# Explain why the potential energy increases when ice starts to melt and becomes liquid water. My answer is, While the ice melts kinetic energy is being added to the particles. This breaks the bond and causes a change of state

86,693 results
1. ## Science

1: Use the table to answer the question. Student Name | Potential Energy Rating (lowest to highest) ------------------------------------------------------------------------------------- Henry | gas, liquid, solid

2. ## Physical Science

Ice melts in the water while remaining at 0 degrees Celsius. Which energy changes occur as it melts? (1 point) A. The kinetic energy of the molecules will increase, and the potential energy remains the same. B. Both the kinetic and potential energy will

3. ## Science 8

1. A bottle of water is taken out of a refrigerator and put on a kitchen table. As the bottle of water warms up, what happens to the particles in the water? a The average kinetic energy of the particles increases. *** b The average temperature of the

4. ## Thermal ENERGU UNIT TEST

1.In which case would the kinetic energy of particles be increasing? ANSWER: Metal is heated from room tempature to 200C 2.Water boils at 100°C and turns into steam. Which similarities or differences are there between water at 100°C and steam at 100°C?

5. ## ELA

A student adds ice to several samples of water. The results are shown in the table. Which conclusion can be drawn from the results? (1 point) As the amount of ice added increases, the change in temperature increases. As the amount of ice added increases,

6. ## Chemistry

22.) The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/gC. (1) What quantity of heat is required to melt 25.0 g of ice at 0C? (2) What quantity of

7. ## physics

A 40-g block of ice is cooled to −71°C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 27°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts,

8. ## connexus chemistry

Help me check my work. Which statement accurately describes a type of potential energy found in a container full of a chemical substance in liquid form? The rotation of the particles is one place where potential energy is stored. The speed of the particles

9. ## Physics - ice to liquid

Fifty grams of hot water at 80oC is poured into a cavity in a very large block of ice at 0oC. The final temperature of the water in the cavity is then 0oC. Show that the mass of ice that melts is 50 g. To melt ice to 50g of water, I think that it will

10. ## Gifted and Talented Science

Ice is given thermal energy and begins to melt while remaining at the same temperature. Which changes happen to the molecules of water? (1 point) A. The molecules will have more potential energy because of their arrangement. B. The molecules will have a

11. ## Chem

joules needed to melt 30.0 g of ice at 0 ∘C and to warm the liquid to 60.0 ∘C so i did Q=mFf which i set up like 30.g x 334 j/c = 10020 J then i'm sorta confused what i'm doing next. explain in detail please?

12. ## Physics

Take two Styrofoam cups, partially fill them with equal amounts of cold water, and drop equal amounts of ice into each cup to obtain a mixture of ice and water. a. Stir the water and ice mixture in one of the cups vigorously with a nonmetallic stirrer

13. ## science

1) Read the scenario. A car starts 10 m north of a reference point. It moves at a constant velocity over the next 5 s, reaching a position of 10 m south of the reference point. What is the car’s average velocity? 0 m/s 4 m/s north 2 m/s south 4 m/s south

14. ## College Chemistry

Using the values for the heat of fusion, specific heat of water, or heat of vaporization, calculate the amount of heat energy in each of the following: * calories removed to condense 125g of steam at 100 degree C to cool the liquid to 15 degree C * joules

15. ## Physics

Occasionally, huge icebergs are found floating on the ocean's currents. Suppose one such iceberg is 114 km long, 31.3 km wide, and 194 m thick. (a) How much heat in joules would be required to melt this iceberg (assumed to be at 0 °C) into liquid water at

16. ## science

Explain why the potential energy increases when ice starts to melt and becomes liquid water. My answer is, While the ice melts kinetic energy is being added to the particles. This breaks the bond and causes a change of state making the solid become a

17. ## physics

A 2.5 kg block of ice at a temperature of 0.0 degrees Celcius and an initial speed of 5.7 m/s slides across a level floor. If 3.3 x 10^5 J are required to melt 1.0 kg of ice, how much ice melts, assuming that the initial kinetic energy of the ice block is

18. ## chemistry

When ice at 0C melts to liquid water at 0C, it absorbs 0.334 kj of heat per gram. Suppose the heat needed to melt 31.5 g of ice is absorbed from the water contained in a glass. If this water has a mass of .210 kg and a temperature of 21.0C, what is the

