The specific latent heat will not change with a change of scale.

The latent heat of vaporization of water is 2260 × 103 J/kg. Answer: The phenomenon of the trapping of infrared radiations of long wave length being radiated to space by greenhouse gases like carbon dioxide (CO2), methane (CH4), nitrous oxide (N2O) to keep the environment warm at the planet’s surface and the lower atmosphere is called greenhouse effect. What amount of heat is withdrawn? Hence, if they do not put on extra clothes, they are likely to catch cold. When it is allowed to solidify at the same temperature, it gives out 75000 J of heat. The compressed gas is transferred to the top of the hot vessel where it percolates down through the gravel, transferring its heat to the rock and cooling to ambient temperature. Solution: Question 15: Calculate the total amount of heat required to convert 100g ice at 0°C to steam at 100°C. (g = 10 ms-2; Specific heat capacity of water = 4200 J / kg°C) Solution: If the whole of the energy due to fall of water changes into heat energy, and 0°C be the rice in the temperature of water, then. The system uses the reaction energy created when salts are hydrated or dehydrated. Answer: According to the principle of calorimetry, if two bodies at different temperatures are mixed together (or kept in contact), heat flows from a body at higher temperature to a body at lower temperature till both the bodies attain the same temperatue. Answer: The measurement of the quantity of heat is termed as colorimetry. It works by storing heat in a container containing 50% sodium hydroxide (NaOH) solution. Question 20: Explain, Why is it advisabile to pour cold water over burns, caused on human body, by hot solids? Solution: Heat released by 5 kg of steam at 100°C to convert into water at 100°C. (ii) Burning of forests and deforestations. Give reason for this observation.

In pumped-heat electricity storage (PHES), a reversible heat-pump system is used to store energy as a temperature difference between two heat stores.[39][40][41].

Water at −10 °C (ice) solid: 2.05: 38.09: 1.938: 1.53 R Zinc: solid: 0.387: 25.2: 2.76: 3.03 R … Solution: Question 16: Steam at 100°C is passed over 1000 g of ice at 0°C.

The observations recorded are: If L j/gm be the specific latent heat of fusion of ice and sc be the specific heat capacity of copper, then: Question 1: The temperature of a lead piece of mass 400 g rises from 20°C to 50°C when 1560 J of heat is supplied to it. U.S. Pat. The contents of the calorimeter are well stirred and its final highest temperature is recorded to be 28 °C. It means that we need 2260 × 103 J of heat to convert 1 kg of water at its boiling point into steam.

Question 61: Why are athletes advised to put on extra clothes after competing on event? If the specific heat capacity of water is 4.2 J/g°C and of copper is 0.4 J/g°C, find: (i) the heat gained by water, (ii) the heat gained by calorimeter, (iii) total heat supplied by the metal piece, and (iv) the specific heat capacity of metal. What is its specific heat capacity in S.I. Answer: During the state change heat supplied increases potential energy of molecules as distance between molecules increases work is done by heat supplied against attractive force.

It follows that that ice-cream, at 0°C, will draw more heat (about 340 joule more per gram) from burbody than water at 0°C. Answer: (i) Calorie: It is the quantity of heat required to raise the temperature of 1 gm of water by 1°C (more accurately the rise in temperature is taken from 14.5°C to 15.5°C). The amount of heat added to this substance and the temperature of the substance are plotted on the following graph:  If the specific heat capacity of the solid substance is 500 J/kg °G, find from the graph, (i) the mass of the substance. The energy is recovered as electricity by reversing the cycle.

Question 44: Bottled drinks are cooled more effectively, when surrounded by lumps of ice than iced water. It is also defined as the total kinetic energy possessed by all the molecules of a body. Answer: The heat required to convert 1 g of ice from 0°C to 1 g water at 0°C is 336J. The gas is then transferred to the bottom of the hot vessel to be reheated.

It follows that if s is more, Δθ will be small (for given values of H and m). In doing so, it absorbs large amount of heat from surroundings, hence temperature falls sharply. Solution: Question 11: A heater supplies heat at the rate of 800 J/s. It is quite appropriate, therefore, to regard specific heat capacity as a measure of thermal inertia. Thus, for a given body, its specific heat capacity determines the change in temperature produced by a given quantity of heat.

