The following table contains some standard enthalpies of formation, \( \Delta H_f^\circ \), at 298 K:| Substance | Formula | \( \Delta H_f^\circ \) (kJ/mol) ||-----------------|-----------|---------------------------------|| Carbon dioxide | \( \text{CO}_2(g) \) | -393.5 || Carbon monoxide | \( \text{CO}(g) \) | -110.5 || Methane | \( \text{CH}_4(g) \) | -74.80 || Propane | \( \text{C}_3\text{H}_8(g) \) | -103.85 || Water (liquid) | \( \text{H}_2\text{O}(l) \) | -285.8 || Water vapor | \( \text{H}_2\text{O}(g) \) | -241.8 |You may want to reference (Pages 186 - 189) Section 5.7 while completing this problem.**Part A**Many portable gas heaters and grills use propane, \( \text{C}_3\text{H}_8(g) \).Using enthalpies of formation, calculate the quantity of heat produced when 20.0 g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.Express the heat in kilojoules to three significant digits.**Input Field for Answer:**- Text box (with unit in kJ)**Submission Status:**- Incorrect; Try Again- 4 attempts remaining**Feedback Section:**- Provide Feedback

Given: mass of propane = 20 g Standard enthalpy of CO2(g) = -393.5 kJ/mol Standard enthalpy of…

The lowing tutle contans some standard enthaipies of formation, AH"r, at 296 K. • Part A Substance Formula Alt (kJ/mol) Many portable gas heaters and grils use propane, C;Hs(g). Carbon dioxide -393.5 Using enthalpies of formation, calculate the quantity of heat produced when 20.0 g of propane is completely combusted in air under standard conditions Assume that liquid water is forming Carbon monoxide CO(g) Methane -110.5 CHalR) -74.80 Express the heat in kilojoules to three significant digits. Propane CaHa(g) -103.85 Vol AZO + HO(1) H30(g) Water 285.8 Water vapor -241.8 kJ You may want to reforence (Pages 186-190) Section 5.7 while completing this problem Submit Previous Answers Request Answer X Incorrect; Try Again: 4 attempts remaining

The lowing tutle contans some standard enthaipies of formation, AH"r, at 296 K. • Part A Substance Formula Alt (kJ/mol) Many portable gas heaters and grils use propane, C;Hs(g). Carbon dioxide -393.5 Using enthalpies of formation, calculate the quantity of heat produced when 20.0 g of propane is completely combusted in air under standard conditions Assume that liquid water is forming Carbon monoxide CO(g) Methane -110.5 CHalR) -74.80 Express the heat in kilojoules to three significant digits. Propane CaHa(g) -103.85 Vol AZO + HO(1) H30(g) Water 285.8 Water vapor -241.8 kJ You may want to reforence (Pages 186-190) Section 5.7 while completing this problem Submit Previous Answers Request Answer X Incorrect; Try Again: 4 attempts remaining

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...

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II. Rapid walking through a distance of 2.2 km for 30 minutes per day requires 41 J while swimming for the Same penod of time through the same distance requires 226 J. Will these forms of exercise allow you to lose weight equivalent to ig of glucose (MW = 180 g/mol) in 1 week? The standard enthalpy of combustion of glucose is -2806 kJ.
One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%
Consider the following balanced combustion reaction: C7H16(l) + 11 O2(g) → 7 CO2(g) + 8 H2O(g) ΔrH°= -1160 kJ/mol If the density of C7H16(l) is 0.68 g/mL, how much heat (in J and scientific notation) is released if 125 mL of C7H16(l) undergoes complete combustion?
A 0.1375g sample of solid Mg is burned in a constant volume bomb calorimeter that has a heat capacity of 3024 J/0C. The temperature increases by 1.1260C. Calculate the heat given off by the burning Mg in kJ/g Mg and kJ/mole Mg
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A chemist measures the energy change AH during the following reaction: 2 NH;(g) - N(9)+3H,(9) AH=160, kJ Use the information to answer the following questions. O endothermic. This reaction is... O exothermic. Suppose 93.6 g of NH, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. Explanation Check 02021 McGraw Hill LLC. Al Rights Reserved Terms of Use Pivecy
A chemist measures the energy change AH during the following reaction: CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(1) N Use the information to answer the following questions. This reaction is... Suppose 23.2 g of CH4 react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. ΔΗ= - 882. kJ endothermic. exothermic. OYes, absorbed. OYes, released. No. 0 kJ X 5
How much heat is rel;eased to the surroundings when 5.00 g of CO2 is produced according to the following thermochemical equation? C3H8 + 5 O2 --> 3 CO2 + 4 H, AHn = -2220 kJ/mol %3D Note: the molar mass of CO2 is 44.0 g/mol 757 kJ O252 kJ 740 kJ 84.1 kJ
a) Given that AgNO3 is -124.4 kJ/mol, at standard conditions, what is dH when 56g of AgNO3 (M = 169.9 g/mol) reacts? b) If the heat involved (derived from answer a) is transferred without loss to 100.0g of water at 25ºC, what is the final temperature of the water (CH2O = 4.18J/gºC)?
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