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Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would have  been the number of Joules released in the reaction? What effect would this have on  the value of X1?

Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would have  been the number of Joules released in the reaction? What effect would this have on  the value of X1?

Chemistry
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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Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would have 
been the number of Joules released in the reaction? What effect would this have on 
the value of X1?

Components Mass (g) Volume (mL) Concentration (M) Initial Temperature (°C) Final Temperature (°C) Calculated Values PART A H₂O (s) 20g 100g 1 www H₂O (1) .… ……. 2.70°C PART B C=0.12 J/°C NaOH (s) 2g 1 .…. H₂O (1) 100g 1 ……w ΔΗ, = 2180.49 J -8°C 20°C 20°C 20°C 20°C 25.21°C PART C NaOH HCI (s) (aq) 2g www www 0.500M 100ml 50ml 31.83°C PART D NaOH HCI (aq) (aq) AH₂ = 4951.09 J -ww www 50ml 1M 1M 26.81°C AH₂ = 2850.12 J
Transcribed Image Text:Components Mass (g) Volume (mL) Concentration (M) Initial Temperature (°C) Final Temperature (°C) Calculated Values PART A H₂O (s) 20g 100g 1 www H₂O (1) .… ……. 2.70°C PART B C=0.12 J/°C NaOH (s) 2g 1 .…. H₂O (1) 100g 1 ……w ΔΗ, = 2180.49 J -8°C 20°C 20°C 20°C 20°C 25.21°C PART C NaOH HCI (s) (aq) 2g www www 0.500M 100ml 50ml 31.83°C PART D NaOH HCI (aq) (aq) AH₂ = 4951.09 J -ww www 50ml 1M 1M 26.81°C AH₂ = 2850.12 J
Heat is a form of energy, sometimes called thermal energy, which can pass spontaneously from an object at high temperature to an object at a lower temperature. If the two objects are in contact, given enough time, they will reach the same temperature. Heat flow is typically measured in a device called calorimeter. A calorimeter is simply a container with insulating walls, made so that essentially no heat is exchanged between the contents and the surroundings. Within the calorimeter, phase changes and reactions may occur, or heat may flow from one part of the contents to another, but no heat transfers into or out of the calorimeter. One type of calorimeter is the constant- pressure calorimeter. Typically, it can be made from styrofoam cup or a more advanced one as shown in Figure 1. These devices are used to measure enthalpy changes in physical or chemical processes. Thermometer Styrofoam Cover Styrofoam Cups Water Stirrer (b) Figure 1. Set-up of constant-pressure calorimeters as (a) styrofoam cups and (b) pre-made type. In this experiment, the heat capacity of a calorimeter and the heat involved in the following reactions will be determined and compared. Reaction 1: Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. NaOH(s) Na (aq) + OH(aq) + X₁J AH₁ = -X₁ J Reaction 2: Solid sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride. NaOH(s) + H(aq) + Cl(aq) H₂O + Na'(aq) + Cl(aq) + X₂J AH₂ = -X₂J
Transcribed Image Text:Heat is a form of energy, sometimes called thermal energy, which can pass spontaneously from an object at high temperature to an object at a lower temperature. If the two objects are in contact, given enough time, they will reach the same temperature. Heat flow is typically measured in a device called calorimeter. A calorimeter is simply a container with insulating walls, made so that essentially no heat is exchanged between the contents and the surroundings. Within the calorimeter, phase changes and reactions may occur, or heat may flow from one part of the contents to another, but no heat transfers into or out of the calorimeter. One type of calorimeter is the constant- pressure calorimeter. Typically, it can be made from styrofoam cup or a more advanced one as shown in Figure 1. These devices are used to measure enthalpy changes in physical or chemical processes. Thermometer Styrofoam Cover Styrofoam Cups Water Stirrer (b) Figure 1. Set-up of constant-pressure calorimeters as (a) styrofoam cups and (b) pre-made type. In this experiment, the heat capacity of a calorimeter and the heat involved in the following reactions will be determined and compared. Reaction 1: Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. NaOH(s) Na (aq) + OH(aq) + X₁J AH₁ = -X₁ J Reaction 2: Solid sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride. NaOH(s) + H(aq) + Cl(aq) H₂O + Na'(aq) + Cl(aq) + X₂J AH₂ = -X₂J
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