What is the specific heat capacity of the ice water mixture, the specific heat capacity of water and

The ice-water mixture absorbs a lot of heat in the melting process, the temperature does not rise, and the absorbed heat is not used to heat up, but is used in melting, because ice melting needs to absorb heat, as long as there is ice, the heat will be absorbed by the ice, until the ice is completely melted and completely turned into water, and the heat absorbed can make the water heat up, which is such a process.

Not because the specific heat capacity of water is greater, but because the heat is absorbed by the ice.

The temperature of the ice-water mixture is specified in physics as 0 degrees, and there is no heat transfer between ice and water. Ice water mixture: Ice absorbs other heat as it melts, and the specific heat capacity of the ice is the specific heat capacity.

The ice is gradually melting, the water level remains the same, and the temperature of the ice-water mixture remains at zero degrees Celsius until the ice melts completely.

The premise that the water level does not change is that the ice floats in the water with a clear surface, and it is not like a glass of shaved ice. ）

Kilograms of joules.

On the first floor, I don't agree with the fact that the specific heat capacity of solid liquids is related to their specific heat capacity for endothermic or exothermic as they change from each other. The heat absorption and exothermia of gases and solid-liquid conversion is related to their molecular spacing. The essence of hot melt is the combined effect of molecular potential energy and the strength of motility.

Pyroke kilograms Celsius dui de believe me.

What is the specific heat capacity? Do you calculate? How do you count without numbers? The topic is not clear, and it stumped me, the representative of the physics class, hehe.

The specific heat capacity of water is: 4200J (kg..)The specific heat capacity of ice is: 2100 J (kg.).℃)

When the specific heat capacity of water is 25, it is about higher than that of other liquids, and ice is half of the specific heat capacity of water, so the specific heat capacity of water is greater. The molecular structure of ice is stable relative to that of water, and the rate of motion between particles is ratioWater moleculesThe rate of motion is low, so the specific heat capacity of ice is smaller than that of water.

Specific heat capacity, referred to as specific heat, is also known as specific heat capacity.

It's thermodynamics. is a commonly used physical quantity.

Indicates the ability of an object to absorb heat or dissipate heat. The greater the specific heat capacity, the greater the ability of the object to absorb heat or dissipate heat. It refers to the amount of heat absorbed or released by a large circle as a unit mass of a substance rises or falls at a unit temperature.

Different substances have different specific heat capacities, and the specific heat capacity is a property of the substance, so it is possible to roughly identify different substances by the difference in specific heat, but it should be noted that some substances are quite close to the specific heat.

The specific heat of the same substance generally does not change with the change of mass and tumbling shape, and for the same substance, the specific calorific value.

Related to the state of matter, the specific heat of the cavity pants of the same substance in the same state is certain (ignoring the influence of temperature versus heat), but the specific heat is not the same in different states.

There is also a small change in specific heat capacity when the temperature changes, but it is generally negligible. The specific heat values given in the specific heat capacity table are the average values of these substances at room temperature.

The specific heat capacity of the gas and the thermal expansion of the gas are closely related, and they are different when the volume is constant and the pressure is constant, so there are two concepts of the specific heat capacity of the constant volume and the specific heat capacity of the constant pressure, but for the solid and the liquid, the difference between the two is very small, and it is generally no longer distinguished.

The reason why water melts into ice is because it releases heat, but the mass of the water does not change, so the heat capacity at the same mass is greater than that of ice. Therefore, the specific heat capacity of water is naturally greater than that of ice.

The intermolecular force (van der Waals force) depends on the molecular spacing, and the change of state of matter (which is a physical change) is to destroy the effect of van der Waals force. The volume of the same amount of water is less than that of ice (the volume ratio is about 10 to 11), so the intermolecular distance of ice is greater than that of water, and the specific heat capacity of ice is less than that of water.

Common units: j (kg· )j (g· )kj (kg· )cal (kg· )kcal (kg· )etc. Note that Celsius and Kelvin differ only in the representation of the temperature scale, and are equivalent in the sense of the magnitude of the temperature difference, so that and k in these units can be arbitrarily substituted with each other. For example, "joules per kilogram Celsius" and "joules per kilogram open" are equivalent.

The specific heat capacity of water is: 4200J (kg..)℃)

The specific heat capacity of ice is: 2100 J (kg.).℃)

The spacing between liquid molecules is much greater than that between solid molecules, and the intermolecular force (van der Waals force) depends on the molecular spacing. At the same time, the change of state of matter (which is a physical change) is to destroy the effect of van der Waals forces. Therefore, ice needs to absorb more energy for physical changes, and its specific heat capacity is much greater than that of water on a macroscopic scale.

The question you ask is like the difference between the volume of the same water and the ice, because the specific heat capacity of the state change is also changing.

Because it is more important to consider state changes than heat capacity.

The specific heat capacity of ice is: 2100 J (kg.).℃)

Specific heat capacity refers to the amount of heat required to increase the temperature of 1kg of homogeneous material by 1k when there is no phase change and chemical change.

Using the concept of specific heat capacity, it is possible to deduce a molar heat capacity that represents the amount of heat required to raise 1 k of a mol of substance. And the molar heat capacity cp under isobaric conditions is called constant pressure molar heat capacity. The molar heat capacity CV under isochoric conditions is called the constant volume molar heat capacity.

He usually correlates the relationship between the molar heat capacity of constant pressure and temperature as a polynomial.

The specific heat capacity of a substance is related to the process undertaken. Commonly used in engineering applications is the specific heat capacity of constant pressure.

There are three types: CP, specific heat capacity CV and specific heat capacity in saturated state.

Constant pressure specific heat capacity cp: It is the energy absorbed or released by a unit mass of a substance under the condition that the pressure is constant, and the temperature rises or falls by 1 or 1K.

The specific heat capacity of the jujube is the energy absorbed or released by 1 or 1k of a unit mass of a substance under the condition that the volume (volume) remains unchanged.

Specific heat capacity in saturated state: It is the amount of heat absorbed or emitted by a unit mass of a substance when the temperature rises or falls by 1 or 1 k in a certain saturated state.

It shows that the temperature of 1kg of ice rises or decreases, and the amount of heat that needs to be absorbed or released is.

Ice is made up of water molecules.

Crystals formed by orderly arrangement, water molecules are joined together by hydrogen bonds to form a very "open" (low-density) rigid structure.

The spacing between the O—O nuclei of the nearest water molecule is about 109°, which is very close to the ideal tetrahedron.

The bond angle is 109°28. However, the O-O spacing of each water molecule that is only adjacent and not directly bound is much larger, and the farthest one should be reached. Each water molecule can combine with 4 other water molecules to form a tetrahedral structure, so the coordination number of the water molecule is 4.

Ice is a colorless and transparent solid, a product formed by liquid solidification, condensed by cold and frozen environment, and liquefied and dissolved by high temperature, which is a normal natural phenomenon, which can be formed naturally or artificially made.

Hydrogen bonds are mainly used to interact with each other, but van der Waals forces are also present.

The lattice structure is generally hexagonal, and its density is less than that of water. However, there can also be other lattice structures at different pressures.