Can you help me with the number 3 questions? Also can you please show the step-by-step including the formula? Calculations for Temperature and Phase Change WorksheetThe heat of fusion of ice is 79.7 cal/g.The heat of vaporization of water is 540 cal/g.Report the answer using the correct number of significant figures!1. How much energy is required to melt 100.0 grams of ice? Mass of ice = 100.0gHeat of fusion of ice: 79.100.0g|79.7.cal-1970 cal2. How much energy is required to vaporize 234.5 g of water?234.5g 540 cal--1.2241.2 cal/g12 6630 1.2663X1051.3x105Answer: 1.3 x 105 calcal3. If 30.6 calories are required to vaporize 25 g of a substance, what is the heat of vaporization ofthat substance?mass of substance: 25genergy require vaporization: 30.6 Calmay30.6 cal25926.00 °C?100c,05 (6બ (22)=xtel3.00x 10³cal4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 °C?mass m) = 500.09AT=-1.10°C500.0g (ca.1000) = [500.g (4.1845 -1.10 23.01.2-2,3012×10³.-550 cal5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 °C to0.0924 cal3-21) (100.024)до сm= 1000.09 Q=SOMIATS=1 cal/goc Teinal-TinitidT₁ = 23.00%T2=26.00°C3.00 x 10³ cal (or 1.26 x 10¹J)is required to raise themass of copper: 100gSpecific heat copper: 0.0924cal/g °CAT=100.0°CAnswer: 92.4 cal7. If 25.6 J of energy raised 786 g of a substance from 20.0°C to 35.0°C, what is the specific heat ofthe substance (S)?= mxsx Delta + mass(m) = 786 gramT₁ = 20.0%T₂=35:0°C-0.002171332 TFinal-Tinitial0.002174184511.2552x10Içal6. The specific heat of copper is (0.0924 cal/g°C), how much energytemperature of 10.0 g of copper by 100.0 °C?10.09Mass of water 234.59Heat of vaporization: 540 cal/gHeat of vaporization substance: 1.2 cal/gAnswer: 1.2 cal/g25.65=786 gx sx35°C-20°c)---5=25.6J7869x:79.7 cal/gAnswer: 7970 cal15°CQ==ssocalAnswer: -550. cal (or -2.30 x 10³ J)92.4call(2617X10³J/g °C26.00-23.00=3%Answer: 2.17 x 10-³J/g °C35.0%-2010°C = 15.0°C

Thermodynamics is a branch of chemistry in which we deal with amount of heat evolved or absorbed by…

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Can you help me with the number 3 questions? Also can you please show the step-by-step including the formula?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 15P

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If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
If 10. J of heat is applied to 5.0-g samples of each of the sub stances listed in Table 10.1, which substance’s temperature will increase the most? Which substance’s temperature wilt increase the least?
9.81 A substance has the following properties: Hfusion = 10.0 kJ/mol Hvaporiztion = 20.0 kJ/mol Cp(solid) = 30 J/mol/K Cp(liquid) = 60 J/mol/K Cp(gas) = 30 J/mol/K Which of the four graphs below would he most consistent with these data? Explain how you are able to identify the correct graph.
On a hot day, you take a six-pack ot a on a pcmc, cooling it with ice. Each empty (aluminum) can weighs 12.5 g. A can contains 12.0 oz of soda. The specific heat of aluminum is 0.902 J/g C; take that of soda to be 4.10 J/g C. (a) How much heat must be absorbed from the six-pack to lower the temperature from 25.00 to 5.00C? (b) How much ice must be melted to absorb this amount of heat? (Hfus of ice is given in Table 8.2.)
When a vapor condenses into a liquid: a.it absorbs heat. b.it generates heat. c.its temperature rises. d.its temperature drops.
If it takes 654 J of energy to warm a 5.51-g sample of water, how much energy would be required to warm 55.1 g of water by the same amount?
A 45-g aluminum spoon (specific heat 0.88 J/g C) at 24 C is placed in 180 mL (180 g) of coffee at 85 C and the temperature of the two become equal. (a) What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water. (b) The first time a student solved this problem she got an answer of 88 C. Explain why this is clearly an incorrect answer.
How much heat, in joules and in calories, must be added to a 75.0g iron block with a specific heat of 0.449 Jig C to increase its temperature from 25 C to its melting temperature of 1535 C?
How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from 23.0 C to 1.0 C?
Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
During a recent winter month in Sheboygan, Wisconsin, it was necessary to obtain 3500 kWh of heat provided by a natural gas furnace with 89% efficiency to keep a small house warm (the efficiency of a gas furnace is the percent of the heat produced by combustion that is transferred into the house). (a) Assume that natural gas is pure methane and determine the volume of natural gas in cubic feet that was required to heat the house. The average temperature of the natural gas was 56 F; at this temperature and a pressure of 1 atm, natural gas has a density of 0.68 1 g/L. (b) How many gallons of LPG (liquefied petroleum gas) would be required to replace the natural gas used? Assume the LPG is liquid propane [ C3H8 : density, 0.5318 g/mL; enthalpy of combustion, 2219 Id/mo for the formation of CO2(g) and H2O(l) ] and the furnace used to burn the LPG has the same efficiency as the gas furnace. (c) What mass of carbon dioxide is produced by combustion of the methane used to heat the house? (d) What mass of water is produced by combustion of the methane used to heat the house? (e) What volume of air is required to provide the oxygen for the combustion of the methane used to heat the house? Air contains 23% oxygen by mass. The average density of air during the month was 1.22 g/L. (f) How many kilowatt—hours ( 1kWh=3.6106 J) of electricity would be required to provide the heat necessary to heat the house? Note electricity is 100% efficient in producing heat inside a house. (g) Although electricity is 100% efficient in producing heat inside a house, production and distribution of electricity is not 100% efficient. The efficiency of production and distribution of electricity produced in a coal-fired power plant is about 40%. A certain type of coal provides 2.26 kWh per pound upon combustion. What mass of this coal in kilograms will be required to produce the electrical energy necessary to heat the house if the efficiency of generation and distribution is 40%?
9.90 Many engineering designs must incorporate ways to dissipate energy in the form of heat. Water evaporators are common for this task. (a) What property of water makes it a good material for evaporators? {b} If an application could not use water, hut instead was forced to use a material with a value for the property in part (a) that was one half that of water, what changes would need to be made in the design?