19. ## Chemistry

Which of the following statements correctly describes the change which occurs when a liquid vaporizes at its boiling point at a given external pressure. a) The entropy decreases b) The temp increases c) The kinetic energy increases d) The potential energy

20. ## Chemistry

Which of the following reactions is exothermic? 1. Na(s) --> Na(g) 2. Na(g) --> Na+ + e- 3. Cl2(g) --> 2Cl(g) 4. Cl(g) + e- --> Cl-1 My guess is 4, but I'm not sure Here is what you do. For 1, do we think it will take energy to change Na as a solid to Na

21. ## Physics

The question is: "A block of ice at 0oC is dropped from a height that causes it to completely melt upon impact. Assume that there is no air resistance and that all the energy goes into melting the ice. Show that the height necessary for this to occur is at

22. ## Science

Which of the following procedures increases the average kinetic energy of the molecules in a beaker of water. 1. heating water from 0 degrees C to 100 degrees C. 2. Cooling steam at 100 degrees C to ice at 0 degrees C. 3. Changing ice at 0 degrees to

23. ## Chemistry

Identify which of the following changes is exothermic. a) liquid water boils to steam b) liquid water freezes to give ice c) ice melts to give liquid water d) liquid water increases in temperature from 35 C to 45 C

24. ## Physics

1) Let's consider an ice cube has the volume of 20 mL. The density of ice is 0.9 g/mL. What is the mass of the ice cube? My answer: 0.9 * 20= 18gr We would now like to calculate the total energy that is required to heat up this piece of ice from -196˚C to

25. ## chemistry

The freezing of water at 0⁰C can be represented as follows: H2O (l) ↔ H2O(s) The density of liquid water is 1.00 g/cm3. The density of ice is 0.92 g/cm3. explain why applying pressure causes ice to melt.

26. ## Physical Science

Which of the following statements about ice melting is true? A. Energy flows from the ice to its surroundings. B. Water molecules move from their fixed position. C. Water molecules lose energy. D. The temperature of the ice increases as it melts. I think

27. ## Physical Science

An ice cube tray full of water is put into a freezer. Which energy change occurs in the particles in the water as it undergoes a phase change from a liquid to a solid? 1. The potential energy increases due to the tighter arrangement of the particles. 2.

28. ## chemistry

Calculate the enthalpy change when 50. g of ice at -30.0 °C is heated to completely melt to liquid water at 0.0°C. (The heat of fusion for water is 333 J/g.)

29. ## science

A ball sitting on the top of a table has potential energy but no kinetic energy. How do potential and kinetic energy change as the ball falls off the table to the floor? A. Its potential energy increases, and its kinetic energy decreases. B. Its potential

30. ## Chemistry

When ice at 0°C melts to liquid water at 0°C, it absorbs 0.334 kJ of heat per gram. Suppose the heat needed to melt 30.7 g of ice is absorbed from the water contained in a glass. If this water has a mass of 0.189 kg and a temperature of 21.0°C, what is

31. ## Chemistry - Energy: Phase Changes

If 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius, how much water at 0 degrees Celsius is produced? How much ice is left? The molar heat of melting is 6.01 kJ/mol. So... 6.01 kJ -> 1 mol (6.01 kJ of energy can melt 1 mole of ice)

32. ## Chemistry

A 100g sample of ice at 0ºC is added to 150.0 mL of liquid water at 80ºC in a styrofoam cup calorimeter. (The specific heat capacity of water is 1.184 J/g•ºC, the density of water is 1.00 g/mL, and ∆Hºfus = 6.01 kJ/mol) a) Does all of the ice

CHECK MY ANSWERS PLEASE 1.When an exothermic phase change occurs, such as freezing water into ice crystals, where does the energy released go? my answer: into the surroundings and the environment 2.When a flashlight battery runs out of energy (charge) does

34. ## Physics

If a cup is half full of ice, how long will it take to melt the ice in a microwave oven (1000 W) set on high? Also, if you did the above but added 100ml of ice cold water to the ice would this change the results of melt time?

35. ## physics

A 2.6 kg block of ice at a temperature of 0.0C and an initial speed of 5.3 m/s slides across a level floor. If 3.3 × 105 J are required to melt 1.0 kg of ice, how much ice melts, assuming that the initial kinetic energy of the ice block is entirely

36. ## Science "HELP"!

Passage:The particles of matter are in constant motion. The energy of motion is called kinetic energy, so the particles of matter have kinetic energy. As matter becomes warmer, its particles move faster. As a result, their kinetic energy increases.

