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...

See similar textbooks

Similar questions

Pls help ASAP
The heat capacity of a bomb calorimeter is equal to 7.18 kJ/°C and is used for the combustion of 14.85 g of C2H4. What is the heat of combustion on a molar basis (kJ/mol) when the temperature goes from 19.32°C to 27.01°C? (write the result without decimals) Answer:
QUESTION 5 What is the standard enthalpy of formation of liquid methanol, CH3OH()? C(graphite) + O2(g) - CO2(g) AH°TXN = -393.5 kJ/mol H2(g) + ½O2- H20(1) AH°rxn = -285.8 kJ/mol CH3OH() + 3/202(9) → CO2(g) + 2H20() AHrxn = -726.4 kJ/mol O -238.7 kJ/mol O -1691.5 kJ/mol O -47.1 kJ/mol O 47.1 kJ/mol O 1691.5 kJ/mol QUESTION 6 Benzene is a starting material in the synthesis of nylon fibers and polystyrene (styrofoam). Its specific heat capacity is 1.74 J/g.°C. If 16.7 kJ of energy is absorbed by a 225-g sample of benzene at 20.0°C, what is its final temperature? О 37.7°С О 80.1°C O 42.7°C О 62.7°С О -22.7°С
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)
Question 7 of 8 Submit What is the change in enthalpy in kilojoules when 3.24 g of CH:OH gas is completely reacted according to the following reaction? CH.OH(g) – CH:(g) + O2(g) AH = 252.8 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 4.00 x 10-4 0.001 2 25.6 0.101 16.05 32.05 12.8 252.8 6.022 x 1023 3.24 1 1000 32.00 7.80 x 10-4 mol CH4 g O2 mol CH:OH g CH. kJ mol O2 J g CH:OH
Please refer to image...
mation [References] INTERACTIVE EXAMPLE Using Enthalpies of Formation Nitroglycerin is a powerful explosive that forms four different gases when detonated: 2 C3H;(NO3)3(t) → 3 N2(g) + ½ O2(g) + 6 CO,(g) + 5 H20(g) -> Calculate the enthalpy change that occurs when 18.0 g of nitroglycerin is detonated. The standard enthalpies of formation are shown below. AHF (kJ/mol) C3H5(NO3)3(t) -364 CO2(g) -393.5 H,O(g) -241.8 kJ Submit Show Approach Show Tutor Steps
A container filled with 3.29 kg of water underwent a temperature change from 23.89 °C to 28.28 °C. How much heat, measured in kilojoules, did the water absorb? (The specific heat of water is 4.18-J.g1,ºC-1). kJ e Textbook and Media Hint Save for Later Attempts: 0 of 2 used Submit Answer. "pe'here to search a 成中 o 4+ ha insert prt 144 & 24 4 @ %23 8. E bac 3 Q W E T Y U F G H KL A S pause X. C V B|| N M alt ctri alt R
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 nitrogen monoxide(g) with oxygen(g) to form nitrogen dioxide(g) proceeds as follows: 2NO(g) + O2(g) 2NO2(g) When 9.57 g NO(g) reacts with sufficient 02(g), 18.2 kJ is evolved. Calculate the value of A,H for the chemical equation given. kJ/mol