(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
- Calculate 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_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_forwardWhat is the standard enthalpy of isomerization (kJ/mol) of propanol to isopropanol in the liquid state?arrow_forward
- For 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_forwardFor 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: 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_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_forwardCalculate 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_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_forwardWhen ethyl acetate in dilute aqueous solution is heated in the presence of a small amount of acid, it decomposes to acetic acid and ethanol according to the equation CH;COOC;Hs + H;0 -> CH3COOH + C2HSOH Since the reaction takes place in dilute solution, the quantity of water present is so great that the loss of the small amount which combines with ethyl acetate produces no appreciable change in the total amount. Hence, of the reacting substances, only ethyl acetate suffers a measurable change in concentration. A chemical reaction of this sort, in which the concentration of only one reaction substance changes, is called a first-order reaction. It is a law of physical chemistry that the rate at which a substance is being used up in a first order reaction is proportional to the amount of that substance instantaneously present. If the initial concentration of ethyl acetate is Co, find the expression for its concentration at any time t.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning