5.3 b HEAt

Predict thermal equilibrium temperatures. A 14.58-g block of solid zinc at 67.45 C is immersed in a 20.77-g pool of liquid ethanol with a temperature of 10.16 C. When thermal equilibrium is reached, what is the temperature of the zinc and ethanol? Specic heat capacities: zinc = 0.388 J/g DC; ethanol = 2.44J/g C C Material: Block Mass: Copper 5.0 g 10.0 g Flame Duration: 2 seconds Tinitial Tfinal Heat Reset 20.0 .C 71.9 .C 100 joules of heat energy have been added to the block. Experiment Complete Click Reset for a new experiment. 6 of 9 Specific heat capacity is a measure of the amount of heat required to raise 1 g of a substance by 1 C(K). Specific heat capacity can be calculated by: quantity of heat (J) mass (g) . AT( C) Use the following settings: Material: Copper Flame Duration: 2.0 seconds Block Mass: 5.0 g Run the experiment and calculate the value of the specific heat capacity for copper. 385.16 * J/go CIn the laboratory a student finds that it takes 66.2 Joules to increase the temperature of 10.6 grams of solid zinc from 20.9 to 38.4 degrees Celsius. The specific heat of zinc she has measured is 0.226 J/g.C.In the laboratory a student finds that it takes 20.8 Joules to increase the temperature of 13.3 grams of liquid mercury from 24.9 to 37.1 degrees Celsius. The specific heat of mercury she has measured is J/g.C.How much energy is required to raise the temperature of 11.2 grams of solid titanium from 20.9 C to 39.9 C? Answer: Joules A sample of solid chromium is heated with an electrical coil. If 89.0 Joules of energy are added to a 12.5 gram sample initially at 23.8 C, what is the final temperature of the chromium? Answer: .CA chunk of zinc weighing 18.8 grams and originally at 98.23 C is dropped into an insulated cup containing 77.2 grams of water at 22.91 C. Assuming that all of the heat is transferred to the water, the nal temperature of the water is C. The following information is given for ether, C2H50C2H5, at 1 atm: boiling point = 34.6 .C AHvap(34.6 .C) = 26.5 kJ/mol melting point = -116 .C AHfus(-116 .C) = 7.27 kJ/mol specific heat liquid = 2.32 J/goC At a pressure of 1 atm, kj of heat are needed to vaporize a 21.2 g sample of liquid ether at its normal boiling point of 34.6 .C.The following information is given for water, H20, at 1 atm: boiling point = 100 .C AHvap(100 .C) = 40.7 kj/mol melting point = 0.00 .C AHfus(0.00 .C) = 6.01 kJ/mol specific heat liquid = 4.18 /goC At a pressure of 1 atm, what is AH in kj for the process of condensing a 29.3 g sample of gaseous water at its normal boiling point of 100 .C. KJUse the References to access important values if needed for this question. The following information is given for diethyl ether at 1 atm: _ AH.39(34-60C) = Tb _ 34.60C 357.5 M}; _ AHfus(_116'300C) = Tm _ 116.30C 98.10 J/g Specific heat gas = 1.460 J/g C Specific heat liquid = 2.320 J/g C A 21.20 g sample of liquid diethyl ether is initially at -11.00C. If the sample is heated at constant pressure (P = 1 atm), k] of energy are needed to raise the temperature of the sample to 58.40C. The following information is given for tin at 1atm: To = 2270.00.C AHvap (2270.00.C) = 1.939 x 103 J/g Tm = 232.00.C AHfus (232.00.C) = 59.60 J/g Specific heat solid = 0.2260 J/g .C Specific heat liquid = 0.2430 J/g C A 29.30 g sample of liquid tin at 594.00C is poured into a mold and allowed to cool to 27.00 C. How many kJ of energy are released in this process? (Report the answer as a positive number.) Energy = KJ