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- An important flavor component of vanilla extract is vanillin (C8H8O3, molar mass = 152.15 g/mol). When vanillin burns in a bomb calorimeter with a heat capacity of 7.87 kJ/°C, the temperature increases from 25.52°C to 30.43°C. If the heat of combustion of vanillin is -3,760 kJ/mol, what mass of vanillin (in g) was combusted? Please give your answer to 2 decimal places.When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is CuSO4·5 H2O(s) --> CuSO4(s) + 5 H2O(g) *heat above the arrow If 5.32 g CuSO4·5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid.Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
- The enthalpy of combustion of isooctane (C8H18(l)) is -5461 kJ/mol. From data found in appendix G, calculate the enthalpy of formation of C8H18(l): C8H18(l) + 12.5 O2(g) → 8 CO2(g) + 9 H2O(l) ∆Hrxn = -5461 kJ ∆Hf = ___ kJ/mol Correct answer is not 259.2Chlorine trifluoride, CIF3, is a toxic, intensely reactive gas. It was used in Word War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, Chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride reacts, 1196 kJ of heat is evolved. What is the standard enthalpy of formation of chlorine trifluoride?The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.09g of glucose is burned in a calorimeter containing 826 g of water, and the temperature of the assembly increases from 20.10oC to 24.70oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol. (Final answer: TWO decimal places)
- Acetylene burns in air according to the following equation:C₂H₂(g)+5/2O₂(g)→2CO₂(g)+H₂O(g) ΔH°ᵣₓₙ =-125.8kJ Given ΔH°f of CO₂(g) 393.5 kJ/mol and ΔH°f of H₂O(g) =241.8 kJ/mol, find ΔH°f of C₂H₂(g)10. Which of the following constants is/are needed to calculate the amount of energy required to heat 30.5g of H2O(s) at –25.0°C to H2O(l) at 55.0°C? I. ΔHfus (H2O)II. ΔHvap (H2O)III. specific heat of H2O(s)IV. specific heat of H2O(l)V. specific heat of H2O(g) A. I only B. I, II, III, IV, and IV C. I, III, and IV D. I, II, III, and IV E. III and IVA bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6421 g sample of 2-naphthylacetic acid (C12H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.267×103 g of water. During the combustion the temperature increases from 27.50 to 30.60 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 843.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data. C12H10O2(s) + (27/2) O2(g) 5 H2O(l) + 12 CO2(g) + EnergyMolar Heat of Combustion = kJ/mol
- A certain coal has the following ultimate analysis C=70%, N2=4%, H2=2.5%, O2=3.5%, S2=7%, Ash=5%, Moisture=2% Determine the heating value of fuel in Btu/lb. ANSWER: 11,735.351Click the button within the activity, and analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, ΔHΔH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. Reaction 1: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g),C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), ΔH1=−2043 kJΔH1=−2043 kJ Reaction 2: 5C3H8(g)+25O2(g)→15CO2(g)+20H2O(g),5C3H8(g)+25O2(g)→15CO2(g)+20H2O(g), ΔH2=?ΔH2=? Express your answer to four significant figures and include the appropriate units. View Available Hint(s)Ethyl chloride (C2H5Cl) can be used as a topical anesthetic, for example prior to giving a painful injection. When liquid ethyl chloride is sprayed on the skin, energy absorbed from the skin causes the liquid to evaporate. This numbs the injection site by quickly decreasing the skin temperature to near 0oC. How much heat (in kJ) is required to evaporate 2.81 mL of ethyl chloride at 25oC? For C2H5Cl: d = 0.924 g/mL and ΔHovap = 24.6 kJ/mol at 25°C.