The standard reaction enthalpy of Zn(s) + H2O(g) → ZnO(s) + H2(g) is approximately constant at +224 kJ mol−1 from 920 K up to 1280 K. The standard reaction Gibbs energy is +33 kJ mol−1 at 1280 K. Estimate the temperature at which the equilibrium constant becomes greater than 1.
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- The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.The standard reaction enthalpy of Zn(s) + H2O(g) → ZnO(s) + H2(g) is approximately constant at +224 kJ mol-1 from 920 K up to 1280 K. The standard reaction Gibbs energy is +33 kJ mol-1 at 1280 K. Assuming that both quantities remain constant, estimate the temperature at which the equilibrium constant becomes greater than 1.The reaction A(g) + B(g) ↔ C(g) + D(g) has ΔGrxn° = -28.62 kJ mol-1 and Kp = 0.63 at 980 °C. A rigid cylinder at that temperature contains 1.2 atm of A, 0.20 atm of B, 0.30 atm of C, and 0.27 atm of D. What is the reaction Gibbs energy?
- The dissociation vapor pressure of a salt A2B(s) ⇌ A2(g) + B(g) at 367°C is 208 kPa but at 477°C it has risen to 547 kPa. For the dissociation reaction of A2B(s), calculate (i) the equilibrium constant, (ii) the standard reaction Gibbs energy, (iii) the standard enthalpy, and (iv) the standard entropy of dissociation, all at 422°C. Assume that the vapor behaves as a perfect gas and that ΔrH° and ΔrS° are independent of temperature in the range given.Borneol is a pungent compound obtained from the campharwood tree of Borneo and Sumatra. The standard reaction Gibbs energy of the isomerization of borneol to isobarneal in the gas phase at 503 K is +9.4 kJ mol-1. Calculate the reaction Gibbs energy in a mixture consisting of 0.15 mol of borneol and 0.30 mol of isoborneol when the total pressure is 600 Torr.The equilibrium pressure of hydrogen H2 over solid uranium U and solid uranium hydride UH3 at 500 K is 139 Pa. Calculate the standard Gibbs energy of formation of UH3 (s) in the reaction: U(s) + 3/2 H2 (g) → UH3 (s) at 500 K. Hint: start with writing the equilibrium constant K expressed through activities that include pressure of gas. Examples are in class notes. Then, convert K to the standard Gibbs energy of the pertinent reaction.
- The standard reaction Gibbs energy of the isomerization of cis-2-pentene to trans-2-pentene at 400 K is -3.67 kJ mol-1. Calculate the equilibrium constant of the isomerization.a)For the reaction given in Part A, how much heat is absorbed when 3.10 molmol of AA reacts? Express your answer numerically in kilojoules. b)For the reaction in Part A, ΔrS∘=25.0 J K−1 mol−1ΔrS∘=25.0 J K−1 mol−1. What is the standard Gibbs energy of reaction at 281 KK , ΔrG∘ (281K)ΔrG∘ (281K)? Express your answer numerically in kJ mol−1kJ mol−1.The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 i) Calculate the standard Gibbs energy of formation for A and B. ii) Calculate the Gibbs energy change for the reaction A - B at standard conditions. iii) Calculate the enthalpy change for the reaction A - B at 350 K if the average heat capacity C0p = 42 J.K-1.mol-1.
- The standard reaction Gibbs energy for the reactionH2(g) + (1)/(2)O2(g) → H2O(I) is -237.13 kJ mol-1 at 25 °c. Determine the equilibrium constant in terms of concentration, Kc, at this temperature.State the limits to the generality of the expression for estimating the pH of an amphiprotic salt solution. Suggest reasons for why these limitations exist.Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte.found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs:CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac)and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.