3 P Question 41 Consider these reactions: Reaction 1: H2 (g) + Cl2 (9) 2HCI(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 1. Determine the mass, in grams, of chlorine gas consumed (with excess H2) when 1,721.0 kJ of energy is released from the system. Answer: g (mass must be positive; round to nearest whole number)

3 P Question 41 Consider these reactions: Reaction 1: H2 (g) + Cl2 (9) 2HCI(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 1. Determine the mass, in grams, of chlorine gas consumed (with excess H2) when 1,721.0 kJ of energy is released from the system. Answer: g (mass must be positive; round to nearest whole number)

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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Calculate AH for the reaction. Enter your answer in the provided box. CH3OH + HCI →→→ CH₂Cl + H₂O kJ/mol
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H, (g) AH = -931.0 kJ HCI(g) → HCI(aq) AH2 = -74.8 kJ H,(g) + Cl,(g) → 2 HCI(g) AH3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) AH, = -118.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) 2. 3.
Question 40 Consider these reactions: Reaction 1: H2 g) + Cl2 (g) → 2HC1(g) AH= -184.6 kJ Reaction 2: 20F2(g) + 02 (g) + 2 F2 (g) 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 56.0 g of oxygen difluoride decomposes? Answer: - kJ (enter a positive value)
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HC1(aq) → 2 MCl,(aq) + 3 H,(g) ΔΗ = -589.0 kJ 2. HCI(g) → HCI(aq) AH2 = -74.8 kJ 3. H,(g) + Cl,(g) –→ 2 HCI(g) AH3 = -1845.0 kJ 4. MCI,(s) → MCl,(aq) AH4 = -262.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCl,(s) ΔΗ- kJ
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When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
#3
Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCl(9) AH = -184.6 kJ Reaction 2: 20F2(g) → O2(g) +2F2(g) AH=-49.4 kJ Reaction 3: Na (g) +202 (9) 2NO2(g) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,409.0 kJ of energy is released from the system. Round to the nearest whole number .
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)
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H, (g) ΔΗ = -847.0 kJ 2. HCI(g) → HCl(aq) AH2 = -74.8 kJ H,(g) + Cl,(g) → 2 HCl(g) 3. AH3 = -1845.0 kJ 4. MCI,(s) –→ MCI, (aq) AH4 = -424.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g)→ 2 MCI, (s) ΔΗ-