If a chemist started with only 15.21 grams of K2Cr2O7 solid and an unlimited amount of H2O2(aq) then what is the equilibrium constant (K) under standard conditions at 25°C? O2(9) + Cr* (a0) → H2O2(aq) + Cr20,2 (aq) 2.82 x 107 3.63 x 1011 4.03 x 1013 3.81 x 10-8 4.21 x 106 2.66 x 1014 3.27 x 10-9 3.49 x 1010 2.40 x 1014 12
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- Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction. Fe2O3(s)+ 3H2(g)→ 2Fe(s)+ 3H2O(l) Round your answer to 2 significant digits. delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/molFor the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: ΔrH∘ΔrH∘ 182.6kJ mol−1 ΔrS∘ΔrS∘ 24.80J K−1 mol−1 T= 7363 K. Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C∘C:? N2(g)+O2(g)→2NO(g) Express your answer numerically to three significant figures.The reaction below has an equilibrium constant of K=2.2×106K=2.2×106 at 298 KK. 2COF2(g)⇌CO2(g)+CF4(g)
- Reaction KspKsp ΔH°ΔH° ΔS°ΔS° FeCO3(s)⇄Fe2+(aq)+CO32−(aq)FeCO3(s)⇄Fe2+(aq)+CO32−(aq) 3×10−113×10−11 <0<0 >0>0 MnCO3(s)⇄Mn2+(aq)+CO32−(aq)MnCO3(s)⇄Mn2+(aq)+CO32−(aq) 2×10−112×10−11 <0<0 >0 The table above lists the equilibrium constants and changes in thermodynamic properties for the dissolution of FeCO3 and MnCO3 at 25°C. The two-particle diagrams below represent saturated solutions of each compound at equilibrium. (see attached image) a.) The particle diagrams best represent that ΔH°<0ΔH°<0 because the ions from both compounds are solvated by water molecules. b.) The particle diagrams best represent that ΔH°<0ΔH°<0 because both compounds produce about the same amount of CO32−CO32− ions from the dissolution. c.) The particle diagrams best represent that ΔS°>0ΔS°>0 because both compounds produce a very small amount of ions from the dissolution. d.) The particle diagrams best represent that the molar solubility is greater for…The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)Calculate the equilibrium constant k for the following reaction at 75 degree C A2 + B2 > 2AB Given Delta H(kJ/mol) DeltaS(J/mol K) A2 0 119 B2 0 125 AB 0 292 Write your answer in exponential form
- Calculate the standard free-energy change and theequilibrium constant Kp for the following reaction at 25°C. CO(g) + 3H2(g) <----> CH4(g) + H2O(g)1. What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous?1.1 Using the given in 1, what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean?2. If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system?Write down the thermodynamic equilibrium constant expressions of the following reactions. If possible, associate them with Kc and Kp.(a) Si (k) + 2 Cl₂ (g) ↔ SiCl ₄ (g)(b) Cl₂ (g) + H₂O (s) ↔ HOCl (aq) + H⁺ (aq) + Cl- (aq)
- The equilibrium constant Kc for the following system is 24.4. H2(g) + X2(g) ⇌ 2HX(g) A 3.00 L reactor was charged with 0.150 moles of H2, 0.150 moles of X2, and 0.600 moles of HX. A catalyst was introduced using a remote unit, and the system was allowed to come to equilibrium. Which statement below describes the situation? A) The reaction goes to the right, Qc > Kc B) The reaction goes to the left, Qc < Kc C) The reaction goes to the right, Qc < Kc D) The reaction goes to the left, Qc > Kc E) The direction of the reaction depends on the pressure of the system7.6(a) The equilibrium constant of the reaction 2 C3H6(g) 5 C2H4(g) + C4H8(g) is found to fit the expression ln K = A + B/T + C/T2 between 300 K and 600 K, with A = −1.04, B = −1088 K, and C = 1.51 × 105 K2 . Calculate the standard reaction enthalpy and standard reaction entropy at 400 K.Use data found in the Resource section to decide which of the following reactions have K < 1 at 298 K: (i) Hg(l) + Cl2(g) ⇋ HgCl2(s),(ii) Zn(s) + Cu2+(aq) ⇋ Zn2+(aq) + Cu(s)