**Text Transcription for Educational Website****Problem Description:**The heat of combustion of ethanol, C₂H₅OH(l), is -1367 kJ/mol. A batch of sauvignon blanc wine contains 12.1% ethanol by mass.You may want to reference (Pages 191 - 192) Section 5.8 while completing this problem.**Part A:**Assuming the density of the wine to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a 6-oz glass of wine (177 mL)?Express your answer using two significant figures.**[Submission Section]**- Answer Input Field- Submit Button- Request Answer ButtonAdditional options: Return to Assignment, Provide Feedback.**Explanation:**The problem involves calculating the caloric content based on the percentage of ethanol present in the wine and its density. No graphs or diagrams are present in this content.

Given: Heat of combustion of ethanol = -1367 kJ/mol Percent of ethanol by mass = 12.1% Density…

The heat of combustion of ethanol, C,H,OH(I), is-1367 k.J/mol. A batch of sauvignon blanc wine contains 12.1 % ethanol by mass. • Part A You may want to reference (Pages 191-192) Section 5.8 while completing this problem Assuming the density of the wine to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a 6-oa glass of wine (177 mL)? Express your answer using two significant figures. να ΑΣΦ ? Cal Submit Request Answer < Return to Assignment Provide Feedback

The heat of combustion of ethanol, C,H,OH(I), is-1367 k.J/mol. A batch of sauvignon blanc wine contains 12.1 % ethanol by mass. • Part A You may want to reference (Pages 191-192) Section 5.8 while completing this problem Assuming the density of the wine to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a 6-oa glass of wine (177 mL)? Express your answer using two significant figures. να ΑΣΦ ? Cal Submit Request Answer < Return to Assignment Provide Feedback

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

of 1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg2+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.
The specific heat of water is 4.18 J/g-K. AHsolution = -67.91 thermometer When a 7.99-g sample of gaseous hydrogen bromide dissolves in 32.4 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 20.00 °C to 69.54 °C. Calculate AH in kJ/mol HBr for the solution process. HBr(g) → H*(aq) + Br (aq) XkJ/mol HBr. stirrer coffee cups containing reaction mixture
Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 47.3 g of KNO, is dissolved in 213 g of water at 23.00 °C. KNO, (s) soln= 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? H₂O Incorrect 1.87 AHxn= What is the enthalpy of the reaction? K+ (aq) + NO3(aq) 4.0 Incorrect kJ kJ/mol
A piece of metal (mass = 43.4 g) at 135 ̊C is placed in a Styrofoam coffee cup containing 41.2 g of water at 25.0 ̊C.  When the metal and water reach equilibrium, the final temperature of the water is 39.8 ̊C. What is the specific heat of the metal to three decimal places. The specific heat of water = 4.18 J/g-C.
If a sample of salt is in water in a constant pressure calorimeter with a heat capacity of 35.5 J/℃ Salt: FeCl2 Mass of Salt: 2.288 g Mass of Water: 1.768 g Initial Temp: 20.00 c Final Temp: 25.646312 c a) Calculate the heat of the solution. b) Calculate the heat of the calorimeter. c) Calculate the heat of the reaction. d) Calculate the value of DHdiss.
Consider the reaction. 2Fe2O3⟶4Fe+3O2. Δ?∘rxn=+824.2 kJ The formation of 12.0 g of O2 results in the release or absorption of what amount of heat? in kJ
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. what is the total heat for the dissoulion reaction of the 6.55 g of salt? How many moles of the unknown salt were used in the reaction? what is the enthalpy change (in KJ/mol of salt for the dissolution reacrion?
E In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH), was added to 70.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and BO specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H₂O
Calorimeler? 5. In a calorimetry experiment similar to the one performed today, a student used 50.0 mL of 1.0 M NaOH and 50.0 mL of 1.0 M HCl each initially at 22.5 °C. The maximum temperature observed after mixing was 28.0 °C. What is the heat of reaction in units of kJ? Show all work. 6. The true value for the experiment described in the previous question is 2.89 kJ. Calculate the % error.
combustion products? 2. The standard enthalpy of formation of liquid water AH3° is -285.9 kJ/mole. Write the balanced chemical equation for which that value is appropriate.
ch.10.
In the following reaction, how many moles of CH;OH are required to produce -2191 kJ of heat? 2 CH;OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH° = -1280. kJ mol 1 3 4 6. C 7 8 9. + +/- x 100