How much heat energy is transferred when 8 moles of CH3OH react? 2 CH3OH) + 302 (g) +4 H20 (0 + 2C02 (9) 4= -1452.8 kj/ mol O a. 363.2) b. 5811) OC.- 5811J Od.- 363.2) QUESTION 38 A 2.5 L container with 2 mol N2 gas has a pressure of 2.40 atm, 0.40 mol of gas escape, what is the new pressure? O a. 41 atm O b.0.10 atm Oc. 9.8 atm d. 0.82 atm

How much heat energy is transferred when 8 moles of CH3OH react? 2 CH3OH) + 302 (g) +4 H20 (0 + 2C02 (9) 4= -1452.8 kj/ mol O a. 363.2) b. 5811) OC.- 5811J Od.- 363.2) QUESTION 38 A 2.5 L container with 2 mol N2 gas has a pressure of 2.40 atm, 0.40 mol of gas escape, what is the new pressure? O a. 41 atm O b.0.10 atm Oc. 9.8 atm d. 0.82 atm

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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If the heat produced by the reaction of combustion of 1 mole of ethanol (MMethanol" 46.07 g/mol) is 1366.8 kJ/mol, (see the thermochemical equation below, formula of ethanol is C2H6O), how much heat in kJ is produced by the combustion of 155 g of ethanol at the same conditions? C2H6O(g) + 302(g) 2CO2(8) + 3H2O(g); AH°rxn=-1366.8 kJ/mol O 8.818 O 2.11854 x10s O 4.06 x102 O 4.60x103 2.12x105
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b My Questions | bartleby 101 Chem101 app.101edu.co Submit Question 11 of 29 In the following reaction, how much heat is generated when 3.43 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol %3D kJ 1 4 8 +/- x 100 7:50 PM O Type here to search 12/9/2019 LO
Based on the following reactions: Rxn A: C(s) + O2(g) CO2 (g) AH C = -393.5 kJ/mole Rxn B: C8H18() + 25/2 O2(e) → 8CO2(g) + 9H2O) AH°C = -5461 kJ/mole Which reaction would produce more heat 3*A or B? ) 3*A would produce more heat B would produce more heat they would produce the same amount of heat
The following thermochemical equation is for the reaction of water(l) to form hydrogen(g) and oxygen(g). 2H2O(l) -> 2H2(g) + O2(g) ΔH = 572 kJ How many grams of H2O(l) would be made to react if 110 kJ of energy were provided? _____ grams.
15. The balanced equation below shows the combustion of propane gas: C3H8(g) 502(g) 3CO2(g) + 4 H2O() When 4.4 g of propane gas is combusted, 222 kJ of heat is released. The enthalpy change will be representec with a sign, which corresponds to an process. AXla a. negative, endothermic b. negative, exothermic c. positive, endothermic d. positive, exothermic A)+BZg
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A chemist measures the energy change AH during the following reaction: Cl₂(g) + H₂(g) → 2 HCl(g) Use the information to answer the following questions. This reaction is... Suppose 35.0 g of Cl₂ Will any heat be released or absorbed? react. AH-184. kJ 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. O endothermic. O exothermic. O Yes, absorbed. O Yes, released. O No. x10 X
A propane BBQ combusts propane as shown below: СЗН8 (9) + 5 О2 (9) - 3 CO2 (a) + 4 H2O ) A,H = -2220 kJ/mol What mass of carbon dioxide (in g) is produced when a BBQ grill releases 135 kJ of heat to its surroundings at constant pressure? No pork roasts were cooked in the making of this question.
Octane (C8H18) undergoes combustion according to the following thermochemical equation: 2C8H18(l) + 25 O2(g) --> 16CO2(g) + 18 H2O(l) delta H rxn= -11,020 kj/mol Given that delta H f[CO2(g)]= -393.5 kj/mol, delta H f[O2(g)]= 0 kj/mol and delta H f[H2O(l)]= -285.8kj/mol, calculate the standard enthalpy of formation of octance