The complete combustion of 1.35 g of cinnamaldehyde (C₂H8O, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter = 3.10 kJ/°C) produced an increase in temperature of 13.4 °C. 1st attempt See Periodic Table Calculate the molar enthalpy of combustion of cinnamaldehyde (AHcomb) (in kilojoules per mole of cinnamaldehyde). kJ/mol

The complete combustion of 1.35 g of cinnamaldehyde (C₂H8O, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter = 3.10 kJ/°C) produced an increase in temperature of 13.4 °C. 1st attempt See Periodic Table Calculate the molar enthalpy of combustion of cinnamaldehyde (AHcomb) (in kilojoules per mole of cinnamaldehyde). kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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* formation, using Standard heats of calculate the Standard enthalpy change for the following reaction. 2 H₂O(l) → 2H₂(g) + O₂ (9) 7 ANSWER: IRJ clo C
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Using the standard enthalpies of formation, calculate the standard enthalpy change for the overall reaction that occurs when ammonia is burned in air to form nitrogen dioxide and water. 4NH,(g) +70,,g) 4NO,(g) 6H.O(1) AH of NH₂(g) = -46 kJ/mol AH of NO(g) = 34 kJ/mol, AH of H₂O() = -286 kJ mol f f 5 O-360 kJ -1396 kJ O-1496 kJ O -1496 kJ Question 9 - 1 Not yet answered - Flag question
Review | Constants | Periodic Table MISSED THIS? Watch KCV 9.10. IWE 9.12; Read Section 9.10. You can click on the Review link to access the section in your e Text. Part A Use standard enthalpies of formation from the following table to calculate AH for each reaction. C,H2 (g) + H2(g) → C,H4 (g) Substance AH; (kJ/mol) Express your answer in kilojoules to one decimal place. AlOs(s) -1675.7 BizO3 (s) -573.9 ΑΣΦ ? C2H2 (g) 227.4 CH1(g) 52.4 AHin = kJ C,Hs (g) -84.68 CO(g) -110.5 Submit Request Answer CO2 (1) -413.8 CO2(g) -393,5 Part B Cr203 (s) -1139.7 H2O(g) -241.8 CO(g) + H20(g) - H2 (g) + CO2(g) H20(1) -285.8 HNO3 (aq) Express your answer in kilojoules to one decimal place. -207 NO(g) 91.3 + ΑΣφ. ? NO2(g) 33.2 AHin = kJ Submit Request Answer Part C P Pearson
1. Write the balanced equation for the production of the brown nitrogen dioxide (NO2) gas from nitrogen and oxygen gases. Calculate the enthalpy of the reactions given below. N2 (g) +O2 2NO (g) 2NO (g) AH = 180 kJ ne 2NO(g) +Q2 (g) AH = 112 kJ 2. Methylhydrazine (N2H3CH3) is common liquid propellant used in rocket fuels. Look for the standard molar enthalpies of formation of the reactants and products. Calculate the AH° for the reaction per mole of N2H3CH3. 4N2H3CH3 (1) + 5N2O4 () 12H20 (g) +9N2 (g) +4CO2 (g)
e page 474 Use enthalpies of formation below to calculate the standard enthalpy of reaction for the following methane-generating reaction of methanogenic bacteria. 1st attempt i See Periodic Table O See Hint 4CH,NH, (g) + 2H,0(1) 3CH,(g) + CO2(g) + 4NH, (g) kJ AH, Substance (kJ/mole) CH,NH, (g) -22.97. H,0(1) -285.80 CH (g) -74.80 Co,(g) -393.50 NH, (g) -46.10 ESTIONS COMPLETED
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Using Hess's law find the final enthalpy which is delta H! Show your steps! We know delta H is -283.46kJ/mol for this reaction, however how did we get that!
Homework 3 • Use standard enthalpies of formation from Table 7.2 to determine the enthalpy change at 25 °C for the following reaction. 2 Cl2(g) + 2H20(1) 4 HCI( g) + O2(g) AH° = ?
TUTOR Enthalpy Changes I The reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g) proceeds as follows: 2H,S(g) + 302(g) →2H,0(g) + 2SO2(g) When 11.3 g H,S(g) reacts with sufficient O2(g), 172 kJ is evolved. Calculate the value of A,H for the chemical equation given. kJ/mol Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 6 item attempts remaining