Date: Name(s): 4. HCl is a corrosive colourless gas that dissolves readily in water. Aqueous HCL reacts with NaOH to form water and NaCl. In a simple calorimeter, a 100.00 mL sample of 0.355 mol/L HCl(aq) is mixed with 50.00 mL of excess NaOH(aq). During the reaction, there is a rise in temperature by 4.200 °C. Calculate the molar enthalpy change for the above reaction. SHOW ALL YOUR WORK. mr.sciencen ~ 4 of 6~ (answer + units) SCH4U Date: Name(s): 3. Examine the reaction mechanism found below: A+ B₂ → AB₂ (slow) AB + C→ ABC (fast) AB₂C+C B₂C₂ + A (fast) B₂CD+E (fast) Overall equation: a. Draw a circle around any reaction intermediates. b. Draw a box around any species that can be considered a catalyst. c. In the box above, provide the overall equation for this process. d. In the box below, provide the rate law based on this mechanism. Rate law: mr.sciencen ~ 3 of 6~ SCH4U

Date: Name(s): 4. HCl is a corrosive colourless gas that dissolves readily in water. Aqueous HCL reacts with NaOH to form water and NaCl. In a simple calorimeter, a 100.00 mL sample of 0.355 mol/L HCl(aq) is mixed with 50.00 mL of excess NaOH(aq). During the reaction, there is a rise in temperature by 4.200 °C. Calculate the molar enthalpy change for the above reaction. SHOW ALL YOUR WORK. mr.sciencen ~ 4 of 6~ (answer + units) SCH4U Date: Name(s): 3. Examine the reaction mechanism found below: A+ B₂ → AB₂ (slow) AB + C→ ABC (fast) AB₂C+C B₂C₂ + A (fast) B₂CD+E (fast) Overall equation: a. Draw a circle around any reaction intermediates. b. Draw a box around any species that can be considered a catalyst. c. In the box above, provide the overall equation for this process. d. In the box below, provide the rate law based on this mechanism. Rate law: mr.sciencen ~ 3 of 6~ SCH4U

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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26. Calculate the enthalpy change for the reaction below. NO(g) + O(g) →→→ NO₂(g) Given following data: NO(g) + O₂(g) →→ NO₂(g) + O₂(g) 03(g) → 1.50₂(g) 0₂(g) →20(g) AH-198.9 kJ AH = -142.3 kJ ΔΗ = 495.0 kJ
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCl, (aq) + 3 H, (g) AH1 = -582.0 kJ 2. HCl(g) → HCl(aq) AH2 = -74.8 kJ 3. H, (g) + Cl, (g) → 2 HCI(g) AH3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) AH4 = -434.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) ΔΗ- kJ
A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. Was the dissolution process endothermic or exothermic?
A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What quantity in moles of the unknown salt were used in the reaction?
A chemist dissolved an 14.2-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 30.5 ∘C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g⋅°C. ?= kJ Calculate the heat of solution for KOH in kJ/mol.
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
You have 8.99 g sample of an unknown salt (MM = 116.82 g/mol). It is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the Mass inside calorimeter (g)? Change in Temp inside calorimeter (C)? How much Heat gained (J)? Total Heat? How many mols of the unknown salt? What is the change in empalthy?
8. Instant cold packs can be made from ammonium nitrate by mixing/reacting it with water (reaction shown below). When 1.25 g of NH4NO3 is dissolved in 25.0 g of water at 25.8 °C, the temperature of the water after the reaction is 21.9 °C. What is the enthalpy change (ΔH) for this reaction in units of kJ/mol of NH4NO3? The heat capacity of water is 4.18 ?/ ?℃ . NH4NO3(s) → NH4+(aq) + ??3 − (aq)
For the reaction: 2 CH3OH) +3 02(g) (1) → 2 CO2 + 4 H20u) + 4 H200 + 347 kcal Calculate the amount of heat in kcal & kJ released when 25.4 g of CH,OH reacts.
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-