Concept explainers
(a)
Interpretation: Whether the given reaction is exothermic or endothermic should be determined.
Concept Introduction: The reaction which requires energy for the conversion of reactant to product is called as endothermic reaction whereas the reaction that releases some amount energy during the conversion of reactant to product is called as exothermic reaction.
(b)
Interpretation: The amount of energy in kilojoules required when 1.5 mol of SO3 reacts should be determined.
Concept Introduction: The reaction which requires energy for the conversion of reactant to product is called as endothermic reaction whereas the reaction that releases some amount energy during the conversion of reactant to product is called as exothermic reaction.
(c)
Interpretation: The amount of energy in kilojoules required when 150 g of O2 is formed should be determined.
Concept Introduction: The reaction which requires energy for the conversion of reactant to product is called as endothermic reaction whereas the reaction that releases some amount energy during the conversion of reactant to product is called as exothermic reaction.
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Basic Chemistry Plus Mastering Chemistry With Pearson Etext -- Access Card Package (6th Edition)
- (10.8)Which of the following resonance forms of SCN contributes least to its correct structure? (Hint: Assign the formal charge for each atom in all resonance structures.) [:S-C=N:] O b O a Oa and b O C [S=C=N] (b) [:S=C-N:] (c)arrow_forward8. The equation below represents the burning of carbon disulfide, CS20 in a calorimeter. CS20) + 302(g) → CO2(g) + 2SO2(g) + 1690 kJ What mass of CS20 must have burned to increase the temperature of 1.0 kg of water by 15.5°C? [2.92g] n 1471 m -0.967arrow_forward1N2 + 3H2 -----> 2NH3 Diatomic nitrogen has a triple bond. (946) Diatomic hydrogen hs a single bond. (436) The three bonds in ammonia are single bonds. (390) The bond energies are given. Determine the formula to find the heat of reaction. a. (1)(+946) + (3)(+436)+(2)(-390) b. (3)(+946) + (3)(+436)+(3)(-390) c. (1)(-946) + (3)(-436)+(2)(+390) d. (1)(-946) + (1)(-436)+(3)(+390) e. (3)(-946) + (3)(-436)+(3)(+390)arrow_forward
- Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂ H₂ (-1300. kJ/mol), C2H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction ΔΗ = C₂H₂(g) + 2H₂(g) → C₂H6 (9) kJarrow_forward33.9 Given the following two reactions and their enthalpy changes, 2 ClO2 (g) --> Cl2 (g) + 2 O2 (g) Delta H = – 204 kJ 2 TiCl4 (l) + 2 O2 (g) --> 2 TiO2 (s) + 4 Cl2 Delta H = – 139.8 kJ What is the value of the enthalpy change for the reaction that is the sum of these two reactions? 2 ClO2 (g) + 2 TiCl4 (l) --> 2 TiO2 (s) + 5 Cl2 Delta H = ? Select one: a. – 64 kJ b. – 344 kJ c. 64.2 kJ d. 64 kJ e. 344 kJ f. – 204 kJ g. none of thesearrow_forwarddoes it compare with the known melting and boiling point? (1) 9. The average kinetic energy of water molecules is a measure of the temperature of water. When the temperature of water remains constant the average kinetic energy of the molecules remains constant, even though the water is being heated by the Bunsen flame. So, energy is being taken in by the water, but it is not being used to increase the kinetic energy of the molecules. 9.1 What type of energy are the water molecules gaining during a phase change? (1) 9.2 Explain your reasoning (to question 9.1) with reference to the kinetic theory of matter. 10. Write the conclusion. (3) [30]arrow_forward
- In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/molarrow_forwardPractice 9.5 How many grams of chromium(III) chloride are required to produce 75.0 g of silver chloride? CrCl, + 3 AgNO, Cr(NO,), + 3 AgCl Practice 9.6 What mass of water is produced by the complete combustion of 225.0 g of butane (C,H10)? 2 C,Hj0 + 13 0, 8 CO, + 10 H,Oarrow_forwardGO and O-H bonds are stronger than C-C and C-H bonds, because C-O bonds and O-H bonds e polar. The partial charges on the atoms result in stronger attraction between the atoms. This is why combustion reactions are exothermic and why fossil fuels are so valuable Which of the following reactions would you predict to be endothermic? a) 200 + 4H2 > CHạ + 02 b) 2H2(8) + Oz(8) → 2H;O(1) c) Na(s) + Chie) → 2NACI(s) d) paper burning to form CO; and H20 6) Consider the reaction CH3OH + HBr > CH,Br + H;0 Draw the Lewis structures for reactants and products. Which bonds are broken in this reaction? Which bonds are formed? Use the table below to determine if this reaction is exothermic or endothermic and the value for AH. Table 5.4 Average Bond Enthalpies (kJ/mol) C-H 413 N-H 391 0-H 463 155 C-C 348 N-N 163 0-0 146 614 N-O 201 495 d-F 253 C-N 293 N-F 272 0-F 190 C-a 242 C-O 358 N-C 200 2113 799 N-ir 24.1 0-1 234 lir- 237 C-F 485 218 C-a 328 H-H 436 Br-Br 193 C-Br 276 H-F 567 C-I 240 H-CI 431 208…arrow_forward
- 10.105 Complete and balance each of the following: (10.7) a. ZnCO3(s) + H,SO,(aq) b. Al(s) + HBr(aq)arrow_forwardAccording to the given reactions, which of the following is not exothermic? SO2(g) – S(s) + O2(3) AH= +199 kJ/mol AH =+199 kJ/mol SO3(g) – S(3) + 3/2 02(g) AH=+195 kJ/mol so;(g) – SO2(e) + 1/2 02(g) OA. 2 S(s) + 2 02(g) -2 SO2(g) OB. 2 S(s) + 5/2 02(g) –→ SO2(g) + SO3(g) OC. 2502(g) – 2S(s) + 202(g) OD. 2 S(3) + 3 02(g) -2 SO3(g) OE.arrow_forwardFind the AH for the reaction below, given the following reactions and subsequent AH values: B2H6(g) + 6 Cl2(g) → 2 BCI3(g) + 6 HCI(g) ΔΗ = – 72.5 kJ BC13(g) + 3 H₂O(l) → H3BO3(g) + 3 HCI(g) B2H6(g) + 6 H₂O(l) → 2 H3BO3(s) + 6 H2(g) ΔΗ = + 60.8 kJ 1/2 H₂(g) + 1/2 Cl₂(g) → HCI(g) 150.3 kJ ΔΗ = -arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning