Determine the heats of reaction (DH) for the following reaction: Fe2O3 (s) + 3 CO (g) --> 3CO2 (g) + 2 Fe (s) Given the following equations: CO (g) + 1/2 O2 (g) --> CO2 (g) DH = -283.0 kJ 2 Fe (s) + 3/2 O2 (g) Fe2O3 (s) DH = -824.2 kJ --> Answer: DHrxn=

Determine the heats of reaction (DH) for the following reaction: Fe2O3 (s) + 3 CO (g) --> 3CO2 (g) + 2 Fe (s) Given the following equations: CO (g) + 1/2 O2 (g) --> CO2 (g) DH = -283.0 kJ 2 Fe (s) + 3/2 O2 (g) Fe2O3 (s) DH = -824.2 kJ --> Answer: DHrxn=

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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Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic     (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =  kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1
Calculate the enthalpy change in kJ for the following reaction given the data below. Answer: -610.1 kJ    P4O10(g) + 6 PCl5(g) --> 10 Cl3PO(g)                A                1/4 P4(s) + 3/2 Cl2(g) --> PCl3(g) Ho/kJ = -306.4 B                P4(s) + 5 O2(g) --> P4O10(g) Ho/kJ = -2967.3            C                PCl3(g) + Cl2(g) --> PCl5(g) Ho/kJ = -84.2            D                PCl3(g) + 1/2 O2(g) --> Cl3PO(g) Ho/kJ = -285.7
Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic     (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =   kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
4. Hess's Law Calculate AH for the reaction: 2 C(s) + H2(g) → C:H2(g), given the following chemical equations and their respective enthalpy changes: C2H2(g)+02(g)→2CO2(g)+H20(1) AH, = -1299.6 kJ (1) %3D C(s)+02(g)→CO2(g) AH, = -393.5 kJ (2) H2(g)+502(g)→H20(1) AH3 = -285.8 kJ (3)
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
According to the reaction below what is the value of KKJ for the complete combustion of 1.00 g of CH4g?
When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat (in kJ) is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg? ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05
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Given the following two reactions:(1)Fe(s) + Cl2(g)->FeCl2(s) H(1) = -341.8 kJ(2)Hg(l) + Cl2(g)->HgCl2(s) H(2) = -224.3 kJcalculate the enthalpy change for the following reaction:(3) FeCl2(s) + Hg(l)-> Fe(s) + HgCl2(s) H(3) = kJ
A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation:B2H6(g)+3O2(g)➔B2O3(s)+3H2O(g)ΔHcombustion for this process is –1958 kJ/mol. Assume that 0.411 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 22.61°C. What is the final temperature of the calorimeter? The answer is not 18.922°C
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?