Ethene (C₂H₂), at 25 °C and 1 atm, is burned with 300% excess air at 25 °C and 1 atm. Assume that this reaction takes place adiabatically at 25 °C and that the products leave at 25 °C and 1 atm. Use the PG mixture model. Assume cp to be uniform at 1.005 kJ/kg.K.
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- For the following gaseous reaction at 25 °C: H2(g) + 10 O2(g) = H₂O(g) + excess O2(g) (unbalanced). Calculate the maximum temperature (in °C) in an adiabatic explosion of the mixture with reactants initially at 25 °C inside a sealed bomb, given that the heat of formation of H₂O(g) = -58 kcal mol-¹, Cp.H2 = Cp,02 = 6.5 cal K-1 mol-¹, and Cp.H20 = 7.5 cal K-¹ mol-¹.The following reaction is carried out under standard conditions (25°C and 1 bar): 2CH3OH(1) + 302(g) → 2CO2(g) + 4H₂O(1) AH₁° kJ mol-1 Sᵒ J K-¹ mol-1 C6H12O6 (1) -238.4 212.0 O₂ (g) 0.0 205.1 CO₂(g) -393.5 213.7 H₂O (1) -285.8 69.95 Using the data in the table above: a) Calculate the enthalpy of reaction, ArH, for the reaction: kJ mol-¹ b) Calculate the entropy change, AS, for the reaction: 1 c) Calculate AG for the reaction: kJ mol-¹ d) Is the reaction spontaneous? Put any calculations in here: J mol-1Please use the values in the resources listed below instead of the textbook values. Consider the synthesis of urea according to the equation CO2(g) + 2 NH3(g) – (NH2)2CO(s) + H20(/) From the data listed in the supporting materials, calculate the value of A-G° for the reaction at 298 K. 4.0 -6.7 kJ•mol-1 Assuming ideal gas behavior, calculate the value of A,G for the reaction at a pressure of 12.7 bar. The Af G° of urea is -197.3 kJ-mol-1. 4.0 kJ•mol-1 Supporting Materials E Periodic Table Constants and I Supplemental Data Factors Submit Answer
- Find the standard molar enthalpy for the reaction C(s) + ½ O2(2) → CO(g) Cs) + O2(2) → CO2«g) CO243) Given that AH° = -394 kJ and COg) + ½ O2(g) AH°=+283 kJ O a. -111 kJ b. +110 kJ c. -125 kJ d. +120 kJ36. The standard enthalpy (AH) for the reaction of C2H4 with Cl2 C2H4 + Cl2 → C2H3CI + HCI + 110 kJ was determined from the following reactions. Reaction AH at 298 K Cl2 + H2 2 HCI -185 kJ C2H4 + HCI-→ C2H5CI -65 kJ C2H3CI + H2 → C2H;CI Complete the table above by calculating the value of the AH (kJ per mole of CH;Cl produced) of the last reaction.A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
- A 33.0 g iron rod, initially at 22.2 °C, is submerged into an unknown mass of water at 63.9 °C, in an insulated container. The final temperature of the mixture upon reaching thermal Part A equilibrium is 58.6 °C. You may want to reference (Pages 373 - 379) Section 9.4 while completing this problem. What is the mass of the water? Express your answer to two significant figures and include the appropriate units. μΑ Value Units т %3 Request Answer SubmitThe following reaction has these standard thermodynamie parameters: An-30.6 kmol and AS 55.3 J(mol K).ellus_engine.html?ClassID=1087757335# Calculate the standard reaction enthalpy for the reaction between NO and O3. NO(g) + O3(g) NO2(g) + O2(g) Compound AH°; (kJ/mol) NO(g) 90. AHxn = [ ? ] kJ %3D 0,(8) NO,(g) 143 34 Enter either a + or - sign and the magnitude. Enter
- Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 59.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. alo AH = -172. kJ J AS = -420. K CH, OH (g) + CO(3) - HCH,CO, (1) AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither AH =…Calculating dG from dH and ds A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 65.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. 圖 Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. dlo AH = 33. kJ J AS = 78. K 2Fe(s) + 3H,0(1) - Fe,0, (s) + 3H, (g) AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither AH…Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 122.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. P4 (g) + 6C₁₂ (g) → 4PC13(g) AH = - - 1207. kJ AS = -3055. AG = I kJ J K Which is spontaneous? this reaction the reverse reaction neither AH = 1353.…