Photosynthesis in plants converts carbon dioxide and water into glucose and oxygen. Calculate the ∆H°, ∆S° and ∆G°. Supply all the missing values '?'. Is the reaction spontaneous at standard conditions? CO2 (g) + H2O (l) → C6H12O6 (s) + O2 (g) molar ratio of the balanced chemical equation: ? Substance / S° (J/mol • K) CO2 (g) / 213.68 H2O (l) / 69.91 C6H12O6 (s) / 209.2 O2 (g) / 205.03 ∑S° (product) = ? ∑S° (reactant) = ? ∆S° rxn = ? Substance / H° (kJ/mol) CO2 (g) / -393.51 H2O (l) / -285.83 C6H12O6 (s) / -1273.3 O2 (g) / 0 ∑H° (product) = ? ∑H° (reactant) = ? ∆H° rxn = ? in KJ T in Kelvin = ? ∆S (surr) = ? ∆S (universe) = ? ∆G = ? Spontaneity (S for spontaneous and NS for non-spontaneous): ?

Q: Calculate ΔrS° for the reaction 4Cr(s) + 3O2(g) → 2Cr2O3(s) Substance:     Cr(s)    O2(g)…

A: Answer :- ∆S° =-548.1 (J/mol.K)  The standard entropy change (ΔrS°) for the given reaction is =…

Q: Below what temperature does the following reaction become spontaneous? FeO(s) + CO(g) → CO2(g) +…

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Q: Consider the following reaction for the production of hydrogen cyanide.  NH3 (g)  +   S(s) +   CH4…

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Q: A possible reaction for converting methanol to ethanol is; CO(g)  +  2H2(g) +   CH3OH(g)…

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Q: Calculate ΔS°(universe) for the combustion of acetylene at 298.15 K using the reaction below.…

A: Given: ΔS°(system) = –194.6 J/K and ΔH°(system) = –2511.2 kJ ΔS°(universe)Combustion of acetylene at…

Q: Given the following thermodynamic data calculate ∆S and ∆Ssurr for the following reaction at 25°C…

A: Formula used: ∆S=∆product-∆reactant

Q: For the reaction2CO(g) + 2NO(g)2CO2(g) + N2(g)ΔH° = -746.6 kJ and ΔS° = -198.0 J/KThe maximum amount…

A: The given balanced equation can be expressed as: Calculate the standard free energy by using the…

Q: FeO

A: ∆H°rxn = [ ∆H°f(Fe2O3) ] - [ ∆H°f(FeO) + ∆H°f(Fe) + ∆H°f(O2) ]  ∆H°rxn = [ -822.16 kJmol-1 ] - […

Q: Is the following reaction spontaneous at room temperature (25.0 °C) ? 2 H2S(g) + 3 O2(g) 2 SO2(g) +…

A: Interpretation: The given reaction is spontaneous at room temperature or not is to be determined. At…

Q: Use data from Appendix IIB to calculate ΔS∘rxnΔSrxn∘ for each of the reactions given.…

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Q: Consider the following reaction and its associated ΔHrxn. CH3OH=CO+2H2,   ΔHrxn = 90.70 kJ/mol…

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Q: Using the thermodynamic data provided below, determine the temperature in °K at which the…

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Q: 1: Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → →…

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Q: An example of a reaction where ∆G = 0 is   C(graphite)→C(diamond)   any synthesis reaction…

A: We know, The value of  ∆G = 0 when the reaction is at an equilibrium.

Q: spontaneous

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Q: For the reaction C6H6 (l) + 3 H2 (g)  -->  C6H12 (l)        ΔHo = –206.7 kJ/mol What statement is…

A: We know that   ΔGo =  ΔHo - T ΔSo and for a reaction to be spontaneous  ΔGo should be negative.

Q: What is the lowest temperature at which the reaction of C(s) with H2O(g) to produce H2(g) and CO(g)?…

A: The lowest temperature would be 981..3153°C.

Q: Consider the following reaction at constant P. Use the information here to determine the value of…

A: From thermodynamics: ∆Ssurr=∆HT                                                              . . .…

Q: A possible reaction for converting methanol to ethanol is; CO(g)  +  2H2(g) +   CH3OH(g)        -><-…

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Q: . Use Appendix G (Links to an external site.). to calculate ΔS°rxn for the following reaction.…

A: This question can be solves using Hess's law of constant heat summation.

Q: Suppose a reaction has ∆H = -28 kJ and ∆S = -60J/K. What is the cross-over temperature? Is it…

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Q: For a particular reaction, Δ?∘=67.7 kJ/mol and Δ?∘=126.9 J/(mol⋅K). Assuming these values change…

A: Given : ΔHo of reaction = 67.7 KJ/mol = 67700 J/mol…

Q: From the values of ΔH and ΔS, predict which of the following reactions would be spontaneous at 25°C:…

A: The spontaneous nature of the reaction is determined by calculating the change of free energy of the…

Q: Which reaction(s) will be spontaneous at all temperatures? : 4NH3(g) + O2(g) → 2N2(g) + 6H2O(g) ΔrH…

A: For a chemical reaction to be spontaneous, Gibbs free energy, ∆rG should be negative. ∆rG is…

Q: Determine the sign of ΔSsys for the following chemical reactions without doing any calculations.  d)…

A: The objective of the question is to determine the sign of the change in entropy (ΔSsys) for the…

Q: The figure represents the spontaneous deposition of iodine in which iodine vapor, I2(g), becomes…

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Q: From the values of ΔH and ΔS calculate the minimum temperature at which each reaction will become…

A: ∆H = -389 kJ/mole = -389000 J/mole∆S = 27.8 J/K.mol

Q: Calculate ΔSsurr at 25°C for the following reaction at constant pressure. Will the reaction be…

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Q: Calculate ∆G for the reaction 2 H2S(g) + SO2(g) ⇆3 Srhombic(s) + 2 H2O(g) For the following…

A: ∆Gof H2S(g)=-34kJ/mol ∆G of SO2(g)=-300kJ/mol ∆G of H2O(g) = -229kj/mole ∆G of S(rhombic)= 0 kj/mole…

Q: Consider the reaction below for the decomposition of carbon tetrachloride gas:  CCl4(g)    ------>…

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Q: 3. Determine the temperature (°C) range, in which the following reaction will become spontaneous.…

A: In thermodynamics. the relation between Gibbs free energy, enthalpy, and entropy can be given as:…