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- 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.thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do FIsooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C3H13 (2) + 25 02 (g) → 16 CO2(g) + 18 H2O(£) A,H° = -10,922 kJ/mol-rxn What is the enthalpy change if you burn 7.50 L of isooctane (d = 0.69 g/mL)? Enthalpy change |kJ =
- At 25 °C and 765.6 torr, a sample that is a gaseous compound containing carbon, hydrogen, and oxygen occupies a volume of 0.582 L. A mass of 1.103 g of this sample was burned in a bomb calorimeter, producing 1.294 g of liquid water and 2.108 g of gaseous carbon dioxide. The heat produced from the combustion raised the temperate of the calorimeter from 25 °C to 31.94 °C. a.) What is the percent elemental composition by mass of the unknown sample. b.) Determine the empirical formula of the sample.Iron oxides can be smelted in a blast furnace by reacting with CO(g), which serves as the reducing agent. To supply the needed reducing agent, Cs) is added to the blast furnace and is converted to CO(a) through a sequence of two reactions: Reaction I: C(s) + O2g) → CO29) Reaction II: C(e) + CO2(9) →2 Co(g) The standard enthalpies of formation at 298 K for CO2(g) and COg) are -394 kJ/mol and -111 kJ/mol, respectively. (b) Which of the following statements is TRUE? Reactions I and II are both an exothermic process. Reaction I is exothermic, whereas Reaction Il is endothermic. O The overall reaction is spontaneous only at high temperatures. O The overall reaction has an increasing slope when plotted in an Ellingham diagram. Cyclohexane freezes at 6.50 °C. What is its AS of freezing if its AH° of fusion is 2.68 kJ/mol? O +9.59 J/mol-K O -412 J/mol-K O -9.59 J/mol-K O +412 J/mol-K What percentage of the radioactive iodine-131 will be left after 25 days if its decomposition follows 1st order…The synthesis of Hansa yellow dye takes place in a series of two steps. On Sunday June 9th, 1996 a violent runaway reaction occurred causing very significant damage to equipment and buildings. After a detailed analysis, the plant was rebuilt, and production resumed. What is the enthalpy of the overall reaction? Show work for credit. Can you explain which of the two steps was most likely to blame for the incident? Step 1: CsH;CIN2O2(aq) + NANO2(aq) + 2HCI(aq) → C6H3CIN3O2*(aq) + Cl(aq) + 2H2O(I) + NaCI(aq) AH1 = -1212 kJ/mol Step 2: C6H3CIN3O2*(aq) + Cl'(aq) + C10H10CINO2(aq) → C16H12C12N4O4(aq) + HCl(aq) AH2 = 637 kJ/mol %3| Overall Reaction: C6H5CIN2O2(aq) + NaNO2(aq) + HCI(aq) → 2H2O(1) + NaCI(aq) + C16H12CI2N4O4(aq) AHrxn = ? kJ/mol %3D
- NazCr207 H2, Ni 100 atm 150 °Cus_engine.html?ClassID=1834324617# When a 4.25 g sample of solid NH4NO3 dissolves in 60.0 g of water in a coffee cup calorimeter, the temperature drops from 22.0°C to 16.9°C. What is the heat of reaction, qrxn? NH4NO3 ->>> NH+ + NO3 Csoln = 4.18 J/g °C arxn = [?] J Enter either a + or - sign AND the magnitude. Do not round until the end. q,soln (J) EnterApps MyUSU Outlook Canvas Labflow OneNote 101 Chem101 Tophat U USU Tutoring Question 9 of 19 What quantity of heat (in kJ) is absorbed in the process of making 0.957 mol of CF from the following reaction? C (s) + 2 F, (g) → CF, (g) AH° = 141.3 kJ/mol 4. %3D