Tutored Practice Pro 5.4.4 COUNTS TOWARDS GRADE Close Problem Use constant-volume calorimetry to determine energy change. A 0.934-g sample of dimethyl oxalate (C,H,O.) is burned in a bomb calorimeter and the temperature increases from 25.40 °C to 27.60 °C. The calorimeter contains 1.15x10 g of water and the bomb has a heat capacity of 943 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of dimethyl oxalate burned (kJ/mol). C,H,O4(s) + 7/2 O2(g) 4 CO2(g) + 3 H20(1) AE = kJ/mol Check & Submit Answer Show Approach

Tutored Practice Pro 5.4.4 COUNTS TOWARDS GRADE Close Problem Use constant-volume calorimetry to determine energy change. A 0.934-g sample of dimethyl oxalate (C,H,O.) is burned in a bomb calorimeter and the temperature increases from 25.40 °C to 27.60 °C. The calorimeter contains 1.15x10 g of water and the bomb has a heat capacity of 943 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of dimethyl oxalate burned (kJ/mol). C,H,O4(s) + 7/2 O2(g) 4 CO2(g) + 3 H20(1) AE = kJ/mol Check & Submit Answer Show Approach

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

True or False: In a coffee cup calorimetry experiment qreaction + qsolution = 0
You would like to determine how many calories are in 10 grams of chicken that is served in the LaGCC cafeteria. Using your understanding of a bomb calorimeter (Figure 5.18 in your textbook) Devise a scheme to find how many calories are in the meat and Assuming the specific heat of chicken is 3.68 J/g⁰C and the change in temperature was 1.90⁰C, how many calories are in 10 grams of chicken? For the following hypothetical reactions: 2A + 3B → C + D ∆H = -46 KJ E + A → C ∆H = 50 KJ A + 0.5D → B ∆H = 23 KJ
Given is the following information for the reaction of magnesium oxide and magnesium with hydrochloric acid in a coffee cup calorimeter. (Atomic masses : Mg = 24.3, O = 16.0 g/mol, respectively) i Weight of Magnesium Oxide used 0.750 g ii mols of Magnesium Oxide used ? iii ∆Tcalorimeter 3.5°C iv qcalorimeter = Ccal x ∆T [Ccal = 418J(g●°C] ? v qreaction ? i Weight of Magnesium metal used 0.725 g ii mols of Magnesium metal used ? iii ∆Tcalorimeter 22.0°C iv qcalorimeter = Ccal x ∆T [Ccal = 418J(g●°C] ? v qreaction ? H2(g) + ½O2(g) → H2O(l) -285.8 kJ Now, calculate the ∆H for the following reactions in kJ /mol. MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) Mg (s) + 2HCl(aq) → MgCl2(aq) + H2 (g) Using all the above information and data, calculate the ∆H for the following reaction: Mg (s) + ½O2(g) → MgO(s) ∆H = ?
True or False: In a coffee cup calorimetry experiment qreaction + qsolution = 0
When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is -26.42 kJig. Multiple Choice 7521 KJPC 4.18 kJ/C 1.34 KJPC 15.87 KJPC 5.52 KJPC
Please don't provide handwriting solution
Ignition wires heat Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. sample Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. %3D Water In the laboratory a student burns a 0.596-g sample of acetylsalicylic acid (C,H3O4) in a bomb calorimeter containing 1090. g of water. The temperature increases from 24.40 °C to 26.80 °C. The heat capacity of water is 4.184 J gl°C 1 The molar heat of combustion is -3869 kJ per mole of acetylsalicylic acid. C,H3O4(s) + 9 O2(g) - →9 CO2(g) + 4 H20(1) + Energy Calculate the heat capacity of the calorimeter. Burning sample Insulated Sample dish Steel outside chamber bomb heat capacity of calorimeter = J/°C Combustion (bomb) calorimeter.
Help please
Need asap
Need help with these calculations
calculating heat of combustion of quinone
How much CO2 is formed from the reaction of 5.0 g of baking soda