37. ## Chemistry

Consider the reaction of Lithium with water: 2 Li(s) + 2H2O(l) ----> 2 LiOH(aq) + H2(g) The delta H of the reaction is -160 KJ The enthalpy of fusion of H2O is 6.0 kJ/mol The specific heat capacity of H2O(l) is 4.18 J/gC When 10 grams of Li(s) is dropped

38. ## chemistry

When water freezes and becomes solid ice, the hydrogen bonds create a crystal structure and there is fixed space between each water molecule. This causes ice to? a.become more dense than liquid water because it is a solid* b.become less dense than liquid

39. ## Science

Consider which is not an example of how an object gains elastic potential energy by stretching is a trampoline part In what form are all potential energy the same What is making an ice block to melt Describe three forms of energy Imagine that you push on a

40. ## Science

15)Which of the following shows the correct sequence of what happens to the water molecules in an ice cube when it is removed from the freezer? 1. the molecules gain enough energy to break free from each other. 2. the ice begins to melt 3. the molecules

41. ## Chemistry

An 850 gram chunk of ice at 0 degrees Celsius is dropped into a container holding 1.7 kg of water at an initial temperature of 35 degrees Celsius. Due to the presence of the ice, the temperature of the water eventually drops to 0 degrees Celsius. Show a

42. ## science

A ball sitting on the top of a table has potential energy but no kinetic energy. How do potential and kinetic energy change as the ball falls off the table to the floor? A. Both its potential energy and its kinetic energy decrease. B. Both its potential

43. ## Science

TRUE or FALSE? when ice cubes melt into liquid water, its physical properties changes

44. ## Physics

A 2.5 kg block of ice at a temperature of 0C and an initial speed of 5.7 m/s slides across a level floor. If 3.3*10^5 J are required to melt 1.0 kg of ice, how much ice melts, assuming that the initial kinetic energy of the ice block id entirely converted

45. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

46. ## physics

The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 7.40 g of condensation forms on a glass containing water and 210 g of ice, how many grams will melt as a result? Assume no other heat transfer

47. ## Physics

Lake Erie contains about 4.8 x 10^17 grams of fresh water. Assume that the lake has frozen solid and that the ice starts off at -3 C. How much energy would the lake need to absorb from the Sun to cause it to evaporate completely? Each gram of water will

48. ## physics

In 1986 a gargantuan iceberg broke away from the Ross Ice Shelf in Antarctica. It was approximately a rectangle 160 km long, 45.0 km wide, and 250 m thick. (a) What is the mass of this iceberg, given that the density of ice is 917 kg/m3? (b) How much heat

49. ## physics

a 75kg skater is travelling at 15m/s stops suddenly on the ice. If the ice is at 0 degrees and it is assumed that all of the skaters energy is converted to heat, how much ice does he melt? (latent heat of fusion for water is 3.3x10^5 J/kg)

50. ## physics

If you drop a piece of ice on a hard surface, the energy of impact will melt some of the ice. The higher it drops, the more ice will melt upon impact.Find the height from which a block of ice should ideally be dropped to completely melt it that falls

1.When an exothermic phase change occurs, such as freezing water into ice crystals, where does the energy released go? my answer: into the surroundings and the environment 2.When a flashlight battery runs out of energy (charge) does that mean the energy

52. ## Chemistry

Please check my answers: 1.When an exothermic phase change occurs, such as freezing water into ice crystals, where does the energy released go? my answer: into the surroundings and the environment 2.When a flashlight battery runs out of energy (charge)

-Steam at 100 ¡ãC is mixed with 166.4 g of ice at ¨C32.8 ¡ãC, in a thermally insulated container, to produce water at 44.6 ¡ãC. Ignore any heat absorption by the container. -Cwater = 4186. J/(kg ¡ãC) -Cice = 2090. J/(kg ¡ãC) -Lf,water = 3.33

54. ## Science

Can you please help me figure out why evaporation is a cooling process and why becoming a solid is a heating process? evaporation absorbs heat from the environment, thus "cooling" the environment. becoming solid is a heating process as heat is moved from

55. ## Chemistry

The question on one of my assignments says, "Explain why a thick layer of ice on the lake can support the weight of a person, but the liquid water cannot." I would assume it's because solids are solid and liquids are liquid, but I feel like they want a

56. ## CHEMISTRY

If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at -27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted? given

57. ## Heat and properties of matter

1. Which of the following is not true a. Evaporation occurs at any temprature of a liquid b. Boiling takes place only at the surface of the liquid c. Evaporation occursonly at the surface of a liquid d. Boiling of a liquid takes place at a definite

58. ## Chemistry HEAT OF FUSION

What amount of energy is required to melt a 26.9 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg-1 Heat required to melt the ice = J What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC? Specific heat of

59. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

60. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

61. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

62. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

63. ## Melting Ice Chemistry

You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B.

