Suppose your favorite TV scientist has equal masses of frozen water (ice) and liquid water. If she decides to cause both substances to go through a phase change to a phase with more energy (ice to water, water to steam), which substance will require more energy tochange phases? The latent heat of fusion for water is Lf,water-3.33. 105, and the latent heat of vaporization for water is Ly,water-2.26. 106kgkgO Changing liquid water to steam requires more energy.O They require the same amount of energy.O Changing ice to liquid water requires more energy.Select true or false for the following statements.✓Vaporization is when a substance goes from a gas to a liquid.✓ The temperature of a substance does not change during a phase change.|---✓ It always takes the same amount of energy to change a substance from solid to liquid as it does to change it from liquid to gas.✓ A substance can exist in two different states of matter at the same temperature.✓ The negative sign in the equation Q=± mL represents when thermal energy is being taken away from a substance during a phase change.✓ The temperature of a substance changes during a phase change.

Latent Heat of Fusion is the amount of energy that is needed to Convert a solid into a liquid form. Latent Heat of Vaporization is the amount that is needed to convert a liquid into a gaseous form. We can determine the energy required for phase change using the relation between energy and latent heat of fusion or Latent heat of Vaporization. Q = m∆H Where Q = Energy m = mass ∆H = Latent heat of Vaporization or fusionIt is given that both has same mass, Therefore Consider mass "m" kg . Energy required to convert frozen ice into water (Q) = m x 3.3 x 105 J Energy required to convert water into steam (Q) = m x 2.26 x 106 J It is clear that Energy required to convert water into steam is more than the energy required to convert frozen ice into water. Therefore Option A is correct.

Science

Chemistry

Suppose your favorite TV scientist has equal masses of frozen water (ice) and liquid water. If she decides to cause both substances to go through a phase change to a phase with more energy (ice to water, water to steam), which substance will require more energy to change phases? The latent heat of fusion for water is Lf,water 3.33. 105, and the latent heat of vaporization for water is Lv,water 2.26. 106 O Changing liquid water to steam requires more energy. kg O They require the same amount of energy. O Changing ice to liquid water requires more energy.

Suppose your favorite TV scientist has equal masses of frozen water (ice) and liquid water. If she decides to cause both substances to go through a phase change to a phase with more energy (ice to water, water to steam), which substance will require more energy to change phases? The latent heat of fusion for water is Lf,water 3.33. 105, and the latent heat of vaporization for water is Lv,water 2.26. 106 O Changing liquid water to steam requires more energy. kg O They require the same amount of energy. O Changing ice to liquid water requires more energy.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.0 g, and its initial temperature is –11.2 °C. The water resulting from the melted ice reaches the temperature of his skin, 29.2 °C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.
A 50.5 g sample of quartz is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The quartz sample starts off at 98.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 19.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits. J g. °C x10 X S thermometer. insulated container water sample a calorimeter ? ola
To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 12.7 g,12.7 g, and its initial temperature is −14.4 ∘C.−14.4⁢ ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.8 ∘C.29.8⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. q= J
Ices] A 21.0 g sample of pure iron at 85 °C is dropped into 66 g of water at 20. °C. What is the final temperature of the water-iron mixture? The specific heat of water is 4.184 J/g °C. The specific heat of iron is 0.45 J/g °C. Final temperature °C
A gold coin whose mass is 8.47 g is heated to 138.9oC and then quickly dropped into an ice calorimeter. What mass of ice melts? (The amount of heat in an ice calorimeter is determined from the quantity of ice the melts, knowing that it takes 6.01 kJ of heat to melt exactly one mole of ice. Molar heat capacity of gold is 25.418 J/mol/K)
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
When 40.00 grams of fictional compound X is added to water to make 236.0 grams of solution, the temperature increases from 19.05 °C to 63.46 °C. What is the heat of solution for compound X (in kJ/mol) given that the molar mass of compound X is 73.87 g/mol. Assume the specific heat capacity of the solution is 4.18 J/g°C.
How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.
Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
What is the heat capacity of 2.63 mol of liquid water? How many kJ of heat are needed to raise the temperature of 2.60 kg of water from 41.1 oC to 70.9 oC?
Duncan knows that it takes 36400 cal of energy to heat a pint of water from room temperature to boiling. However, Duncan has prepared ramen noodles so many times he does not need to measure the water carefully. If he happens to heat 0.750 pint of room-temperature water, how many kilojoules of heat energy will have been absorbed by the water at the moment it begins to boil?
Please fill in the four blanks. Thank you!