When 1.0 g of sodium nitrate was dissolved in 50.0 g of water in a calorimeter at 20.0°C, the temperature of the solution decreased to 14.5°C. Assume the mass of the solution is equal to the mass of water and that c p solution - 4.18 J(g °C), as per Equation (6). Is this process endothermic or exothermic? Explain: a. b. Calculate quhetion Calculate AH d. Calculate moles of NaNO, jou Find AH for the solution of 1 mole of NaNO, in water. e. J/mol uos

When 1.0 g of sodium nitrate was dissolved in 50.0 g of water in a calorimeter at 20.0°C, the temperature of the solution decreased to 14.5°C. Assume the mass of the solution is equal to the mass of water and that c p solution - 4.18 J(g °C), as per Equation (6). Is this process endothermic or exothermic? Explain: a. b. Calculate quhetion Calculate AH d. Calculate moles of NaNO, jou Find AH for the solution of 1 mole of NaNO, in water. e. J/mol uos

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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0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 8.41 °C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･ °C and the density of the solution is 1.02 g/mL).
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
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A student followed the procedure in this experiment , using 29.5 mL of 2.41 molar HCl and 31.5 mL of 2.41 molar NaOH , with both solutions having an initial temperature of 21.9 °C. After mixing , a maximum temperature of 31.0 °C is measured . The final mass of the mixture was found to be 62.201 grams . For this problem , assume the specific heat of the solution is 4.18 J/g °C. What is the heat transferred by this reaction, in Joules?
3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, 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.
If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal). In this reaction, we combine 5.85 g of 63.7 ºC water with 6.63 g of 18.9 ºC water in a calorimeter. Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 28.8ºC. Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water. Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC. The first law of thermodynamics tells us that all of these changes sum up to zero so Enter your answer to one decimal place (tenths)
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