(a)
Interpretation:
Whether the given cis-trans isomerization reaction of gaseous 2-butene is a product-favoured reaction or not has to be given.
Concept Introduction:
Equilibrium Constant & Direction of reaction:
Case 1:
Reaction is strongly product-favoured; equilibrium concentrations of products are much greater than equilibrium concentrations of reactants.
Case 2:
Reaction is strongly reactant-favoured; equilibrium concentrations of reactants are much greater than equilibrium concentrations of products.
Case 3:
Equilibrium mixture contains significant concentrations of reactants and products; calculations are needed to determine equilibrium concentrations.
(b)
Interpretation:
The amount (in moles) of trans iosmer produced when
Concept Introduction:
Equilibrium constant: At equilibrium the ratio of products to reactants (each raised to the power corresponding to its
For a general reaction,
The concentration of solids and pure liquids do not change, so their concentration terms are not included in the equilibrium constant expression.
(c)
Interpretation:
The amount (in moles) of trans iosmer produced when
Concept Introduction:
Refer part (a).
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Chemistry: The Molecular Science
- (a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at 127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction. (b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.arrow_forward2. An experiment was carried out to determine the enthalpy change of combustion of propan-1-ol. The experimental set-up was shown below. a beaker water (500.0 cm³) propan-1-ol (a) Write the equation for the complete combustion of propan-1-ol (C;H¬OH). (b) Give a suggestion to the above set-up so as to minimize heat loss to the surroundings. (c) Burning 2.88 g of propan-1-ol caused the temperature of 500.0 cm³ of water to rise by 46.0°C. Calculate the enthalpy change of combustion of propan-1-ol. (Assume that the specific heat capacity and the density of water are 4.2 J g- K-l and 1.0 g cm- respectively.) (Molar mass of propan-1-ol: 60 g) -3 (d) The enthalpy change obtained in (c) cannot be called as 'standard enthalpy change'. Explain why.arrow_forwardFor a reaction with ?H° = 40 kJ/mol, decide which of the following statements is (are) true. Correct any false statement to make it true. (a) The reaction is exothermic; (b) ?G° for the reaction is positive; (c) Keq is greater than 1; (d) the bonds in the starting materials are stronger than the bonds in the product; and (e) the product is favored at equilibrium.arrow_forward
- For a reaction with ΔHo = 40 kJ/mol, decide which of the following statements is (are) true. Correct any false statement to make it true. (a) The reaction is exothermic; (b) ΔGo for the reaction is positive; (c) Keq is greater than 1; (d) the bonds in the starting materials are stronger than the bonds in the product; and (e) the product is favored at equilibrium.arrow_forwardCalculate AH for the reaction NH3 (g) + CH4 (g) → HCN (g) + 3 H2 (g) , from the following data. N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔΗ- – 91. 8 kJ /mol C (s, graphite) + 2 H2 (g) → CH4 (g) - 74. 9 kJ / mol AH = 2 C (s, graphite) + H2 (g) + N2 (g) → 2 HCN (g) AH = ΔΗ: 270. 3 kJ / molarrow_forward(b) Study the following themochemical data very carefully: Ciz(g) - 2ci(g) I2(g) IC(g) - 1(g) + CI(g) I2(s) → 12(g) AH° = 242.3 kJ AH° = 151.0 kJ 21(g) AH° = 211.3 kJ AH° = 62.8 kJ I2(s) reacts with Cl2(g) to produce ICI(g). Write the chemical equation to produce ONLY one mole of ICI(g) (i) Calculate AH° for the reaction of I2(s) with Cl2(g) to form 1 mole of ICI(g). Use all the data given above. (ii) What law did you use to calculate AH° above? (iii) What are the names of the following processes? I2(s) → 12(g) I2(g) 21(g) ICI(g) I(g) + Cl(g)arrow_forward
- Calculate AH for the reaction NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g), from the following data. N2 (g) + O2 (g) → 2 NO (g) ΔΗ - 180.5 kJ / mol N2 (g) + 3 H2 (g) → 2 NH3 (g) /mol AH = - 91. 8 kJ 2 H2 (g) + O2 (g) → 2 H20 (g) AH ΔΗ- - 483. 6 kJ / molarrow_forwardCalculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N20(g) → 4N2(g) + 3H2O(1) AH = –1010. kJ N20(g) + 3H2 (9) → N¿H4(1)+H2O(1) AH = -317 kJ N2H4 (1) + O2 (g) → N2(g)+ 2H2O(1) AH = -623 kJ H2 (9) + 02 (9) → H2O(1) AH = -286 kJ ΔΗ - kJarrow_forwardWhat is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 Question 5 options: 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1arrow_forward
- 1. The enthalpy of neutralization of a newly discovered compound, J(OH)3, was determined using a styroball calorimeter. The calorimeter was first calibrated using 13.00 mL of 0.104 M NaOH and 11.29 mL of 0.125 M HC1 (AH = -55.85 kJ/mol) and a temperature rise of 4.6 °C was recorded. Using the same calorimeter, 7.58 mL of 0.151 M of J(OH)3 was reacted with 9.60 mL of 0.125 M HCl and the temperature changed from 25.9 °C to 23.4 °C. a. What is the heat capacity of the calorimeter? b. Write the balanced chemical equation for the reaction between J(OH); and HCI. c. Identify the limiting reactant in the reaction between J(OH)3 and HCl. d. What is the enthalpy of the reaction of J(OH); and HC1?arrow_forwardA.) Given the standard enthalpy changes for the following two reactions: (1) 2Ni(s) + O2(g)-2NIO(s) AH° = -479.4 kJ (2) Ni(s) - Cl2(g)–→NIC2(s) AH° = -305.3 kJ what is the standard enthalpy change for the reaction: (3) 2NICI,(s) + O2(g)2NIO(s) + 2C2(g) AH° = ? kJ B.) Given the standard enthalpy changes for the following two reactions: (1) 4C(s) - SH2(g) C,H10(e) AH° = -125.ó kJ (2) C,H(g)2C(s) + 2H2(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C,H4(g) + H2(g) ) C,H10(g) AH° = ? kJarrow_forwardA) Given the standard enthalpy changes for the following two reactions:(1) 2C(s) + H2(g)C2H2(g)...... ΔH° = 226.7 kJ(2) 2C(s) + 2H2(g)C2H4(g)......ΔH° = 52.3 kJwhat is the standard enthalpy change for the reaction:(3) C2H2(g) + H2(g)C2H4(g)......ΔH° = ?------- kJ B) Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) 2PbCl2(s) + O2(g)2PbO(s) + 2Cl2(g)......ΔH° = ?------ kJarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning