The standard heat of reaction for the production of formaldehyde in the reaction, 2 CH;OH (1) + 02 (g) →2 HCHO (g) + 2 H20 (1), is -326.2 kJ/mol. a. Is the reaction exothermic or endothermic? Would you heat or cool the reactor to keep the temperature constant? b. Explain physically why heat is released or absorbed when a reaction occurs. c. If the temperature and pressure are keep at standard (25°C, 1 atm), what is the rate of heating/cooling required in kcal/hr if 1000 kg/hr of formaldehyde is formed?

The standard heat of reaction for the production of formaldehyde in the reaction, 2 CH;OH (1) + 02 (g) →2 HCHO (g) + 2 H20 (1), is -326.2 kJ/mol. a. Is the reaction exothermic or endothermic? Would you heat or cool the reactor to keep the temperature constant? b. Explain physically why heat is released or absorbed when a reaction occurs. c. If the temperature and pressure are keep at standard (25°C, 1 atm), what is the rate of heating/cooling required in kcal/hr if 1000 kg/hr of formaldehyde is formed?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 134IP: Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is...

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Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly CH3NO2(l) + O2(g) CO2(g) + N2(g) + H2O(g) a. The standard enthalpy change of reaction (Hvan ) for the balanced reaction (with lowest whole-number coefficients) is 1288.5 kJ. Calculate Hf0 for nitromethane. b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (nitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?
Nagyung wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O, qrxn, ΔHrxn ? Is the reaction endothermic or exothermic?
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O? What is qrxn? What is ΔHrxn? Is the reaction endothermic or exothermic?
Formaldehyde Can Be Made By The Oxidation Of Methanol (CH3OH). If Stoichiometric Amounts Of CH3OH(G) And O2 (G) Enter The Reactor At 100 C, The Reaction Is Complete, And The Products Leave The Reactor At 200 °C, Calculate The Heat That Is Added Or Removed From The Reactor Per Mole Of Methanol Fed To The Reactor. The Reaction Is: This problem has been solved! See the answer Formaldehyde can be made by the oxidation of methanol (CH3OH). If stoichiometric amounts of CH3OH(g) and O2 (g) enter the reactor at 100 C, the reaction is complete, and the products leave the reactor at 200 °C, calculate the heat that is added or removed from the reactor per mole of methanol fed to the reactor. The reaction is:
The reaction SO2(g)+2H2S(g)⇌3S(s)+2H2O(g)SO2(g)+2H2S(g)⇌3S(s)+2H2O(g) is the basis of a suggested method for removal of SO2SO2, a pollutant that irritates airways causing coughing, from power-plant stack gases. The values below may be helpful when answering questions about the process. Substance ΔG∘fΔGf∘(kJ/mol)(kJ/mol) ΔH∘fΔHf∘(kJ/mol)(kJ/mol) H2O(g)H2O(g) −−228.6 −−241.8 H2O(l)H2O(l) −−237.1 −−285.8 SO2(g)SO2(g) −−300.4 −−296.9 SO3(g)SO3(g) −−370.4 −−395.2 H2S(g)H2S(g) −−33.01 −−20.17 S(s)S(s) 0 0 Assume that the partial pressure of sulfur dioxide, PSO2PSO2, is equal to the partial pressure of dihydrogen sulfide, PH2SPH2S, and therefore PSO2=PH2SPSO2=PH2S. If the vapor pressure of water is 24 torrtorr , calculate the equilibrium partial pressure of SO2SO2 (PSO2PSO2) in the system at 298 KK. Express the pressure in atmospheres to two significant figures. Kp= 8*10^15
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. 1. What is qH2O in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 2. What is qdissolution in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 3. What is the ΔHdissolution in kilojoules per mole? A. +44.866 B. -44.866 C. +1.794 D. -1.794 4. Is the reaction endothermic or exothermic? A. Endothermic B. Exothermic
Consider the ideal combustion of ethanol: C2H5OH(ℓ) + 3 O2(g) → 2 CO2(g) + 3 H2O(ℓ) ∆Ho = -1367.5 molar masses (g/mol): C2H5OH - 46.07 CO2 - 44.01 Indicate the 3 statements about the ideal combustion of ethanol that are true by checking the box in front of each true statement. The reaction is endothermic. The reaction is exothermic. There is more chemical energy stored in the products than in the reactants. When 50.0 g of ethanol combusts, 47.8 g of carbon dioxide are formed. When 50.0 g of ethanol combusts, 1480 kJ are released. When 1030 kJ are released, 40.7 g of water are formed.
suppose that the gas-phase reaction 2no(g)+o2(g) ? 2no2(g) were carried out in a constant-volume container at constant temperature. would the measured heat change represent ?h or ?e? if there is a difference, which quantity is larger for this reaction? Bartleby
The efficiency of striated muscle is typically 37%, that is, the muscle converts 37% of the chemical energy reaching it (in the form of glucose) into mechanical work, converts the remainder into waste heat. Your biceps muscle performs mechanical work at the rate of 50 W. (a) What is the rate at which it consumes chemical energy? (b) What is the rate at which it produces waste heat? (c) Given that the oxidation of glucose yields 3.70 103 kcal/kg, what is the rate at which this muscle consumes glucose?
Which expression describes the heat emitted in a chemical reaction when the reaction is carried out at constant pressure?Explain.a. ∆E - wb. ∆Ec. ∆E - q
At 32°C, liquid Glauber's salt – sodium surface decahydrate, Na2SO4 x 10H2O(I) – solidifies amd releases 78.0 KJ/mol of energy. Calculate the enthalpy change when 2.50kg of Glauber's salt enters the solid state.
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O? What is qrxn? What is ΔHrxn?