Consider the following reactions:(1) N2(g) + O2(g) → 2NO(g)AH = +180.7 kJ(2) 2NO(g)+ O2(g) 2NO2(g)AH = -113.1 kJ= =113.1 kJ(3) 2NO2(g) → 2N2(g) + O2(g)AHr = -163.2 kJuse Hess's law to calculate AH for the reactionNO2(g) + NO2(g) 3NO(g)

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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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Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.
18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)
Calculate the value of AH for the following reaction: 2 NO₂ (g) N₂O4 (g) → based on the formation reactions for each of the reaction components as shown below: N2 (g) + O2(g) →→→ NO₂ (g) AH = 33.2 kJ/mol N₂ (g) + 2O2 (g) →→→ N₂O4 (g) AH₂ = 11.1 kJ/mol AH: kJ/mol
Fe O3(s) + 3CO(g) → 2Fe(s) + 3CO;g); AH® = -26.8 kJ %3D FeO(s) + CO(g) -Fe(s) + CO2(g); AH° = -16.5 kJ determine AH for the following thermochemical equation. Fe O(s)+ CO(g) 2FEO(s) + CO;(g) 6.2 kJ O 22.7 kJ O 10.3 kJ 2433KJ 2-103KJ
Consider these reactions: Reaction 1: H2 (9)+ Cl2 (g) → 2HC1(g) AH = -184.6 kJ %3D Reaction 2: 20F2 (g) → 02 (g) + 2 F2 (g) AH = -49.4 kJ Reaction 3: N2 (9) + 202 (9) - → 2NO2 (9) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H2) when 1,529.0 kJ of energy is released from the system. Answer: g (mass must be positive; round to nearest whole number)
How much energy in kJ is released in burning 1.63 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol) The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ) ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8 Round your answer to 2 decimal places.
Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5
Can you please help me with this question
Given the data below, H°, for the reaction rxn 3C12 (g) + PH3 (g) → PCI3 (g) + 3HCI (g) is kJ. AH° (PCI3 (g) = -288.07 kJ/mol AH°F (HCI (g)) = -92.30 kJ/mol AH°r (PH3 (g)) = 5.40 kJ/mol 570.37 O The AH°, of Cl2 (g) is needed for the calculation. -385.77 385.77 -570.37
Consider these reactions: Reaction 1: H2 (g) + Cl2 (g) → 2HC1(g) AH = -184.6 kJ Reaction 2: 20F2 (9) → 02 (9) + 2 F2 (9) AH= -49.4 kJ Reaction 3: N2 (g) + 202(g) → 2NO2(g) AH=+66.4 kJ Use Reaction 2. How much energy (in kJ) is released when 61.0 g of oxygen difluoride decomposes? Answer: - kJ (enter a positive value)
Given the following combustion reaction and its molar enthalpy of reaction: 2NO(g) + O2(g) 2NO2(g) AH° = -112 kJ What is the heat (q) associated with the combustion of 2.00 mole of NO(g)? O -112 kJ O -224 kJ +56.0 kJ -56.0 kJ O +112 kJ

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Consider the following reactions: (1) N2(g) + O2(g) → 2NO(g) AH = +180.7 kJ (2) 2NO(g)+ O2(g) 2NO2(g) AH = -113.1 kJ = =113.1 kJ (3) 2NO2(g) → 2N2(g) + O2(g) AHr = -163.2 kJ use Hess's law to calculate AH for the reaction NO2(g) + NO2(g) 3NO(g)