What is the most common way that energy is exchanged with the environment during a chemical reaction? 2 Through the creation of water molecules b By burning oxygen с Through the production of electricity d By the production or absorption of heat A__ is a device that is designed so that there is no exchange of heat between the system and surroundings. a barometer b calorimeter с chromatograph d spectrophotometer

What is the most common way that energy is exchanged with the environment during a chemical reaction? 2 Through the creation of water molecules b By burning oxygen с Through the production of electricity d By the production or absorption of heat A__ is a device that is designed so that there is no exchange of heat between the system and surroundings. a barometer b calorimeter с chromatograph d spectrophotometer

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...

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Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) 2HCl(g) AH = -184.6 kJ Reaction 2: 20F2(g) → O₂(g) + 2 F₂ (g) AH = −49.4 kJ Reaction 3: N₂(g) + 2O₂(g) →→→ 2NO₂(g) AH = +66.4 kJ Use Reaction 2. How much energy (in kJ) is released when 69.0 g of oxygen difluoride decompos Answer: kJ (enter a positive value)
An isolated system is one that O exchanges heat and matter with the surrounds. exchanges neither heat nor matter with the surroundings. O exchanges matter but not heat with the surroundings. O exchanges heat but not matter with the surroundings.
Hydrogen sulfide, H2 S, is produced during decomposition of organic matter. When 0.4300 mol H2S burns to produce SO2 (g) and H20(g), -222.7 kJ of heat is released. What is this heat in kilocalories? Heat kcal
Reactions are classified as either exothermic or endothermic. Exothermic reactions feel hot (e.g., a burning campfire), whereas endothermic reactions feel cool (e.g. squeezing an instant cold pack). A thermometer measures the temperature of the surroundings in a calorimeter to determine the amount of energy being transferred by the system. Water molecules speed up when they gain heat and slow down when they lose heat; note that you can track both the cold and hot water molecules in the simulation based on the shade of red of the larger central oxygen atom by checking the box labeled Show microscopic view. Select the Experiment tab in the simulation, and then click Run Demonstration. When observing the simulation, pay particular attention to the temperature change and movement of the molecules by clicking Show microscopic view when HCl and NaOH neutralize each other in the fourth experiment. Use your observations to complete the following sentences. Match the words in the left column to…
Titanium reacts with iodine to form titanium(III) iodide, emitting heat, via the following reaction: 2Ti(s)+3I2(g)→2TiI3(s), ΔHrxn=−839kJ Determine the mass of titanium that reacts if 1.53×103 kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units. Determine the mass of iodine that reacts if 1.53×103 kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units.
1. The thermochemical equation showing the formation of ammonia, NH3 from its elements is AH - -92 kJ Na(g) + 3H2[g) - 2NH3(g) This equation shows that 92 kJ of heat is A. lost to the surroundings when one mole of hydrogen is used up in the reaction B. absorbed from the surroundings when one mole of nitrogen reacts C. absorbed from the surroundings when one mole of ammonia is formed D. lost to the surroundings when 2 moles of ammonia is formed 2. Given the hypothetical thermochemical equation: A +B-C+D AH - -430 kJ Which among the following statements is correct about this reaction? A. the reaction is endothermic B. the equation may be written as A +B+ 430 kJ -C +D C. the heat content of C and D is greater than the heat content of A and B D. the heat content of A and B is greater than the heat content of C and D 3. Which of the following is an example of an exothermic process? C. evaporation of water D. sublimation of dry ice A. melting of ice B. freezing of water 4. An oxyacetylene…
[References] Use the References to access important values if needed for this question. When HBr(g) reacts with Cl₂(g) according to the following reaction, 9.902 kcal of energy are evolved for each mole of HBr(g) that reacts. Complete the following thermochemical equation. 2 HBr(g) + Cl₂(g) → 2 HCI(g) + Br₂(g) AH = kcal
Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J; 1 kcal = 1000 cal J kJ kcal 549 0.684 0.226
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI, (аq) + 3 Н, (2) AH1 = -556.0 kJ 2. HCl(g) HCl(aq) AĦ2 = -74.8 kJ 3. H, (g) + Cl, (g) → 2 HCI(g) ΔΗ = -1845.0 kJ 4. MCI, (s) – MCI, (aq) AĦ4 = -493.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) – - 2 MCl, (s) -556.0 ΔΗ- Incorrect
Explain what the equation Q = m•C•ΔT means and how it relates to energy and calorimetry.
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 2.70kg of water at 39.2°C . During the reaction 128.kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1 . Be sure your answer has the correct number of significant digits.
When 145 mL of 0.212 M NaCl(aq) and 145 mL of 0.212 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.7°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.14 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction.