A chemist measures the enthalpy change AH during the following reaction: 2 H,O(1) + O2(9)→2 H,O,(1) AH=196. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 4H,0, (1) - 4H, 0(1) + 20, (g) 2H,0,(1) → 2H,0(1) + 0, (g) O kJ H,0() + 0,(2) – H,0,(1) • H,0,(1) O kJ

A chemist measures the enthalpy change AH during the following reaction: 2 H,O(1) + O2(9)→2 H,O,(1) AH=196. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 4H,0, (1) - 4H, 0(1) + 20, (g) 2H,0,(1) → 2H,0(1) + 0, (g) O kJ H,0() + 0,(2) – H,0,(1) • H,0,(1) O kJ

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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A chemist measures the enthalpy change AH during the following reaction: P4(s) + 6 Cl₂(g) →4 PC1₂(g) AH-1148. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction PC₁₂ (9) → 4PCL, (g) P₁(s) + 2C₁₂ (9) P₁ (s) + 6Cl₂ (g) P₁ (s) + C₁₂(g) → PCI, (g) ΔΗ [] kJ KJ kJ x10 X
A chemist measures the enthalpy change AH during the following reaction: C,H,0,(s)-3 CH,(o) + 3CO,(g) AH=-132. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH 9CH, (0) + 9Co, (a) - 30H,0,0) 3CH, (6) + 300, (a) - C,H,0,0) GH,0,) - CH, 6) + co,()
A 1.71 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.09oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place).
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4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
The combustion of 1.880 g of sucrose, C,H,,O, (s), in a bomb calorimeter with a heat capacity of 4.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.31 °C to 29.52 °C. What is the internal energy change, AU, for the combustion of 1.880 g of sucrose? AU = kJ Calculate the enthalpy of combustion, AHe, of sucrose in kilojoules per mole. kJ/mol AH. = A étv w MacBook Air DI DD 80 888 F12 F11 F9 F10 F7 FB 3 F4 F5 F6
Calculate the ΔH°rxn of the reaction in a bomb calorimeter: NaOH(s) → NaOH(aq) Given the following: Volume of solution = 100mL (when solid added to water) Concentration = 1M Mass of NaOH = 1.0359g Change in temperature = 2.5°C Specific heat capacity of solution = 4.184 J/°C Specific heat capacity of bomb calorimeter = 30 J/°C Molecular mass of NaOH = 40g/mol
Determine the reaction enthalpy, ΔHrxn for the reaction, N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g) ΔHrxn = ??? kJ by using some combination of the reactions below. 1) 2NH3(g) → N2H4(l) + H2(g) ΔH1 = 20 kJ 2) 2NH3(g) → N2(g) + 3H 2(g) ΔH2 = 60 kJ 3) CH2O(g) + H2(g) → CH 4O(l) ΔH3 = 80 kJ. .
10. Bacteria sour wines and beers by converting ethanol, C₂H5OH, into acetic acid, CH₂COOH. Assume that the reaction is C₂H5OH(1) + O₂(g) → CH₂COOH() + H₂O(1) The standard molar enthalpies of combustion of ethanol and acetic acid to produce liquid water are, respectively, - 1367 kJ/mol and -875 kJ/mol. Write chemical equations for the combustions, and use Hess' law to determine the standard enthalpy change for the conversion of ethanol to acetic acid.
A chemist measures the enthalpy change AH during the following reaction: 2 HNO3(1) + Mg(s)→Mg(NO3),(s) + H,(9) AH=-443. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH x10 10HNO,() + SMg(s) - 5Mg(NO,),(-) + 5H,(3) kJ 4 Mg(NO,),() + 4H, (8) → 8HNO,(1) + 4Mg(s) kJ Mg(NO,),(s) + H,(s) 2HNO,(1) + Mg(s) - 443. kJ