In a Hess's Law problem, reaction A (with enthalpy AH_A) is multiplied by 2. Reaction B (with enthalpy AH_B) is reversed. Reaction A and reaction B are then added together. What mathematical operation is performed on the enthalpies? 2 ΔΗ Α+ (-ΔΗ Β ) 2ΔΗ Α+ ΔΗΒ ΔΗ Α' ΔHB O AH A+ (-AH_B)

In a Hess's Law problem, reaction A (with enthalpy AH_A) is multiplied by 2. Reaction B (with enthalpy AH_B) is reversed. Reaction A and reaction B are then added together. What mathematical operation is performed on the enthalpies? 2 ΔΗ Α+ (-ΔΗ Β ) 2ΔΗ Α+ ΔΗΒ ΔΗ Α' ΔHB O AH A+ (-AH_B)

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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Constructing Hess's cycles Given the enthalpy changes AHị and AH2 below, construct a Hess's cycle that will enable you to find the enthalpy change for the reaction: 1 MGCO3(s) MgO(s) + CO2(g) AHRI AH1 MgCO3(s) + 2HCI(aq) → MgCl2(aq) + CO2(g) + H20(1) MgO(s) + 2HCI(aq) → H,O(1) + MgCl,(aq) AH2 Given the enthalpy changes AH3 and AH4 below, construct a Hess's cycle that will enable you to find the enthalpy change for the reaction: MgCl2(s) + 6H2O(1) → MgCl2.6H2O(s) AHR2 AH3 MgCl2(s) + aq → MgCl2(aq) MgCl2.6H20(s) + aq → MgCl2(aq) ΔΗ Given the enthalpy changes AHs and AH, below, construct a Hess's cycle that will enable you to find the enthalpy change for the reaction: 2NaHCO;(s) → Na,CO3(s) + CO2(g) + H,O(1) ΔΗR3 HCI(aq) + NaHCO;(s) → NaCl(aq) + CO2(g) + H2O(1) 2HCI(aq) + Na,CO;(s) → 2NaCl(aq) + CO2(g) + H2O(1) ΔΗ AH6 4 Think of a reaction for which the enthalpy change of reaction would be difficult to determine. Write the equations for the reactions that could be used to find the…
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© Macmillan Learning For a particular isomer of Cg H₁8, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁8 (g) consumed, under standard conditions. Cg H18 (g) + 25/ 0₂(g) → 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = esc 1 TOOLS X10" 2 # 3 с $ 4 AHxn=-5108.7 kJ/mol G Search or type URL L 5 MacBook Pro % < 6 & kJ/mol 8
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In a Hess’s Law problem, reaction A (with enthalpy ΔH_A) is multiplied by 2. Reaction B (with enthalpy ΔH_B) is reversed. Reaction A and reaction B are then added together. What mathematical operation is performed on the enthalpies?
This question has multiple parts. Work all the parts to get the most points. Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly CH;NO2 (1) + O2 (9) → CO2(9) + N2(9)+H2O(g) a The standard enthalpy change of reaction (AH) for the balanced reaction (with lowest whole-number coefficients) is –1288.5 kJ. Calculate AH; for nitromethane. rxn CO2 (9) H2O(g) ΔΗ ΔΗ = -393.5 kJ/mol :-242 kJ/mol = ΔΗ kJ/mol bA 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 920. torr. If the mole fraction of nitrogen (Xnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced? Mass = g
1.Given reactions A - C, determine the the change in enthalpy (kJ) for the reaction between C(s) + H2(g). Do not type units into your answer. C(graphite) + 2 H2(g) ⟶⟶ CH4(g) Δ?=?ΔH=? A. C(graphite) + O2(g) ⟶⟶ CO2(g) Δ?=−393.51??ΔH=−393.51kJB. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJC. CO2(g) + 2 H2O(l) ⟶⟶ CH4(g) + 2 O2(g) Δ?=890.30??ΔH=890.30kJ 2. Based on your answer to the previous problem, determine the value of q (kJ) if 5.08 grams of methane (CH4) gas is produced from graphite and hydrogen gas. Do not type units into your answer.
C2H5OH(l)+3O2(g)=2CO2(g)+3H2O(l) The reaction enthalpy for standard conditions. I got the answer of -1,367 is this correct?
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Use Hess’s law to obtain the enthalpy change for this reaction: H2(g) + 1/8 S8(rhombic) -> H2S(g) from the following enthalpies:H2S(g) + 3/2 O2(g) à H2O(g) + SO2(g) ΔH = -518 KJH2(g) + ½ O2(g) à H2O(g) ΔH = -242 KJ1/8 S8(rhombic) + O2(g) à SO2(g) ΔH = -297 KJ
Given the following equations (1-3) and AHO values, determine the heat of reaction at 298 K for the reaction: C(s) + 2 H₂(g) → CH₂(g) 1) C(s) + O₂(g) → CO₂(g) AH° = -380 kJ 2) H₂(g) + 1/2 O₂(g) 3) CO₂(g) + 2 H₂O(1) kJ H₂O(1) AH° = -280 kJ CH₂(g) + 2 O₂(g) AH° = 880 kJ
What is the % error if the theoretical value of the enthalpy of a reaction is 97 kJ and the experimental value is 36 kJ?