For the reaction, Fe203 (s) + 3 H2(g) <> 2 Fe(s) + 3 H20g), AG - 53 k at 25 °C and AH- 100 k). Which of the following is completely true about the relationship between AG and T for this reaction? OA AG 635 K O B. AG>0 when T> 635 K OC. AG 0.6 K O D. AG
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- I need it in 6 min!!! When H2 iscombusted in the presence of excess O2 to form liquid water, what is ∆H° to the nearest kJ? Sign must be correct for full credit. ∆Hf° (H2O(l)) = −286 kJ. 2 H2 (g) + O2 (g) --> 2 H2O(l)At constant pressure and 25°C, what is ΔH° for the following reaction2C2H6(g) + 7O2(g) → 4CO2(g) + H2O(l)if the complete consumption of 38.2 g of C2H6 liberates 1981 kJ of heat energy?a. 3120 kJb. 1560 kJc. 5030 kJd. 2510 kJe. 784.05 kJA coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
- Calculate the Enthalpy of change in Kj/mol and % difference in the neutralization reaction below: HNO2 + NH3 = N2 + 2 H2O Initial Temp= 20 Deg celsius Final Temp= 22.3 Deg celsius Conc= 0.4 M [HNO3] and 0.4 M [NH3] Vol= 55 mL [HNO2] and 60 mL [NH3]= Mass is 115 g Specific Heat= 4.184 J/g For the other value in % difference use: -348 Kj/molA coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹Use standard Gf values from the Thermodynamic Data Table in Resource Section of Atkin's Physical Chemistry to calculate ΔG° (in kJ) for the combustion of propane.C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) Answer in 4 significant figures.
- The formulas give the enthalpy when Coal and Methane react with oxygen:C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJCH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4gives 44 gram of CO2+891kJ 1-Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg.Calculate the lower heating value for Methane. 2-Calculate the amount of CO2 which is produced per kWh for Coal and MethaneAnswer the following the questions given below Given (Dissolution of Sodium Hydroxide) Mass of Water = 200g Initial Temperature of water = 20.0°C Final Temperature of water = 26.49 °C ?water= 5430.832J ?dissolution= 5566.6028J Mass of Solid NaOH= 5.0g Moles of solid NaOH=0.12501 mol Δ?of NaOH dissolution= -44.51 kJ/mol Questions: 1.Is the dissolution of NaOH endothermic or exothermic? Justify your answer. 2.If you touch the sides of a beaker containing NaOH being dissolved, will it feel warm or cold to touch?For the following reaction and data (all data is valid at 298 K):4??2(?) +?2(?) +2?2?(?) ⇌ 4???3(?) ∆??° (??2(?)) = 51.3 ?? ???−1 ∆??° (?2?(?)) = −228.6 ?? ???−1 ∆??° (???3(?)) = −80.7 ?? ???−1 a) What is ΔfG° of O2 (g) ?b) What is ΔrG° ? Express your answer in kJ mol-1. c) If ΔrH° = -346 kJ mol-1, what is ΔrS° in J mol-1 K-1? In a few words, explain why your answer intuitively does (or does not) make sense.
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