64. ## Physics

A 0.0475 kg ice cube at −30.0°C is placed in 0.577 kg of 35.0°C water in a very well insulated container. The latent heat of fusion of water is 334 kJ/kg, the specific heat of ice is 2092 J/(kg · K), and the specific heat of water is 4184 J/(kg · K).

65. ## physics

The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 8.80 g of condensation forms on a glass containing water and 170 g of ice, how many grams will melt as a result? Assume no other heat transfer

66. ## physics

The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 8.80 g of condensation forms on a glass containing water and 170 g of ice, how many grams will melt as a result? Assume no other heat transfer

67. ## physics

The Weistin Stamford Hotel in Detroit is 228 m tall. Suppose a piece of ice which initially has a temperature of o degrees celcius falls from the hotel roof and crashes to the ground. Assuming that 50% of the ices mechanical energy during the fall and

68. ## physics

A piece of ice its mass is 2.5 kg and at 0.0 C temperature , it is crawling on the ground with 5.7 m/s , what is the mass of the melted ice , if we know all of the kinetic energy of the ice turn into the internal energy (of the ice ) , that we need 3.3 X

A 0.106 kg ice cube is taken out of a freezer with temperature -16°C. It is then added to a glass of water with mass 0.25 kg. The water initially has a temperature of 24.2 °C. Assume no heat is added or lost to the surroundings. Calculate the amount heat

70. ## physics

Suppose 300 g of water at 20°C is poured over a 50-g cube of ice with a temperature of -6°C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the water–ice mixture reaches

71. ## Physics repost - need more explanation

Posted by Ceres on Wednesday, September 23, 2009 at 4:07pm. The question is: "A block of ice at 0oC is dropped from a height that causes it to completely melt upon impact. Assume that there is no air resistance and that all the energy goes into melting the

72. ## chemistry

Couze The water in the buket has some energy (tempreture) it is absorbed by the water and the ice melts this way water cools...now if you consider the ice outside the bucket water will no longer be in tuch with ice ,since energy of water since must be

73. ## Physics

50 grams of ice cubes at -5oC is added to a 1 litre (1 kg) of water that is initially at 30oC. a) Use the table of values to find the energy needed to melt the ice:(energy to raise the temperature of the ice to 0oC+ change the state of the ice to water) b)

74. ## Chemistry

A 2.75 kg block of ice is heated until it completely melts. It is then heated again until it completely changes to water vapor. Is more energy required to melt the ice or to vaporize the liquid water.

75. ## Physics-

-Steam at 100 ¡ãC is mixed with 166.4 g of ice at ¨C32.8 ¡ãC, in a thermally insulated container, to produce water at 44.6 ¡ãC. Ignore any heat absorption by the container. -Cwater = 4186. J/(kg ¡ãC) -Cice = 2090. J/(kg ¡ãC) -Lf,water = 3.33

76. ## Science

These are some more questions, they're not multiple answers they're S.A so the questions will be first and my answers will be on the bottom. 17. Describe the difference between thermal energy and temperature. Use the following words to help structure your

77. ## Science

Wil kinetic energy increase or decrease based on the amount of potential energy it starts with?? If potential energy is lost, KEnergy increases. Potential Energy + kinetic energy= constant.

78. ## Jake

If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at -27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted? given

79. ## Survey of the Sciences

Thank you Damon! now, here's the last part of that along with the first again.... Calculate the height from which a block of ice at zero degrees celcius nust be dropped for it to completely melt upon impact. Assume that there is no air resistance and that

80. ## Physical Science

The sun's energy melts part of a glacier of ice at 0 degrees Celsius. The sun supplies 880 kilocalories to a big glacier of ice at 0 degrees Celsius. How many kilograms of ice will melt into liquid water at 0 degrees Celsius?

81. ## Physical Science

The sun's energy melts part of a glacier of ice at 0 degrees Celsius. The sun supplies 880 kilocalories to a big glacier of ice at 0 degrees Celsius. How many kilograms of ice will melt into liquid water at 0 degrees Celsius?

