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 %3D cal kJ 528 185 0.634 Submit Answer Retry Entire Group 8 more group attempts remaining

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…

Identify the correctly written "formation reaction" among the following reactions. Hint: Recall the definition of a "formation reaction". O 2H2 (g) + 02 (g)→ 2H20 (1) N2 (g) + O2 (g) → 2NO (g) O 2H2 (g) + 02 (g)→ 2H20 (g) 2C (s. graphite) + 2H2(g) → C2H4 (g) H20 () + 1/2 02 (g) → H202 (1)

Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ  Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ  Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ    Use Reaction 3.   How much energy (in kJ) is absorbed when 106. L of nitrogen dioxide is created at STP? Round to the nearest whole number.

1. How many grams of copper (II) oxide are needed to produce 693 kJ of energy? 3 CuO + 2 Al -> 3 Cu + Al2O3  △ H  = 1190 kJ/mol 2. How much titanium in grams is required to release 126.81 kJ of heat? Ti + 2 B -> TiB2  △ H  = 316 kJ/mol

Write and balance the equation for the complete combustion of acetylene,  C2H2.  Phase symbols and energy changes are optional.

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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

nuraipy changes in chemical reactions Read through pages 18-20 in your laboratory manual for information on how to calculate the enthalpy change in a solution. Part A - Calculating ms In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 °C. The effective mass of the glass in the thermos flask (mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-¹K-1¹. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-¹K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Calculate the total mass of solution in kilograms (ms) Give your answer to four significant figures. ▾ View Available Hint(s) Hint 1. Calculating ms mg = mass water (kg) + mass solute (kg) —| ΑΣΦ Submit Request Answer ? kg < Pear 10

ORT SHEET Heat of Neutralization EXPERIMENT elemsboomfchg lom 12 A. Heat Capacity of Calorimeter 1. Temp. of calorimeter and water before mixing 2. Temp. of warm water °C 22.0 39,0 30.3 3. Maximum temp. determined from your curve °C 4. Heat lost by warm water (temp decrease x °C 50.0 g x 4.184 J/K-g) = 02), 5. Heat gained by cooler water (temp. increase x 50.0 g x 4.184 J/K-g) = 30,3 22.0)x 13626J s0.0gmpi S0.0gy 6. Heat gained by the calorimeter [(4) – (5)] = 7. Heat capacity of calorimeter: heat gained by the calorimeter temperature increase J/K 3. Heat of Neutralization of HCl-NaOH 22.2 22.2. °C . Temp. of calorimeter and NaOH Temp. of HCI AT determined from your curve after adding HC1 °C to the NaOH Heat gained by solution (temperature increase x ON 100 g x 4.184 J/K-g) = 9977.8J %3D Heat gained by calorimeter (temperature increase x heat capacity of calorimeter) = J %3D Total joules released by reaction [(3) + (4)] = Tight O 2018 Pearson Education, Inc.