Data Table 4: Temperature of Solution Every 20 Seconds Time after mixing (min:sec) Temperature ("C) Initial 27.8("C) 0.20 27.9("C) 0:40 27.7("C) 1:00 27.7("C) 1:20 27.7("C) 1:40 27.6("C) 2:00 27.5("C) 2.20 27.5("C) 2:40 27.5("C) 3:00 27.4("C) 3:20 27.4("C) 3:40 27.4("C) 4:00 27.3("C) 4:20 27.3("C) 4:40 27.2("C) 5:00 27.1("C)
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- Only typed answer otherwise leave it 82 grams of ethanol are mixed with 327 grams of carbon tetrachloride (CCl4). Initially, the temperature of CCl4 is 86ºC, and after mixing, the final temperature of the mixed solution is 58ºC. Calculate the initial temperature of the ethanol in Celsius.Chemistry Heat of Solution (ΔHsoln) for NH4NO3 TRIAL 1 TRIAL 2 Mass of NH4NO3: (NH4NO3 = 80.05 g/mol): 5.06g 5.01g Volume of Water (mL): 50 mL 50 mL Temperature (°C): 1 min: 22.7°C 22.8°C 2 min: 22.7°C 22.8°C 3 min: 22.7°C 22.8°C 4 min: 14.6°C 22.8°C 5 min: 15.6°C 16.0°C 6 min: 16.0°C 16.0 °C 7 min: 16.0°C 16.0 °C 8 min: 16.2°C 16.2 °C ΔT = (Tfinal - Tinitial): 6.5 6.6 Mass of Calorimeter + Solution (g): 226.22g 226.48g Mass of Calorimeter empty (g): 174.58g 175.04g Mass of Solution (g): 51.64g 51.44g CALCULATIONS PART A: qcalorimeter(cal) = (0.961 cal/g °C) · (m) · (ΔT): cal cal qreaction=-qcalorimeter= cal cal #moles NH4NO3: mol mol ΔHsoln=(qreaction/moles NH4NO3: cal/mol cal/mol Average ΔHsoln(NH4NO3) cal/mol cal/mol %error= % % qreaction=- qcalorimeter.You dissolve 10 grams of a mystery chemical into 150 grams of water. The resulting solution freezes at -2.3 Celsius. Calculate the molar mass of the mystery chemical. (Hint: work backwards). Kf for water is -1.86 Celsius/m.
- Heat of Neutralization Reaction between a Strong Acid and a Strong Base In calculating the mass of water in the mixture, assume that the volume of the solution is mainly from water and that the volume of HCl and NaOH are negligible. Also, assume that the density of water is 1 g/mL. volume of HCl solution: 100ml volume of NaOH solution:100 ml total volume of mixture: 200ml mass of water in the mixture:200g initial temperature of water:20°c final temperature of water:23.41°c qwater? qreaction? molarity of HCl solution: molarity of NaOH solution moles of HCl: moles of NaOH: limiting reactant: moles of limiting reactant Δ?reaction:The recommended daily dose of calcium for an 18-year-old male is 1200 mg. If 1.0 cup of whole milk contains 290 mg of calcium and milk is his only source of calcium source, how much milk should an 18-year-old male drink each day in mL? Suppose the child is lactose intolerant, do some research and explain what type of milk would be a good substitute for the child. Please give mg of calcium per cup of alternative milk value, and show calculations for how much of the alternative milk an 18-year-old male should drink each day in mL. (Hint: 1 cup = 236.588 mL) Show all work. Give numerical answers in 2 significant figures.A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?
- Seconds(s) Tap H2OTemp (°C) Salt Solution(+ 2.5 mL salt)Temp (°C) Salt Solution(+ 5 mL salt)Temp (°C) 30 9 7 0 60 4 4 -1 90 3 2 -2 120 2 1 -2 150 1 1 -2 180 1 1 -2 210 1 1 -2 240 1 1 -2 270 1 1 -2 300 1 1 -2 330 1 1 -2 360 1 1 -2 390 1 1 -2 420 1 1 -3 450 1 1 -3 480 1 1 -3 510 1 1 -3 540 1 1 -3 570 1 1 -3 600 1 1 -3 Attach three (virtual) graphs. On one graph, plot the data from the tap water. On the other two graphs, plot the data from the salt solutions. Clearly label the freezing point on each graph.Find the boiling point and freezing point of a solution containing 0.52 g of glucose dissolved in 30.2 g of water. For water, Kb = 0.52 K kg mol-1; Kf = 1.86 k K kg mol-1) Please compute with 3 significant figures for each step and final answer.3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 19.21°C. Calculate ∆H for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g・°C and the density of the solution is 1.20 g/mL). Make sure answer is in the correct number of significant figures.
- A solution is made by mixing 212.0 mL of ethanol initially at 10.0 C with 212.0 mL of water initially at 22.8 C what is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 G/mL snd the density of water is 1.00 g/mL the specific heat of ethanol is 2.46 J/g and the specific heat of water is 4.184 J/g C.You have 0.500-L of a 0.275-M solution of acetone (C3H6O), initially at 37.0°C. You place a copper brick, initially at a temperature of 150.0°C, into the solution of acetone. The temperature of the acetone and copper brick at thermal equilibrium is 58.0°C. What was the mass of the copper brick? Assume the copper brick does not undergo a phase change over the course of the temperature change. Report your answer in units of g and to 3 significant figures. Hfus = 5.7 kJ/mol Hvap = 31.3 kJ/mol Cgas = 75.5 J/mol K Cliq = 125.5 J/mol K Csolid = 96 J/mol K Boiling Point of Acetone = 329 K Freezing Point of Acetone = 179 KDetermine the final temperature of a 32.3 mL salt solution initially at 21.05ºC when 1.93 kJ of heat is added to the solution. The specific heat of the solution is 3.264 J/(ºC · g) and the density of the solution is 1.235 g/mL. Report your answer in units of degrees Celsius to 4 sig figs, but do NOT include units in your answer.