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- Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of SO2 must be evaporated to remove as much heat as evaporation of 1.00 kg of CC12F2 (enthalpy of vaporization is 17.4 kJ/mol)? The vaporization reactions for SO2 and are SO2(l)SO2(g) and CCl2F(l)CCl2F2(g), respectively.A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOHin a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCLand NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change inenthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densitiesand specific heat of the solutions are the same as for water (1.00 g/mL and4.184 J/g.0C, respectively).NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)A. Write the chemical equation of -Luminous flame: -Non-luminous flame: B. Between the two types of flame, which is hotter and why? Explain P.s will upvote if informative, tyyy!!
- 2. What is the heat capacity of ethene and carbon dioxide. In details explain the answer (drawings is requires).A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.(II) A 1.0-L volume of air initially at 3.5 atm of (gauge)pressure is allowed to expand isothermally until the pressureis 1.0 atm. It is then compressed at constant pressure to itsinitial volume, and lastly is brought back to its originalpressure by heating at constant volume. Draw the processon a PV diagram, including numbers and labels for the axes
- 19. Solid urea, (NH2)2CO, burns to give CO2, N2, and liquid H2O. Its heat of combustion is -632.2 kJ/mol. 1.Write the balanced combustion equation. Record fractions as ratios (e.g. 1/2) if needed. Include aggregation states in your answer. 2.Calculate the heat generated per mole of H2O formed to 0.1 kJ. 3.Using this heat of combustion and the appropriate thermodynamic data, determine the heat of formation of urea to 0.1 kJ.At constant pressure and 25C, what is enthalpy for the reaction: 2C2H6 + 7O2 -> 4CO2 + H2O, if the complete consumption of 12g of C2H6 liberates - 700kJ of heat energy? (-3508 kJ)The heat of combustion of liquid octane (C8H18) to carbon dioxide and liquid water at 298 K is -1303 kJ/mol. Find ΔE for this reaction.
- The compound is Methyl Acetate. Referencing applicable thermodynamic data, calculate the ΔH° of combustion, ΔS° of combustion, ΔG°, of the compound assigned to you. Please include references for any data you've sourced (e.g., pages from the CRC Handbook, website, publications, etc.). ΔH° of combustion = ΔS° of combustion = ΔG° = Is this reaction spontaneous? Is this reaction endo- or exo- thermic? Does the entropy increase or decrease?The specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?Calculate the heat of reaction, for 2 mol of NaCl(s) with the stoichiometric amounts of SO2 , O2 and water at an atmosphere, assuming 100% yield and that all reagents and all products are at 400°C .Cp (Na2SO4(s)) = 0.26 cal/mol°C NaCl(s) + SO2(g) + O2(g) + H2O(g) → Na2SO4(s) + HCl(g)