3. A solid chemical called Instant Ice can be purchased, which when mixed with water at room temperature, produces a slushy ice-cold mixture. Which chemical process is involved (endothermic or exothermic)?

Chemistry
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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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**Questions to Answer:**

1. In the calorimeter experiment, you mixed 50 mL of 1.0 M NaOH with 50 mL of approximately 1.0 M HCl. Suppose that 50 mL of a more concentrated solution of each were mixed.
   
   a. Should any additional heat have been released? Explain.
   
   b. Should you have obtained the same ΔT? Explain.
   
   c. Would the true molar enthalpy change, ΔH, for this reaction be different? Explain.

2. What type of reaction would have a positive ΔT value? Explain.

3. A solid chemical called Instant Ice can be purchased, which when mixed with water at room temperature, produces a slushy ice-cold mixture. Which chemical process is involved (endothermic or exothermic)?
Transcribed Image Text:**Questions to Answer:** 1. In the calorimeter experiment, you mixed 50 mL of 1.0 M NaOH with 50 mL of approximately 1.0 M HCl. Suppose that 50 mL of a more concentrated solution of each were mixed. a. Should any additional heat have been released? Explain. b. Should you have obtained the same ΔT? Explain. c. Would the true molar enthalpy change, ΔH, for this reaction be different? Explain. 2. What type of reaction would have a positive ΔT value? Explain. 3. A solid chemical called Instant Ice can be purchased, which when mixed with water at room temperature, produces a slushy ice-cold mixture. Which chemical process is involved (endothermic or exothermic)?
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