Consider the following reactions:AH= -1939.402 WO3 (s)kJ/mol2W(s)+ 302 (g)AH= - 477.842H,0 (9)kJ/mol2H2 (g)+ 02 (9)Use Hess's law to Calculate AH (in kJ/mol) for the following reaction:+ 3H,0 (9)W(s)WO3 (s) + 3H2 (a)

According to Hess’s law, if a reaction can be obtained by multiple reaction steps, then the ΔH° of…

AH= -1939.40 kJ/mol Consider the following reactions: 2 WO3 (s) + 302 (9) 2W (s) AH= - 477.84 kJ/mol 2H20 (9) (g) 2H2 (0) + O2 (9) Use Hess's law to Calculate AH (in kJ/mol) for the following reaction: + 3H2 (g) W6) + 3H,0 (9) WO3 (s)

AH= -1939.40 kJ/mol Consider the following reactions: 2 WO3 (s) + 302 (9) 2W (s) AH= - 477.84 kJ/mol 2H20 (9) (g) 2H2 (0) + O2 (9) Use Hess's law to Calculate AH (in kJ/mol) for the following reaction: + 3H2 (g) W6) + 3H,0 (9) WO3 (s)

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

Consider the reaction of nitrogen monoxide with hydrogen to form nitrogen and water vapor, H2O(g): NO(g) + H2(g) 1/2 N2(g) + H2O(g) H = -332.2 kJ Balance the forward reaction with whole-number coefficients. What is H for the reaction represented by this equation?H = kJ/mol.
Consider the following thermochemical equation: 2NO (9) + O2(g) 2 NO, 2(g) AH = -114.1 kJ Choose... If 3.00 x 10 g NO, were produced, then the amount of heat released (in kJ) would -2 be: Consider the following reactions: 2W, + 30, 2 (g) 2 WO3 AH= -1939.40 (s) kJ/mol 2H, + 2 (g) 02 (g) 2H,0 "2 (g) AH= - 477.84 kJ/mol Choose... Use Hess's law to Calculate AH (in kJ/mol) for the following reaction: WO3 (6) + 3H2 (g) W. + ЗН,0 (g) What is the molar heat of combustion of methanol CH,0OH ( in kJ/mol), if the combustion of 1.0 g of methanol causes a temperature rise of 3.68 °C in a bomb calorimeter that has a heat capacity of Choose... 6.43 J/°C? The mole fraction of N, gas in the air is 0.781 at 760 torr. Calculate the partial pressure of N, in air Choose... DI f th
14. For the incomplete combustion of silicon: 2Si(s) + O:(g) → 2SIO(g) AH = -88.2 kJ calculate the amount of heat released for each of the following: (a) 5.00 mol of Si is reacted (b) 5.00 g of Si is reacted
*You may need your knowledge in balancing equations which you had learned in your Chem. 1 1. Calculate AH for the reaction from the given thermochemical equations. Tell whether the reaction is exothermic or endothermic C:H« (9) + Ha(g) CaHo(g) CO-(g) CO2(g) H;O(1) H20() H20() AH = -1411 kJ * CHalg) * CaHelg) + O2(g) * Hz(g) + Oz(g) O2(9) AH = -1569 kJ + AH = -285.8 kJ
The following thermochemical equation is for the reaction of sodium(s) with water(1) to form sodium hydroxide(aq) and hydrogen(g). 2Na(s) + 2H2O(1)- →2NaOH(aq) +H2(g) AH= -369 kJ When 5.86 grams of sodium(s) react with excess water(1), kJ of energy are
How many kilojoules of energy are generated when in 82.8 grams of CO(g) reacts according to the following reaction? CO(g) + O2 (g) → CO2(9) Hint: balance the reaction first Answer in decimal form with 1 decimal place Compound H; (KJ/mol) Compound H;(KJ/mol) CH(9) HCl(g) H,0(g) H2O(1) H2 S(g) 89.5 H2SO,(1) 33 M9SO, (s) -75.7 -93.2 Co2(9) 394.4 -242.7 SO2 (g) NH,C(s) NO(g) NO,(g) -297 -286.7 -316.3 -21 -812.2 -1279.1 SnCl4 (1) Sn0(s) SnO2(s) NaF(s) NaOH(s) Mn0(s) :-287.1 MnO2(s) -581.6 NaCl(s) SO: (9) Zn0(s) ZnS(s) -546.1 -385.8 -520.0 -411.9 -569.9 -396.1 -427.6 -3489 NH3 (9) -47.1 -203.8 CO(g) -111.4 O2(9)
Using Hess's law, what is AHf rxn for the following reaction? NO(G) + O(g) – NO2(9) NO(g) + O3(9) – NO2(9) +O2(9) AH xn = -198.8 kJ/mol Og(9) – 3/2 02(9) AHrxn = -142.2 kJ/mol 02(9) → 20(9) AH Prxn = +498.8 kJ/mol -839.8 kJ/mol -306.0 kJ/mol 394.9 kJ/mol 157.9 kJ/mol O 442.3 kJ/mol QUESTION 8 Octane (C3H18) undergoes combustion according to the following thermochemical equation. 2C8H18() + 2502(g) – 16CO2(g) + 18H20() AH°rxn = -1.0940 x 104KJ/mol What is the standard enthalpy of formation of liquid octane? AH°{(CO2(g)) = -393.5 kJ/mol and AH°F{H2O(1)) = -285.8 kJ/mol 495 kl/mol O -250 kJ/mol -495 kJ/mol -10,940. kJ/mol -2188 kJ/mol
A reaction of the following type is called H2O(g) H2O(1) AH =-44.01KJ/mol O Exothermic reaction O Endothermic reaction O Thermochemical reaction O Thermal reaction
The following thermochemical equation is for the reaction of Fe3O4(s) with hydrogen (g) to form iron(s) and water(g). Fe3O4(s) + 4H₂(g) 3Fe(s) + 4H₂O(g) ΔΗ = 151 kJ When 81.5 grams of Fe3O4(s) react with excess hydrogen (g), kJ of energy are 0. Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
How many kilojoules of energy are generated when in 82.8 grams of CO(g) reacts according to the following reaction? CO(g) + O2 (g) –→ CO2(9) Hint: balance the reaction first Answer in decimal form with 1 decimal place Compound H;(KJ/mol) Compound H;(KJ/mol) HC(g) H,O(g) H2O(1) H,S(g) 89.5 H2SO4(1) 33 M9SO4(8) -546.1 Mn0(s) :-287.1 MnO2(s) NaCl(s) SO3 (g) ZnO(s) ZnS(s) O2(9) CH(9) -93.2 -75.7 -242.7 CO2(g) SO2 (9) NH,Cl(s) NO(g) -394.4 -297 -286.7 -316.3 -21 -812.2 -1279.1 NO2(g) SnCl4(1) Sn0(s) SnO2(s) NaF(s) NaOH(s) NH3 (9) CO(g) -385.8 -520.6 -581.6 -411.9 -569.9 -396 1 -427.6 -3469 -47.1 -203.8 -111.4
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)?
When a 7.41-g sample of solid potassium chlorate dissolves in 59.3 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 22.00 oC to 12.96 oC. Calculate H in kJ/mol KClO3 for the solution process. KClO3(s) K+(aq) + ClO3-(aq) The specific heat of water is 4.18 J/g-K.Hsolution = _________ kJ/mol KClO3.