CHEMISTRY
2nd Edition
ISBN: 9781593995782
Author: OpenStax
Publisher: XANEDU PUBLISHING
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Chapter 5, Problem 29E
If the 3.21 g of
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When 8.6 grams of a certain compound is dissolved in 78 grams of water in a calorimeter, the temperature of the calorimeter changes from 25.00ºC to 23.09 ºC. Assuming that the specific heat capacity for the resulting solution is 4.184 J/(g oC), and the heat for this solvation is found as x kJ, what is the value of x?
The salt calcium chloride is soluble in water. When 1.14 g of CaCl2 is dissolved in 115.00 g of water, the temperature of the solution increases from 25.00 to 26.82 °C. Based on this observation, calculate the enthalpy of dissolution of CaCl2 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.
) The salt potassium perchlorate is soluble in water. When 2.84 g of KClO4 is dissolved in 106.00 g of water, the temperature of the solution decreases from 25.00 to 22.54 °C. Based on this observation, calculate the enthalpy of dissolution of KClO4 (in kJ/mol).Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.
Chapter 5 Solutions
CHEMISTRY
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- A student used a coffee-cup calorimeter to determine the enthalpy of solution for NH4NO3.When NH4NO3 is added to water, there is a decrease in temperature of the solution. Is the solution process exothermic or endothermic? (a) endothermic (b) exothermicarrow_forwardDissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)arrow_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forward
- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forwardou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.arrow_forward3.66 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.arrow_forward
- When 1.34 g of KClO3 was added to 142.07 g of water in a calorimeter, the temperature dropped by 0.663 °C. The heat capacity of H2O is 4.184 J/g°C. Assume the specific heat of the solution equals that of pure H2O and that the calorimeter neither absorbs nor leaks heat. What is the molar heat of solution of solid potassium chlorate? Give the answer in kJ, but do not include the unitarrow_forwardWhen 6.72 grams of potassium chlorate (KCIO3) are dissolved in 120.0 grams of water at 25.0 °C in an insulated container, the temperature of the water decreases to 20.7 °C. Assuming that the specific heat of the solution is 4.184 J/(g °C) and that no heat is gained or lost by the container, what is the AH of solution of KCIO3 in kJ/mol?arrow_forward3.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.arrow_forward
- A constant pressure calorimeter contains 286 g of water at 20.0 °C. A 13.41 g of substance X (molar mass 154 g/mol) at 20.0°C was dissolved in this water. The temperature of the solution increased to 23.5 °C. Assuming the specific heat of the mixture is 4.184 J g‑1°C‑1, and the density of the solution is 1.00 g/cm3, calculate the enthalpy change (in kJ) for the dissolution of 1 mole of X.arrow_forwardThe enthalpy of solution (∆ H) of NaNO3 is 20.4 kJ/mol. If 2.05 g NaNO, is dissolved in enough water to make a 100.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g•°C and the density of the solution is 1.02g/mL).arrow_forwardWhen 1.31 g of KClO3 was added to 138.34 g of water in a calorimeter, the temperature dropped by 0.506 °C. The heat capacity of H2O is 4.184 J/g°C. Assume the specific heat of the solution equals that of pure H2O and that the calorimeter neither absorbs nor leaks heat. What is the molar heat of solution of solid potassium chlorate? Give the answer in kJ, but do not include the unitarrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY