When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.50 mL of 3.00 M HCl, both initially at room temperature (22.00 \deg C), the temperature increased to 30.00 \deg C. The resultant salt solution had a mass of 28.50 g and a specfic heat capacity of 3.74 J K-' g-'. What is the heat capacity of the calorimeter (in J/°C) ? Note: The molar enthalpy of neutralization per mole of HCI is -55.84 kJ mol-'.

When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.50 mL of 3.00 M HCl, both initially at room temperature (22.00 \deg C), the temperature increased to 30.00 \deg C. The resultant salt solution had a mass of 28.50 g and a specfic heat capacity of 3.74 J K-' g-'. What is the heat capacity of the calorimeter (in J/°C) ? Note: The molar enthalpy of neutralization per mole of HCI is -55.84 kJ mol-'.

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

0.015L of 3mol/L NaOH mixes in a calorimeter with 0.013L of 3mol/L HCl, the two initially at 295K, the temperature increases to 302.1K. The salt solution formed weighs 0.018kg and has a specific heat capacity of 3.74J/K g. What is the heat capacity of the calorimeter (in J/K)?
A 0.500 mole sample of CO(g) is combusted in a constant pressure calorimeter to CO2(g). The temperature is observed to rise from 25.00°C to 27.50°C. The heat capacity of the calorimeter (calorimeter constant) is 56.6 kJ/K. What isA H in kJ/(mole of CO) for the reaction? (A - 282 кУmol B +282 kJ/mol С) +283 кy/mol D -283 kJ/mol
Understanding the definition of enthalpy ARLYC 0/5 Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 383. kU during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -180. kJ of work is done on the mixture during the reaction. Calculate the change in energy 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 II
For the following combustion reaction of benzoic acid (HC7H5O2; molar mass = 122.1 g/mol) HC7H5O2(s) + 15/2 O2(g) --> 7CO2(g) + 3H2O(l); DHcomb = -3226 kJ 1.00 g of benzoic acid is combusted in a bomb calorimeter, which contains 1.00 kg of water (specific heat = 4.184 J/g.oC) and the bomb has a heat capacity of 890 J/oC. If the initial temperature of the calorimeter is 25.0oC, what is the final temperature of the calorimeter when the combustion is completed? (A) 51.8oC (B) 31.3oC (C) 30.2oC (D) 27.0oC
In one experiment, a student placed 50.0 mL of 1.00 M HCl in a coffee-cup calorimeter and carefully measured its temperature to be 25.5oC. To this was added 50.0 mL of 1.00 M NaOH solution whose temperature was also 25.5oC. The mixture was quickly stirred, and the student noticed that the temperature of the mixture rose to 32.4oC. What was the heat of reaction?
The combustion of 0.4683 g naphthalene (C10H8(s); MM = 128.16 g/mol) in a constant volume bomb calorimeter caused a temperature rise in the water bath of 1.707 degrees. The final temperature was 298.00 K. The heat capacity of the calorimeter was 10.3610 kJ/K. Calculate the value of ΔHcomb in units of kJ/mol.
When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee cup calorimeter. The temperture rises from 21.6 degree celcius to 37.8 degree celcius. Caluclate the delta H (in kJ/mol NaOH) Assume that the specific heat solution is the same of that as pure water NaOH(s)---> Na+(aq)+ OH-(aq)
The heat capacity of an Object (F) is the amount of heat (Q) required to raise it’s temperature, per degree (delta T). F=Q/delta T. Will the specific heat capacity be extensive or intensive? c=F/m (m is molar mass)
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? 9.156 kJ Incorrect What is the enthalpy of the reaction? AHrxn 16.35 kJ/mol %D Incorrect
Show the complete solution
A generic solid, X, has a molar mass of 61.8 g/mol. In a constant-pressure calorimeter, 18.6 g of X is dissolved in 369 g of water at 23.00°C. X(s) X(aq) The temperature of the resulting solution rises to 24.30 °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? 2.01 kJ Incorrect What is the enthalpy of the reaction? AHTan= 6.67 kJ/mol Incorrect
When 1.77 g of glucose (C6H1206, molar mass = 180.156 g/mol) is burned in excess oxygen in a bomb calorimeter, the temperature rises from 20.82°C to 28.41°C. What is the heat capacity of the bomb calorimeter in units of kJ °C-1? A,Uº for the combustion of glucose is -2805 kJ per mole of glucose.