Q: Date: Period: Q11: Calculate the AH for the reaction: C2H4 (g) + H2 (g) => C2H6 (g), from the…
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Q: DeltaU°rxn
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Q: Use the data at 25°C given below to calculate the value of AG°rxn for the reaction shown when it…
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Q: For the reaction A + B AB, kassoc = 2.0 sec-1 M-1 and kdissoc = 0.5 sec-1. This means that Kassoc…
A: given reaction, A + B ⇔ AB kassoc = 2.0 sec-1 M-1 kdissoc = 0.5 sec-1
Q: Step 7 of 8 Substitute the value of [Br] from Step 3 and the value of [H] from Step 5 into the…
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Q: What is the autoignition temperature for Acetone?
A: Given, Compound = Acetone What is the autoignition temperature for Acetone = ?
Q: Use the table to calculate AG for the following reactions at 25°C. Species AG (kJ/mol) Mg(s) 02g)…
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Q: What is the value of ΔG°rxn for the reaction: C--->2A+B given: 2A+B--->ΔG°rxn=150.5kJ/mol
A: Given: Reaction-1: 2 A + B --> C ΔG°rxn=150.5kJ/mol Reaction-2: C--> 2 A + B ΔG°rxn=?
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Q: Calculate the Ksp for the dissociation of solid barium nitrate in water at 25.0 oC. The ΔGo for…
A: given - ΔGo for Ba(NO3)2(s) = -797 kJ/mole. temperature T = 25.0 oC. = 25+ 273 = 298 K Ksp = ?
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Q: The A,G° for the following reaction is - 100.4 kJ. C2H4(g) + H2(g) –→ C2H6(g) Given A;G° [C2H4(g)] =…
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Q: What is the value of AGº at |AH®»0 -98.8 kJ•mol- AS rxn rxn 25 °C for the reaction -141.5…
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Q: C6H4(OH)2(aq)+H2O2(aq) -> C6H4O2(aq) +2H2O(I) ^ Hydrooquinone Calculate HRxN for this…
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Q: From the given reaction below, it was determined that the value of dG° = -30kca/mol. Determined the…
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Q: Determine DG0 for the reaction: 2CO(g) + 2H2(g) ---> CO2(g) + CH4(g) DH0 = -247.3 kJ/mol DS0 =…
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- Calculate Ksp for the salt NaCl at 25°C. Substance ΔGf°(in kJ/mol) Na+(aq) –262.0 Cl–(aq) –131.0 NaCl(s) -383.6Calculate the value of DeltaU°rxn at 25°C for the reaction described by H2 ( g ) + 1/2 O ( g ) → H2O ( l ) DeltaHrxn° = – 2 8 5 . 8 k J · m o l – 1 Answer should be 1/2 of -564.2kj/molCalculate DH for the reaction 2N2(g) + 5O2(g) ---> 2N2O5(g), from the following Data.
- Calculate the Ksp for the dissociation of solid barium nitrate in water at 25.0 oC. The ΔGo for Ba(NO3)2(s) = -797 kJ/mole. Ba(NO3)2(s) ↔ Ba+2(aq) + 2NO3-1(aq) Group of answer choices 4.47x10-23 5.06x10-4 1.97x103 5.22x10-40 2.24x1022 0.992What is the value of ΔG°rxn for the reaction: C --> 2A+BGiven: 2A+B --> C and ΔG°rxn = 260.5 kJ/molCalculate the ΔH°f of C6H12O6(s) from the following data: Show the complete and step by step solution ΔH combustion of C6H12O6(s) = -2816kJ/mol ΔH°f of CO2 (g) = -393.5 kJ/mol ΔH°f of H2O (l) = -285.9 kJ/mol Equation: C6H12O6(s) + O2(g) -> CO2(g) + H2O(l)
- can someone find the [OH-] at T hot, the Ksp at T hot, the delta G for T hot, the delta S and delta H and % error given the following values Temp Room: 20.1 deg Cel Temp Hot: 30.7 deg Cel pH Room: 12.78 pH Hot: 12.44 calculate the value given the following standard state entropies S f Ca(OH)2 (aq) = -74.6 J/mol K S f Ca(OH)2 (s)= 83.39 J /mol KC6H4(OH)2(aq)+H2O2(aq) -> C6H4O2(aq) +2H2O(I) ^ Hydrooquinone Calculate HRxN for this reaction froom the following data, Show all calculation. (i) C6H4(OH)2(aq) -> C6H4O2(aq) +H2(g) H=+177.4 kJ (ii) H2(g) + O2(g) -> H2O2(aq) H=-191.2 kJ (iii) H2(g) +1/2 O2(g) -> H2O(g) H= -241.8 kJ (iv) H20(g) -> H2O(I) H=-43.8 kJwhat should i put for the numinator of the Kb equation. Because the value of Kw is not in the options for me tu put in the numinator ?
- When nitric acid is produced industrially, nitrogen monoxide, NO, is first formed at high temperature. Bakefetr reacts NO on cooling further with oxygen to nitrogen dioxide: 2 NO(g) + O2 ⇌ 2 NO2 (g) Table 1: Thermodynamic data at 25°C. Bond ΔfHom Som Cop,m NO(g) 90.25 210.76 29.34 O2(g) 0.00 205.14 29.36 NO2(g) 33.18 240.06 37.20 1) Calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG25o, for reaction (1) at 25°C from the data in Table 1 2) Calculate (with all relevant intermediate calculations) the equilibrium constant K25, for reaction (1) at 25°C. 3) Industrially, however, the reaction does not proceed at 25°C but at 500°C. Therefore, calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG500o, for reaction (1) at 500°C under the assumption that the standard molar heat capacities, Cop, in Table 1 are independent of temperature in the interval [25°C, 500°C]What is the ∆G◦ (in kJ mol−1) for the followingreaction at 25 ◦C?NO2(g) ⇌ N2O4(g)NO2(g):∆H◦ = 33 kJ mol−1; S◦ = 240 J mol−1 K−1N2O4(g):∆H◦ = 11 kJ mol−1; S◦ = 304 J mol−1 K−1A. −41.1 B. −8.8 C. −2.5 D. 16.2E. 5.24 × 104Use the data given in the table to calculate the value of Δ?∘rxn at 25∘ C for the reaction described by the equation A+B↽−−⇀C Compound Δ?∘f (kJ/mol) A +387.7 B –660.6 C +402.0