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- question 15 You have decided to try a new video game called World of Alchemist Hordes (WoAH) and created a character named Artemis. Use the following information for this question Werewolf blood freezes at -12.0 degrees Arwenheit (°A) and boils at 28.0 °A. Its heat of fusion is 65.0 cal/g and heat of vaporization is 400. cal/g. The specific heat of liquid werewolf blood is 1.473 cal/g°A. Part a) What is the heat released in cal when 0.186 kg of frozen werewolf blood at -12.0 °A , melted to liquid? (Please show your work so I can understand going forward) Part b) What is the heat absorbed in cal when 0.186 kg of liquid werewolf blood at -5.0 °A, is heated to 22.0 °A? (Please show your work so I can understand going forward)Olivia and Jaime are trying to increase the temperature of a substance by heating it. . What is the quantity of heat in kiloJoules required to raise the temperature of 4.6 kg of the substance from-5∘C to 127 ∘C at a pressure of 1.0 atm? Please keep three significant figures. Useful information: Melting point =293 K heat of fusion =3.90 x 104 J/kg. boiling point is 423 K heat of vaporization 7.80 x 104 J/kg (at a pressure of 1.0 atm). The specific heats for the solid phase is 600 J/(kg K) The specific heats for the liquid phase is 1000 J/(kg K) The specific heats for the gaseous phase is 400 J/(kg K)Question 17 A substance is characterized by the thermodynamic data below. Using this, determine the amount of heat (in kJ) required to warm 125.0 grams of the substance from 4.2°C to its melting point, and then completely melt it. Cs, solid 1.92 J/g°C Cs, liquid 3.14 J/g°C Cs, gas 1.59 J/g°C ∆H fus 4.89 kJ/mol ∆H vap 50.88 kJ/mol Melting point 42.5°C Boiling point 176.2°C Molar mass 159.4 g/mol
- Which equations heat, cool and can either heat or cool the surroundings? C4H4S(s) → C4H4S(l) 4C(g) +4H(g) + S(g)→ C4H4S(g) C4H4S(l) → C4H4S(g)The heating curve for an unknown substance is shown below. Based on this curve and the information given, answer the question below. In addition to the heating curve above, you know the following information for this substance: • The Heat of Fusion is 38.3 cal/g The Heat of Vaporization is 89.5 cal/g • The Specific Heat in the liquid phase is 0.372 cal/g-°C Question: If you have 13.5 grams of this substance in the solid state at 14 °C (Point B), how much total heat energy (in calories) is required to completely transform it into a gas at 83 °C (Point E)?Suppose 75.0 g of water at 25.0°C is heated until it vaporizes at 100°C. How much heat was needed?Helpful information:Heat of fusion of water = 334 J/gSpecific heat of water = 4.184 J/g·°CHeat of vaporization of water = 2.26 x 103 J/g
- A 7.0 g ice cube is placed into 230 g if water. Calculate the temperature change in the water upon the complete melting of ice. Hint: Determine how much heat is absorbed by the melting ice and then use q=mcat to calculate the temperature change of the 230 g of water.What is the total amount of heat released when 94.0 g water at 80.0 °C cools to form ice at −30.0 °C?The heat of dissolution of a solid substance was determined using an insulated calorimeter containing 150 grams of water initially at 27.4°C. If the temperature of the water increased to 32.8°C, what is the heat of dissolution of the solid? a.) -8103 b.) 8103 c.) -3386J d.) 3386J
- How much energy is needed to heat 356 g of ice at -10 °C to 0 °C and melt it?Heat = (mass)(0.5038)(change in temperature)Heat = (mass)(79.7)Which phase change releases energy (exothermic)? Group of answer choices H2O (s) -> H2O (g) H2O (l) -> H2O (s) H2O (l) -> H2O (g) H2O (s) -> H2O (l)A quart of water (950 g) at 28.0°C was placed in ice. When the water cools to 4°C, how much heat is transferred to the ice? The specific heat of water is 4.184 J/g·°C. Answer: 95.4 kj, I just need steps ty!