, determine the value of K for the reaction, Ca(s) + 1/2 O2(g) + CO2(g) <=> CaCO3(s) Ca(s) + 1/2 O2(g) <=> CaO(s) K = 2,501 CaCO3(s) <=> CaO(s) + CO2(g) K = 8,808 Give your answer to 3 or 4 decimal places
2. (10 pts) Given the following data Ca(s)2C(graphite)CaC2(s) -62.8 kJ OH635.5 Ca(s)1/202(g) CaO(s) kJ CaO(s)H20()- Ca(OH)2(aq) OH 653.1 kJ 2CO2(g)H2O(l OH1300 C2H2(g)5/202(g) kJ C(graphite) O2(g)CO2(g) H= -393.5 kJ calculateH for the reaction (show your work for full credit) CaC2(s)+ 2H20()- Ca(OH)2(aq) CH2(g)
1. A gas is compressed from an initial volume of 5.35 L to a final volume of 1.23 L by an external pressure of 1.00 atm. During the compression the gas releases 124 J of heat. What is the change in internal energy of the gas? 2. Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ
Answer both question below. Show all work and chemical equations. 1. Using the information below answer questions a to c. Ca sº = 41.6 J/mol K CaCO3 (s) sº = 91.7 J/mol K AH° = -1207.6 kJ/mol O2 Sº = 205.2 J/mol K Cao (s) S0 = 38.1 J/mol K AH = -634.9 kJ/mol CO2 (g) sº = 213.8 J/mol K AH° = -393.5 kJ/mol AH° O2 = 0 kJ/mol AH° Ca= 0 kJ/mol a) Calculate AS9rxn and AH°rxn for...
Please answer the questions clearly, showing all working. 1(i). Balance the following equations, and then write the net ionic equation (a) (NH4)2CO3(aq) + Cu(NO3)2(aq) → CuCO3(s) + NH4NO3(aq) (b) Mg(OH)2(s) + HCl(aq) → MgCl2(aq) + H2O(l) (c) BaCO3(s) + HBr(aq) → BaBr2(aq) + H2O(l) + CO2(g) 1(ii). For each reaction equation, identify the driving force of the reaction 2. What is an electrolyte? How can you experimentally differentiate between a weak electrolyte and a strong electrolyte? Name and give the...
9. Consider the following reaction: inputted, <GO CaO(s) + CO2(g) - CaCO3(s); AG° = -130.9 kJ at 298 K At what partial pressure of CO2(g) will the reaction no longer be spontaneous at 298 K? (R- 0.0821 L.atm/(K.mol) = 8.31 J/(K.mol)) a. 1.59 x 108 atm b. 1.00 atm c. 6.28 x 10 atm d. 8.77 x 1022 atm e. 1.14 x 10-23 atm
Calculate AH for the following reaction, CaO(s) + CO2(g) CaCO3(s) given the thermochemical equations below. 2 Ca(s) + O2(g) + 2 Cao(s) AH = -1270.2 kJ C(s) + O2(g) CO2(g) AH = -393.5 kJ 2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) AH = -2413.8 kJ 0-750.1 kJ O +350.2 kJ 0 -178.3 kJ O +2870.6 kJ
Calculate AG for the following reaction at 25°C. 2 Ca(s) + O2(g) → 2 Ca(s) (J/K mol) Substance AH (kJ/mol AG (kJ/mol) Ca(s) Ca2+(aq) CaO(s) Ca(OH)2(5) CaF2(5) CaCl(s) O(g) 028) O3(aq) Oz(8) -542.96 -635.6 -986.6 -1,214.6 -794.96 249.4 -553.0 -604.2 -896.8 -1,161.9 -750.19 230.1 41.6 -55.2 39.8 83.4 68.87 113.8 160.95 205.0 110.88 237.6 -12.09 142.2 16.3 163.4
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ mol−1) CO2(g)CO2(g) −393.5−393.5 Ca(OH)2(s)Ca(OH)2(s) −986.1−986.1 H2O(l)H2O(l) −285.8−285.8 CaCO3(s)CaCO3(s) −1207−1207 H2O(g)H2O(g) −241.8−241.8 Part A: Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) C a ( O H ) 2 ( s ) + C O 2 ( g ) → C a C O 3 ( s ) + H 2 O ( l ) Express your answer in kJ mol−1 k J m o l...