Consider the following equation: CO + 2H 2 -Calculate the amount of heat (in kJ) released when 4.58 g H2. react with 161.2 g of CO.- CH 30H AH rxn = -128 kJ11.0061314153.Li6.944.Be901226.10.811201114.00121314SI28.08515NaMgAl22.990 24.305347.9.10111226.98230.9741920KCa39.098 40.07821222325Mn51.996 54.938242627Co28Ni58.69329Cu63.54630Zn65 38313233As74.922ScTiCrFeGaGe44.95647.86750.94255.84558.93369.723726303738Sr87.6239Y-88.90640414243Te4445Rh46Pd47484950Sn118.7151Sb121.76RbZr91.224NbMoRuAg107.87In85 46892.90695.95(98)101.07102.91106.4211241114.825556Ba57-7172H73747576Os7778Pt79Au80818283CsTaReIrHg200.59PbBi208.98132.91137.33178 49180.95183.84186.21190.23192.22195.08196.97204.38207.287Fr(223)88Ra(226)89-103104105Db(268)106107Bh(270)108Hs(277)109Mt(276)IIIRg(280)110Rr(265)Sg(271)112Cn(285)113Nh(286)114FI(289)115MeDs(281)(289)• Lanthanideseries57La138.915859Pr140.9161Pm(145)6062Sm150.366364656667Но68CeNdEuGd157.25Tb158.93Dy162.50Er140.12144.24151.96164.93167.26# Actinideseries8990919293949596979899100Th 8LOOP 860644.956 47.86750.94240Zr41Nb92.90642Мо95.9543Tc(98)44Ru101.0745Rh102.9146Pd106.42383937Rb85.468 87.62Sr88.906 91.22478Pt195.08767775Re7472Hf73Ta57-7156Ba137.33Os55Cs132.91Ir180.95183.84186.21190.23192.22178.49106Sg(271)107Bh(270)108Hs(277)109Mt(276)110Ds(281)89-10387Fr(223)88Ra(226)104Rf(265)105Db(268)Lanthanideseries61Pm(145)62Sm150.3663Eu151.966057La58Ce140.1259Pr140.91Nd138.91144.2494Pu(244)95Am(243)9293# Actinideseries89Ac(227)90Th232.0491Pa231.04Np(237)238.03O -256 kJO -1024 kJO -239 kJO -1034 kJO -145 kJ

Answered: Image /qna-images/answer/69ca697c-2a19-4f8b-bc6f-07b9572f41b0.jpg

Answered: Consider the following equation: CO +…

Consider the following equation: CO + 2H 2 CH 3OH AH pm = -128 kJ Calculate the amount of heat (in kJ) released when 4.58 g H2. react with 161.2 g of CO.

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

In the following reaction, how much heat (in kJ) is released when 6.35 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol
In the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -
In the following reaction, how many moles of CH;OH are required to produce -2191 kJ of heat? 2 CH;OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH° = -1280. kJ mol 1 3 4 6. C 7 8 9. + +/- x 100
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
A 138.9 g sample of an unknown metal at a temperature of 99.1 °C is added to 44.72 g of water at a temperature of 19.1 °C. The specific heat of water is 4.184 Jg-1 °C- 1. The final temperature of the system is 52.2°C. Calculate the specific heat of the unknown metal.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
NW113AACE04-21 3. a hunk of metal-like substance was found in an archeological site. In an attempt to identify it, the metal was heated and placed in a calorimeter containing water and determined the specific heat of the metal. If the specific heat of the metal is 0.448 J/g °C, what is the approximate molar mass (atomic mass) and likely identity of the metal? (Hint: compare the molar mass (atomic mass) of metal that of metals in periodic table)
Consider the following reaction carried out under constant pressure 5Cl2(g) + 2P(s) → 2PCl5(g) Δ Hrxn = -749.8 kJCalculate the heat associated with the complete reaction of 84.0 g of Cl2 with 20.6 g of P. -6.15×102 kJ -1.78×102 kJ -4.99×102 kJ -8.88×102 kJ -2.50×102 kJ
Iron has a specific heat capacity of 0.444J/g-C. 50.0 g of iron at 35C is added to 50.0 g of water with a specific heat capacity of 4.184 J/g-C. When the temperature of the resulting mixture stops changing, the temperature is closer to that of the original water than to the iron. True or false?
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?
In the following reaction, how many moles of CH3OH are required to give off 3791 kJ of heat? 2 CH,OH (I) + 3 02 (g) → 2 CO, (g) + 4 H,0(g) AH° = -1280. kJ
How much heat is evolved when 8.89x10° g of ammonia is produced according to the following equation? (Assume that the reaction occurs at constant pressure.) N2(9) + 3H,(g) - 2NH3(g); AH = -91.8 k) kJ evolved