The following data are results for an experiment, where the energy released by the complete combustion of propanol was used to heat 200.00 g of water, as shown below: 137 25 g Initial mass burner + propanol Final mass burner + propanol 135.60 g Initial temperature of water 20 °C Final temperature of water 75 °C Specific heat, Cp, of water 4.184 J/g C Molar Mass of propanol, (CsH OH) 60 g/mole a) What is the experimental value of AH for propanol based on the above results? b) If the theoretical AH for propanol is 2021 kJ/mol, what is the percentage error of the results?

The following data are results for an experiment, where the energy released by the complete combustion of propanol was used to heat 200.00 g of water, as shown below: 137 25 g Initial mass burner + propanol Final mass burner + propanol 135.60 g Initial temperature of water 20 °C Final temperature of water 75 °C Specific heat, Cp, of water 4.184 J/g C Molar Mass of propanol, (CsH OH) 60 g/mole a) What is the experimental value of AH for propanol based on the above results? b) If the theoretical AH for propanol is 2021 kJ/mol, what is the percentage error of the results?

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

In your Heat of Neutralization experiment, you will mix 25.0 mL of 1.0 M NAOH(ag) with 25.0 mL of 1.0 M HCI(ag) in a coffee-cup calorimeter; assume that you found the heat capacity of your calorimeter to be 25 J/°C. A graph of your data is shown below. What is the Heat of Neutralization in k] per mole? Neutralizaion Reaction of HCI(aq) and NaOH(aq) 30 8 26 AT 26 25 24 22 20 40 60 80 100 Time, s О а. -15 O b.-85 O C.-65 O d.-26 Temperature, oc
A 138.9 g sample of an unknown metal at a temperature of 99.1 °C is added to 44.72 g of water at a temperature of 19.1 °C. The specific heat of water is 4.184 Jg-1 °C- 1. The final temperature of the system is 52.2°C. Calculate the specific heat of the unknown metal.
A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś
The temperature of the solution increases from 21.3 °C to 38.2 °C. 0.468 g Mg reacting0.0193 mol Mg reacting80.844 g HCl solution The energy released is given by q = specific heat × mass × temperature changeThe solution is almost all water, so we use the specific heat capacity of water, 4.18 J/g•°C. What is the quantity of heat released? Enter your answer as a positive value.
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
A piece of molybdenum metal whose mass is 6.87 g is heated to 100.0 °C and then dropped into an ice calorimeter. As the molybdenum cools to 0.0°C, 0.513 g of ice melts (it takes 6.01 kJ of heat to melt exactly 1 mol of ice). What is the molar heat capacity (in J/mol·K) of molybdenum? i J/mol*K
[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]
When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ
A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?