In a constant-pressure calorimeter, 50.0mL of 0.340MBa(OH)2 was added to 50.0mL of 0.680MHCI. The reaction caused the temperature of the solution to rise from 23.86°C to 28.49°C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ). Q =

In a constant-pressure calorimeter, 50.0mL of 0.340MBa(OH)2 was added to 50.0mL of 0.680MHCI. The reaction caused the temperature of the solution to rise from 23.86°C to 28.49°C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ). Q =

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...

See similar textbooks

Similar questions

When 60.0 mL of a 0.400 M solution of HNO3 (aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 ˚C. The initial temperature of the solutions is 24.0 ˚C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J·g–1·˚C–1, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/oC. (Hint: start with qrxn + qsoln + qcal = 0.) The balanced chemical equation for this reaction is: HNO3 (aq) + NaOH(aq) → H2O(l) + NaNO3 (aq)
Measurements show that the energy of a mixture of gaseous reactants decreases by 206. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -145. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic
Simple Calorimetry. A piece of solid aluminum at 15.0°C is immersed in 12.3 g of nitrogen gas which is initially at 51.1°C and the system is allowed to equilibrate. Given that the specific heat of solid aluminum is 0.908 J/K/g and the specific heat of nitrogen gas is 1.0 J/K/g, what is the mass of the piece of solid aluminum if the final temperature is 34.7°C?
Potassium nitrate, KNO 3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 41.8 g of KNO3 is dissolved in 277 g of water at 23.00 °C. KNO3(s) H₂O K+(aq) + NO3(aq) The temperature of the resulting solution decreases to 20.90 °C. Assume that the resulting solution has the same specific heat as • water, 4.184 J/(g · °C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? Isoln = What is the enthalpy of the reaction? AH rxn = KJ kJ/mol
Suppose 200.0 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH, both initially at 25.0°C, are mixed in a thermos flask. When the reaction is complete, the temperature is 28.4°C. Assuming that the solutions have the same heat capacity as pure water, compute the heat released (in kJ).
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =
THe G.R.A.S.P. method
Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJ
When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)
Use the References to access important values if needed for this question. A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity. When 6.36 g of KBr(s) is dissolved in 115.00 g of water, the temperature of the solution drops from 25.00 to 22.71 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AHdissolution = kJ/mol Submit Answer 5 question attempts remaining
A 44.0 g sample of unknown metal at 99.0°C was placed in a constant-pressure calorimeter containing 80.0 g of water at 24.0°C, the final temperature of the system was found to be 28.4°C. Calculate the specific heat of the metal.