82. ## physics

The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 8.00 g of condensation forms on a glass containing both water and 200 g of ice, how many grams of the ice will melt as a result? Assume no other

83. ## Chemistry

What total energy must be absorbed (from the environment) to change 1.00kg of ice at -30.0°C on a lake surface in February to water at 20.0°C in August? Add the following heats.. heat ice from -30 to OC melt ice at 0C heat water from 0C to 20C

84. ## Chemistry

What amount of energy is required to melt a 27.4 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg-1 Heat required to melt the ice 9.12e3 = J What amount of energy must be removed from 123 g of water to cool it from 71.6oC to 9.41oC? Specific heat

85. ## Chemistry U3 Sample work

Hello, does anyone know the answers to these application questions from the U3 Chemistry Sample Work?? 1. The human body uses catalysts called enzymes to lower the activation energy of some reactions required for life. What is one way that the use of

86. ## Physics

Suppose 100 g of water at 20°C is poured over a 70-g cube of ice with a temperature of -8°C. If all the ice melts, what is the final temperature of the water? If all of the ice does not melt, how much ice remains when the water–ice mixture reaches

87. ## physics

The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 7.40 g of condensation forms on a glass containing water and 210 g of ice, how many grams will melt as a result? Assume no other heat transfer

88. ## Physics-is this correct?

Lake Erie contains about 4.8 x 10^17 grams of fresh water. Assume that the lake has frozen solid and that the ice starts off at -3 C. How much energy would the lake need to absorb from the Sun to cause it to evaporate completely? Each gram of water will

89. ## Physics

Lake Erie contains about 4.8 x 10^17 grams of fresh water. Assume that the lake has frozen solid and that the ice starts off at -3 C. How much energy would the lake need to absorb from the Sun to cause it to evaporate completely? Each gram of water will

90. ## Chemistry

Calculate the enthalpy change when 45 g of ice at -40.0 oC is heated to completely melt to liquid water at 0.0oC. (The heat of fusion for water is 333 J/g.)

91. ## Physics

Lake Erie contains about 4.8 x 10^17 grams of fresh water. Assume that the lake has frozen solid and that the ice starts off at -3 C. How much energy would the lake need to absorb from the Sun to cause it to evaporate completely? Each gram of water will

92. ## science

Which provides more cooling for a Styrofoam cooler, one with 10lb of ice at 0C or one with 10lb of ice water at 0C? Explain your reasoning. 10# ice requires heat to melt the ice + heat to heat the water after it melts. 10# ice water requires heat to heat

93. ## physics

In 1986 a gargantuan iceberg broke away from the Ross Ice Shelf in Antarctica. It was approximately a rectangle 160 km long, 45.0 km wide, and 250 m thick. (a) What is the mass of this iceberg, given that the density of ice is 917 kg/m3? (b) How much heat

94. ## Physics

divide both sides of the equation by mass, it divides out. mass*HeatFusion=mass*gh How do you calculate the height that a block of ice at 0°C must be dropped to completely melt upon impact. Assume that all of the initial gravitational potential energy of

95. ## physics

There is a great deal of ice floating on the ocean near the north pole. If this ice were to melt due to global warming, what would happen to the level of the oceans? A.Rise B.Fall C.Remain the same water is slightly more dense than water, but when the ice

96. ## Physics

Calculate the height that a block of ice at 0°C must be dropped to completely melt upon impact. Assume that all of the initial gravitational potential energy of the block goes into melting the ice. Hmmmm. http://www.jiskha.com/display.cgi?id=1162768243

97. ## Physics

Lake Erie contains about 4.8 x 10^17 grams of fresh water. Assume that the lake has frozen solid and that the ice starts off at -3 C. How much energy would the lake need to absorb from the Sun to cause it to evaporate completely? Each gram of water will

98. ## CHEMISTRY

IF you add ice at zero degrees celcius to a container of water maintained at 0degrees, the ice wil float on the water with that water finding a certain level in the container. As the ice melts, forming liquid at zero degrees, would you expect the water

99. ## Astronomy

Io gets most of its heat flow from tidal pulling and pushing as it orbits Jupiter. Europa also orbits Jupiter and gets quite a bit of tidal pulling. The heat flow on Europa is around 100 times less than that on Io. The latent heat of melting from solid ice

100. ## physics

A 40-g block of ice is cooled to −71°C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 27°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts,