On the heating curve below, the RED ARROW indicates the substance in [ Select] phase, while the BLACK ARROW indicates the [ Select ] point. 140°C Temperature 100°C 0°C -10°C
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![On the heating curve below, the RED ARROW indicates the substance in
[ Select ]
phase, while the BLACK ARROW indicates the
[ Select ]
point.
140°C
Temperature
100°C
0°C
-10°C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89f09dec-875a-4c3e-baa2-de78dd3089ec%2F956e1d02-5586-4521-85c7-d658eea37a9f%2F67fc4hm_processed.jpeg&w=3840&q=75)
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- Using this table of temperation changes of C13H10O,what will be the freezing point of C13H10OThe following information is given for silver at 1atm: boiling point = 2212 °C melting point = 961 °C specific heat solid= 0.238 J/g °C specific heat liquid 0.285 J/g °C = KJ AHvap(2212 °C) = 254 kJ/mol AHfus (961 °C) = 12.0 kJ/mol What is AH in kJ for the process of freezing a 32.4 g sample of liquid silver at its normal melting point of 961 °C. |How much energy (transferred as heat) is required to completely melt a 6.14 g sample of copper? Reference values Substance Specific heat Melting point, °C Heat Specific heat of a liquid (0/(gx°C) Boiling point, of a solid (enthalpy) of fusion (J/g) (0/(8×°C) °C Copper 0.385 1085 205 0.49 2562 Iron 0.444 1538 272 0.82 2862 Silver 0.240 961.8 88 0.28 2162 Water 2.092 333 4.179 100 O A. 2.56 kJ O B. 1.26 kJ O C. 3.01 J O D. 1370 kJ O E. 33.4 J
- Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °CThe following information is given for cobalt at 1atm: boiling point = 3097 °C Hvap(3097 °C) = 389 kJ/mol melting point = 1495 °C Hfus(1495 °C) = 15.5 kJ/mol specific heat solid= 0.418 J/g°C specific heat liquid = 0.686 J/g°C What is H in kJ for the process of freezing a 46.3 g sample of liquid cobalt at its normal melting point of 1495 °C._____ kJCondensation occurs when liquid phase of a substance is converted to its gaseous phase true/false
- 2. Calculate the amount of energy absorbed when 75g ice @ -4°C melts to 31°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?The following information is given for manganese at 1atm: boiling point = 2095 °C Hvap(2095 °C) = 225 kJ/mol melting point = 1244 °C Hfus(1244 °C) = 14.6 kJ/mol specific heat solid= 0.477 J/g°C specific heat liquid = 0.837 J/g°C What is H in kJ for the process of freezing a 47.4 g sample of liquid manganese at its normal melting point of 1244 °C.Specific heat solid The following information is given for silver at 1 atm: T Tm = 2212.00°C = 961.00°C AHvap (2212.00°C) = 2.355 x 103 3/9 J/g AH (961.00°C) = 110.8 3/9 0.2380 J/g °C 0.2850 J/g °C Specific heat liquid A 42.70 g sample of solid silver is initially at 943.00°C. If 7.080 × 103 J of heat are added to the sample at constant pressure (P = 1 atm), which of the following is/are true? (Select all that apply.) The sample is a solid in equilibrium with liquid. The sample is a gas. The sample is at a temperature of 961.00°C. The sample is at a temperature greater than 961.00°C. The sample is a liquid.
- Table 1. Listed below are the common metals with different masses. These metals also have different heat energy and different final temperature at a constant time depending on its thermal conductivity. Metals 25 grams of copper 100 grams of aluminum 20 grams of brass 1 kg steel 50 grams of bronze T₁ 21.4 °C 21.4 °C 21.4 °C 21.4 °C 21.4 °C LE (Ctrl) - T₂ 75 °C 60 °C 55 °C 40 °C 35 °C Heat energyBased on the PEC diagram, which of the following best describes the mixing of these substances? PE UM M: mixed state M UM: unmixed state #C the substances do not mix at any temperatures but mixing increases with a increase in temperature the substances mix at high temperatures only and mixing increases with an increase in temperature. the substances mix at all temperatures but mixing may increase with a decrease in temperature the substances mix at all temperatures but mixing increases with a increase in temperatureThe following information is given for ethanol at 1 atm: Boiling point = 78.40°C Heat of vaporization = 200.0 cal/g Melting point = –114.5°C Heat of fusion = 26.04 cal/g Specific heat gas = 0.3418 cal/g°C Specific heat liquid = 0.5880 cal/g°C A 22.80 g sample of liquid ethanol is initially at –68.20°C. How many kcal of energy must be added to the sample to raise its temperature to 94.20°C? Energy added = kcal