The standard enthalpy change for the isomerization of cis-1.2-dichloroethene to trans-1.2-dichloroethene is 0.4 kJ-mol The thermodynamic equilibrium constant at 25, "Cis 0.893. Part A Determine the equilibrium constant at 996 "C Express your answer to three significant figures K = Submit ΑΣΦ Previous Answers Request Answer
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- Calculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Gibbs free energychange of Go= − 423 kcal/mole of GlucoseCalculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Entropy change of Go= − 423 kcal/mole of GlucoseEstimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.
- A student determines the value of the equilibrium constant to be 1.5297 x 107 for the following reaction: HBr(g) + 1/2 Cl2(g) --> HCl(g) +1/2 Br2(g) Based on this value of Keq, calculate the Gibbs free energy change for the reaction of 2.37 moles of HBr(g) at standard conditions at 298 K.What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?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 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.
- Estimate the temperature at which the equilibrium constant for the decomposition of CaCO3(s, calcite) to CO2(g) and CaO(s) becomes 1; assume pCO2 = 1 bar .1. The equilibrium constant of the reaction 2 C3H5 (g) = C2H4 (g) + C4H8 (g) is found to fit the expression ln K = - 1.04 - (1088 / T) + (1.51 x 105 / T^2 ) between 300 K and 600 K. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K. [2.77 kJ mol-1 ; -16.5 kJ K-1 mol-1 ]Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. The equilibrium expression for the process is: Na2B4O5(OH)4 10H2O (s) ⇌ 2 Na+ (aq) + B4O5(OH)4 2- (aq) + 10H2O(l) Since liquid water and solid borax are not included in the Ksp expression, the solubility product expression associated with this reaction is: Ksp = [Na+]2[borate] The concentration of the borate ion in equilibrium with solid borax can be determined by titration with HCl based on the following equation: B4O5(OH)42- + 2HCl(aq) + 3H2O (l) → 4 H3BO3(aq)+2Cl-(aq) The Ksp for borax will be evaluated at room temperature at 5oC. Knowing the Ksp values at two temperatures allows the use of the following equations to calculate the change in enthalpy and Gibbs free energy: In(Ksp1/Ksp2)=ΔH/R((1/T2)-(1/T1)) ΔGo= - RT InKsp Once ΔHo and ΔGo are known, you can find…
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