Given the following values for the heats of formation, what is the number of moles of ethane (C₂H6, MW 30.0) required to produce6.77x103 kJ of heat by combustion to CO2 (g) and H₂O (1). Express your answer as a number to 3 significant figures, e.g 0.567 or 23.9.C2H6 (g) + 7/2 O2(g) →2 CO2 (g) + 3 H₂O (1)C2H6 (9)AH = -84.7 kJ/molCO2 (g)AH-393.5 kJ/molH₂O (1)AH = -285.8 kJ/mol

Answered: Image /qna-images/answer/13ee934a-1443-4ec2-90b3-5f28ba062ef8.jpg

Given the following values for the heats of formation, what is the number of moles of ethane (C₂H6, MW 30.0) required to produce 6.77x103 kJ of heat by combustion to CO₂ (g) and H₂0 (1). Express your answer as a number to 3 significant figures, e.g 0.567 or 23.9. C2H6 (g) + 7/2 O2(g) →2 CO2 (g) + 3 H₂O (1) C2H6 (9) AH = -84.7 kJ/mol CO₂ (g) AH = -393.5 kJ/mol H₂O (1) AH = -285.8 kJ/mol

Given the following values for the heats of formation, what is the number of moles of ethane (C₂H6, MW 30.0) required to produce 6.77x103 kJ of heat by combustion to CO₂ (g) and H₂0 (1). Express your answer as a number to 3 significant figures, e.g 0.567 or 23.9. C2H6 (g) + 7/2 O2(g) →2 CO2 (g) + 3 H₂O (1) C2H6 (9) AH = -84.7 kJ/mol CO₂ (g) AH = -393.5 kJ/mol H₂O (1) AH = -285.8 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

Given the study of combustion of butane in the bomb calorimeter in the last problem, what is the enthalpy of reaction for the reaction given below? Give your answer in decimal form to 3 significant figures. Do not enter units since they are already given. (Hint: the reaction below shows 2 moles of butane) 2 C4 H10 (g) + 13 O2 (g) – 8 CO2 (g) + 10 H2O (I) kJ
Which of the following reactions corresponds to the standard enthalpy of formation of methane CH4? A: C(s, gr) + 2H2(g) —> CH4(g) B; CH4(g) —> C(s, gr) + 2H2(g) C: C(s,gr) + 4H (g) —> CH4 D:CH4–> C(s,gr) + 4H(g) Choose one. Thanks!
For the questions of the Experiment of Heat and Temperature: The Law of Dulong and Petit, the following data were obtained for the unknown element. specific heat (S) of unknown element (J/g⚫K) Aw of unknown element (g/mol) 0.339 63.96 b) Calculate the atomic heat (C) in J/mol K for the unknown element. 1) In this case, your answer should be in decimal notation (for example, 0.123, not 1.23*10^-1) with the correct number of significant figures. Also follow the unit specified in each question. Do NOT put its unit in your answer because its unit is shown already in the questions. 2) It means students shouldn't include any letters or text in the "Numeric answers", because otherwise it'll be marked wrong even if the numbers are correct. Type your answer...
At constant pressure, the combustion of 11.14 g of C₂H6(g) releases 518.0 kJ of heat. What is AH (in kJ) for the reaction given below? 2 C₂H6(g) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(1) AHrxn = ? Give 4 sig figs in your answer. Make sure to write the correct sign before the numerical value for the enthalpy of reaction.
ch.6.6
Please solve number 2
Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
For a particular isomer of C3H,8, the combustion reaction produces 5099.5 kJ of heat per mole of C3H13(g) consumed, under standard conditions. 25 C,H1g(g) + 0,(8) – 8 CO,(g) + 9 H,O(g) 8 CO,(g) + 9 H,0(g) AHixn = -5099.5 kJ/mol rxi What is the standard enthalpy of formation of this isomer of C3H13(g)? ΔΗ -215 kJ/mol Incorrect
NaHCO3 (aq) + CH3 COOH (aq) —> CO2 (g) + H2O (l) + CH3 COONa (aq) Calculates the amount of heat energy absorbed by the solution in the calorimeter or the amount of heat energy released by the reaction. Note: 100ml of CH3COOH, 2.5ml of NaHCO3, initial temp of 23c, final temp of 21c
Use Hess’s law to obtain the enthalpy change for this reaction: H2(g) + 1/8 S8(rhombic) -> H2S(g) from the following enthalpies:H2S(g) + 3/2 O2(g) à H2O(g) + SO2(g) ΔH = -518 KJH2(g) + ½ O2(g) à H2O(g) ΔH = -242 KJ1/8 S8(rhombic) + O2(g) à SO2(g) ΔH = -297 KJ
A bomb calorimeter is charged with 10.05 grams of sucrose (C12H22O11). The bomb is surrounded by 500.0 grams of water. The water and bomb have an initial temperature of 20.14 oC. After the combustion of the sucrose, the final temperature is 32.86 oC. The heat capacity of the bomb calorimeter is 10.95 kJ/oC and the specific heat of the water is 4.184 J/goC. Calculate the enthalpy change of the following reaction, as balanced, in kilojoules.C12H22O11(s) + 12O2(g) -> 12CO2(g) + 11H2O(l)