4. Consider the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) having AH = -484 kJ/mol. Determine the magnitude of the heat exchanged with the surroundings when 4 mol of H2 and 4 mol of O2 react. (a) 484 kJ (b) 968 kJ (c) 1452 kJ (d) 1936 kJ (c) 2904 kJ (f) 3872 kJ

4. Consider the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) having AH = -484 kJ/mol. Determine the magnitude of the heat exchanged with the surroundings when 4 mol of H2 and 4 mol of O2 react. (a) 484 kJ (b) 968 kJ (c) 1452 kJ (d) 1936 kJ (c) 2904 kJ (f) 3872 kJ

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

A 148 g sample of an unknown metal at 74.0 oC is placed in a beaker containing 80.0 g of H2O at 25 oC. The final temperature of the metal sample and water is 32 oC. cH2O(l) = 4.184 j/ g oC SHOW ALL WORK (a) What is the specific heat (c) of the metal? (b) 5 common metals have the following specific heat capacities (c) [given in units of J/g oC] : Aluminum: 0.921 Copper: 0.377 Gold: 0.126 Iron: 0.461 Nickel: 0.502 Your sample is most likely to be which metal?
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) H = 151 kJ When 51.2 grams of Fe3O4(s) react with excess hydrogen(g), kJ of energy are
(incorrect) Consider the following reaction carried out under constant pressure CaSO4(s) + 4C(s) AHxn=-510.1 kJ Cas(s) + 4CO(g) Calculate the heat associated with the complete reaction of 24.0 g of CaS with 26.1 g of CO. → -1.19x102 kJ (Correct answer) -4.76×10² kJ -5.51×10² kJ -1.70x102 kJ (Your answer) -4.80×10² 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
A 125 g piece of rock of unknown specific heat is heated to 93 degrees C. The rock is then dropped into 100 g of water at 19 degrees C. the water temperature rises to 31 degrees C. What is the specific heat of the rock? (3) O 0.65 J/(g °C) O 0.65 J O 0.71 J/g °C) O 1.14 J/g.
The overall reaction in a commercial heat pack can be repre- sented as 4Fe(s) + 30₂(g) 2Fe₂O3(s) AH = -1652 kJ d. How much heat is released when 10.0 g Fe and 2.00 g O₂ are reacted?
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.
Calculate AHO,xn for each of the following using data from Appendix B. (a) 2 H2S(g) + 3 02(g) → 2 SO2(g) + 2 H20(g) kJ (b) SiO2(s) + 4 HF(g) → SİF4(g) + 2 H20(/) kJ
Consider the decomposition of hydrogen bromide to form hydrogen and gaseous bromine, Br2(g): HBr(g) 1/2 H2(g) + 1/2 Br2(g) H = 72.5 kJ (a) What is the enthalpy change for the reverse reaction?Hreverse = _____ kJ/mol(b) Balance the forward reaction with whole-number coefficients. What is H for the reaction represented by this equation?H = _____ kJ/mol