NEED A PERFECT PAPER? PLACE YOUR FIRST ORDER AND SAVE 15% USING COUPON:

SOLVED

31) Which of the following processes is endothermic? A) the freezing of water B) the combustion of butane C) a hot cup of coffee (system) cools on a countertop D) the chemical reaction in a “hot pack” often used to treat sore muscles E) the vaporization of rubbing alcohol 32) Which of the following processes is exothermic? A) a candle flame B) baking bread C) the chemical reaction in a “cold pack” often used to treat injuries D) the vaporization of water E) None of the above are exothermic. 33) Which of the following processes is endothermic? A) mixing water and acid B) rusting iron C) photosynthesis D) the electron affinity of a fluorine atom E) None of the above processes are endothermic. 34) Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2OΔH°rxn = -11018 kJ A) 19280 kJ B) 19.28 kJ C) 38560 kJ D) 50400 kJ 35) How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)ΔH°rxn = -852 kJ A) 51.2 kJ B) 448 kJ C) 224 kJ D) 1617 kJ E) 808 kJ 36) According to the following reaction, how much energy is required to decompose 59.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s) → 3 Fe(s) + 2 O2(g)ΔH°rxn = +1118 kJ A) 1.42 × 105 kJ B) 1.13 × 104 kJ C) 2.85 × 105 kJ D) 5.70 × 105 kJ E) 8.55 × 105 kJ 37) Using the following thermochemical equation, determine the amount of heat produced from the combustion of 24.3 g benzene (C6H6). The molar mass of benzene is 78.11 g/mole. 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g)ΔH°rxn = -6278 kJ A) 3910 kJ B) 1950 kJ C) 977 kJ D) 40.1 kJ E) 0.302 kJ 38) For a particular process that is carried out at constant pressure, q = 145 kJ and w = -35 kJ. Therefore A) ΔE = 110 kJ and ΔH = 145 kJ. B) ΔE = 145 kJ and ΔH = 110 kJ. C) ΔE = 145 kJ and ΔH = 180 kJ. D) ΔE = 180 kJ and ΔH = 145 kJ. 39) When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C, 169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then A) ΔE = 155.0 kJ and ΔH = 169.5 kJ. B) ΔE = 184.0 kJ and ΔH = 169.5 kJ. C) ΔE = 169.5 kJ and ΔH = 184.0 kJ. D) ΔE = 169.5 kJ and ΔH = 155.0 kJ. 40) When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 683.0 kJ of heat are released during this reaction, and PΔV is equal to -37.00 kJ, then A) ΔH° = +683.0 kJ and ΔE° = +720.0 kJ. B) ΔH° = +683.0 kJ and ΔE° = +646.0 kJ. C) ΔH° = -683.0 kJ and ΔE° = -646.0 kJ. D) ΔH° = -683.0 kJ and ΔE° = -720.0 kJ.

Solution:

15% off for this assignment.

Our Prices Start at $11.99. As Our First Client, Use Coupon Code GET15 to claim 15% Discount This Month!!

Why US?

100% Confidentiality

Information about customers is confidential and never disclosed to third parties.

Timely Delivery

No missed deadlines – 97% of assignments are completed in time.

Original Writing

We complete all papers from scratch. You can get a plagiarism report.

Money Back

If you are convinced that our writer has not followed your requirements, feel free to ask for a refund.