Energy cannot be created nor destroyed, but it canbe transferred between a reaction and itssurroundings. The change in energy, AE, ispositive if the reaction absorbs energy, and it isnegative if the reaction releases energy. You mayalso see this expressed in terms of change ininternal energy, AU. For the purposes of thisquestion, AU and AE are equal.Pearson eTextStudy AreaDocument SharingOne way a reaction can transfer energy to or fromthe surroundings is by releasing or absorbing heat.A reaction can also transfer energy, in the form ofwork, through a change in volume. The totalchange in energy is the sum of the heat and work:User SettingsSubmitCourse Tools>E AE=q+ wPart BAt constant pressure, q = AH and w = -PAVand so%3|A mole of X reacts at a constant pressure of 43.0 atm via the reactionΔΕ-ΔΗ-ΡAVX(g) + 4Y(g)→2Z(g),AH° = -75.0 kJ%3D6.Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was2.00 L. Calculate the value of the total energy change, AE, in kilojoules.Express your answer with the appropriate units.• View Available Hint(s)HAΔΕ -ValueUnits%3DSubmitNext >Provide FeedbackP PearsonCopyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use Privacy Policy Permissions Contact Us |7:32 PM82°F Sunny ^ o Ca6/18/202190e Type here to searchPgDrPrtScnF8HomeF9EndF1011DILF3F7EscF5F6F4F1F256

Given ΔH = -75 kJ Pressure = 43 atm Change in volume = 5L to 2L

oses of this energy to or from er absorbing heat. gy, in the form of e. The total e heat and work: Submit Part B and w = -PAV A mole of X reacts at a constant pressure of 43.0 atm via the reaction AV X(g) + 4Y(g)-2Z(g), AH =-75.0 k.J Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, AE, in kilojoules. Express your answer with the appropriate units. • View Available Hint(s) HA AE = Value Units Submit Provide Feedback Next > P Pearson ht © 2021 Pearson Education Inc. All rights reserved. I Ierms of Use I Privacy Policy I Permissions Contact Us 7:32 PM 82°F Sunny 口 d 6/18/2021 90 PrtScn Home End 49 8. 9 立

oses of this energy to or from er absorbing heat. gy, in the form of e. The total e heat and work: Submit Part B and w = -PAV A mole of X reacts at a constant pressure of 43.0 atm via the reaction AV X(g) + 4Y(g)-2Z(g), AH =-75.0 k.J Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, AE, in kilojoules. Express your answer with the appropriate units. • View Available Hint(s) HA AE = Value Units Submit Provide Feedback Next > P Pearson ht © 2021 Pearson Education Inc. All rights reserved. I Ierms of Use I Privacy Policy I Permissions Contact Us 7:32 PM 82°F Sunny 口 d 6/18/2021 90 PrtScn Home End 49 8. 9 立

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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76 of 76 I Review I Constants I Periodic Table Part A Assuming that all the energy given off in the reaction goes to heating up only the air in the house, determine the mass of methane required to heat the air in a house by 15.0 °C. Assume each of the following: house dimensions are 25.0 m x 25.0 m x 2.8 m; specific heat capacity of air is 30 J/K mol; 1.00 mol of air occupies 22.4L for all temperatures concerned. Express your answer using two significant figures. ? g m = Previous Answers Request Answer Submit
What volume of ethane (C2H6(g)) measured at 23.0 oC and 752 tore must be burned to heat 850 g of water from 20 oC to 90.0 oC? The gram standard heat combustion of the gram- specific heat of water is 4.184 J/ g x oC
A chemist measures the energy change AH during the following reaction: 2 NH,(9) - N,(9)+3H,(9) AH = 160. kJ Use the information to answer the following questions. O endothermic. This reaction is... alo O exothermic. Suppose 46.5 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. Be sure your answer has the correct number of significant digits.
A chemist measures the energy change AH during the following reaction: 2 HgO(s) → 2 Hg(1)+O,(g) AH=182. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Yes, absorbed. Suppose 56.6g of HgO react. Yes, released. Will any heat be released or absorbed? 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. kJ Round your answer to 3 significant digits.
The overall reaction in a commercial heat pack can be represented as 4 Fe(s) + 30₂(g) → 2 Fe₂O₂ (s) AH = -1652 kJ a. How much heat is released when 4.80 moles of iron are reacted with excess O₂? Heat = kJ b. How much heat is released when 1.00 mole of Fe2O3 is produced? Heat = kJ c. How much heat is released when 1.40 g iron is reacted with excess O₂? Heat = kJ d. How much heat is released when 11.4 g Fe and 1.90 g O₂ are reacted? Heat = kJ Submit Answer Retry Entire Group 9 more group attempts remaining
10. Nitrogen oxides undergo many interesting reactions in the environment and in industry. Given the following information, caleculate AlI for the overall equation 2NO, (g) + %0, (g) – N.O; (s): N2O5(s) → 2NO(g) + O2(8) AH NO(g) + 02(g) → NO2(g) AH = -57.1 kJ
Imagine an endothermic reaction had been studied (i.e. AHºrn > 0). In this experiment we assumed the calorimeter was perfect (Acalorimeter = 0). If, however, the calorimeter were not perfect and heat flowed from the calorimeter to the contents, would the measured AH Txn be more or less endothermic than the true AH°? rxn
A chemist measures the energy change AH during the following reaction: 2 HgO(s) → 2 Hg(1)+0,(9) AH=182. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Suppose 61.0 g of HgO react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? 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. |kJ Round your answer to 3 significant digits.
When 56.8 of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0 degrees Celsius, 60.1 kj of heat is released at constant pressure. What is the change in enthalpy at standard condition for the reaction (Please type answer no write by hend)
A food product containing 82% moisture content is being frozen. Predict the specific heat of the product at -8 ° C when 82% of the air is frozen. The specific heat of the dry product is 2.5 kJ / (kg ° C). It is assumed that the specific heat of water at -10 ° C is the same as that of water at 0 ° C, and that the specific heat of ice follows the function Cp ice = 0.0062 T frozen + 2.0649. Cp of frozen product = answer J / kg ° C.
How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar? The reaction we performed was: Na(s) + H2O(l) NaOH(aq) + 1/2H2(g) qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater qreaction = -qwater qreaction = -mwater*Cwater*Twater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?
A chemist measures the energy change AH during the following reaction: Cl,(9)+H,(g) → 2 HCl(g) AH=-184. kJ Use the information to answer the following questions. O endothermic. This reaction is... x10 O exothermic. Suppose 62.6g of Cl, 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. kJ Round your answer to 3 significant digits.