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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When 5.325 g KCL dissolves in 100.0ml of water the temperature decreases from 24.1 c to 21.2 c. Calculate the change in enthalpy per mole of KCL. Determine if the process is endothermic or exothermic.
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl 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, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.
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 is the total mass inside the calorimeter in grams?
When 130. mL of 0.198 M NaCl(aq) and 130. mL of 0.198 M AgNO3(aq), both at 21.8°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 24.2°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.60 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction. This is the complete question, nothing was left out. Thank you
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?
Dry ice is solid carbon dioxide. Instead of melting, solid carbondioxide sublimes according to the equation:CO2(s) ------------>CO2(g) When dry ice is added to warm water, heat from the water causesthe dry ice to sublime more quickly. The evaporating carbon dioxide produces a dense fog often used to create special effects. In a simple dry ice fog machine, dry ice is added to warm water in a Styrofoam cooler. The dryice produces fog until it evaporates away, or until the water gets too cold to sublime the dry ice quickly enough. A small Styrofoam cooler holds15.0 L of water heated to 85°C. Use standard enthalpies of formation to calculate the change in enthalpy for dry ice sublimation, and calculate themass of dry ice that should be added to the water so that the dry ice completely sublimes away when the water reaches 25 °C. Assume no heat loss to the surroundings. (The ∆H°f for CO2(s) is -427.4 kJ/mol.)
Constants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 515 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.1 C to 241 °C. Part A Find A H for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g. C as the specific heat capacity.) να ΑΣφ AH,xn - kJ/mol Submit Previous Answers Request Answer * Incorrect; Try Again; 25 attempts remaining Next > Provide Feedback P 8:36
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.
In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.
25. Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?