Question 3: Differentiate between heat and temperature. Question 6: State the condition for the flow of heat energy from one body to another. Give reason. (ii) a change in itsstate without any change in its temperature? Question 1: Explain briefly, how you would determine the specific heat capacity of a liquid? Hence, it is more effective in cooling than the ice-water. Historically, ice was transported from mountains to citie… Calculate the drop in temperature ignoring the heat capacity of the container. Calculate the specific heat capacity of the metal.

Question 60: Why water get cooled in a ‘Surahi’ in hot season? The heat, which can be derived from a solar collector on a rooftop, expels the water contained in the salt. Several applications are being developed where ice is produced during off-peak periods and used for cooling at a later time. heat capacity × rise in temperature = m × s × (θ2 – θ1).

How much heat is needed to warm it by 15°C?

Answer: Water has the maximum specific heat capacity. [47], Adsorption (or Sorption) solar heating and storage, Endothermic/exothermic chemical reactions. Answer: Heat is a form of energy, which when absorbed by a body makes it hot and when extracted from a makes it cold.

Question 11: Does the specific heat capacity of a substance depend upon its mass and rise in temperature only? Preparation and thermal performance of methyl palmitate and lauric acid eutectic mixture as phase change material (PCM).

Question 5: Will the value of specific heat’capacity and specific latent heat of a substance change if the scale is °F instead of °C? Thermal energy storage using ice makes use of the large heat of fusionof water.

= mL = 5 × 2268 KJ = 11440 kj. [20], One example of an experimental storage system based on chemical reaction energy is the salt hydrate technology. Question 34: Name the liquid which has the highest specific heat capacity. (ii) Intermolecular space increases. Question 39: State the principle of calorimetry. The solid chosen should be insoluble and non reactive with the liquid. Surplus heat generated by inefficiencies in the process is shed to the environment through heat exchangers during the discharging cycle. The substance A shows a greater rise in temperature. latent heat of fusion of 336,000 Jkg-1. Question 46: 1 kg of water freezes to form ice at 0°C. Question 2: What observation you will record and how will you determine the specific latent heat of fusion of ice? Answer: 22,60,000 J.

Only emails and answers are saved in our archive. Question 1: A piece of ice is heated at a constant rate. Then the mass of calorimeter with water and ice is again weighed. Question 1: A substance is in the form of a solid at 0°C. Question 15: Some hot water was added to three times its mass of cold water at 10°C and the resulting temperature was found to be 20°C.

Download Formulae Handbook For ICSE Class 9 and 10. Answer: The greenhouse effect contribute in trapping the sun’s heat energy within the atmosphere to maintain Earth’s surface at an average temperature of about 59°F (15°C) which is suitable for living human beings. In addition to using ice in direct cooling applications, it is also being used in heat pump based heating systems.

[46], Storing energy in molecular bonds is being investigated. These applications will - due to browser restrictions - send data between your browser and our server. Answer: The principle of calorimetry states: When a hot body is brought in contact with a cold body, heat passes from the hot body to the cold body till both attain the same temperature. When the water is added again, the heat is released, with almost no energy losses. [39][42], The developer claimed that a round trip efficiency of 72-80% was achievable. Question 52: What happens to the average kinetic energy of the molecules as ice melts at 0°C?

Under this high pressure, ice melts to form water below 0°C. Solution: Question 9: A vessel of negligible heat*capacity contains 40g of ice in it at 0°C, 8g of steam at 100°C is passed into the ice to melt it. Question 23: Explain, why is water used as a coolent in motor car radiators? Answer: Specific heat capacity ‘A’ 3.8 J/g/K. Google use cookies for serving our ads and handling visitor statistics. Question 69: What do you understand by the ‘latent heat of vaporization’ of a substance? The water so formed makes the surface water skating more slippery. It will also increase the rate of respiratory and Vector-borne disease infections like asthma and malaria respectively. Solution: Question 14: A piece of iron of mass 2.0 kg has a thermal capacity of 966 J/°C. A relatively small storage facility can hold enough ice to cool a large building for a day or a week. Answer: (i) The specific latent heat of fusion of ice is 3,36,000 J/Kg.

Please read Google Privacy & Terms for more information about how you can control adserving and the information collected. But in the process of melting, it takes comparatively longer time. Heat given = Heat Taken. Solution: m = 2.0kg, Thermal capacity = 966 J/°C. Saeed, R.M., Schlegel, J.P., Castano, C. and Sawafta, R., 2018. The observations are to be noted as below: Question 2: Describe a method to determine the specific heat capacity of a solid (say, a piece of copper). This heat is known as Latent heat. What is the S. I. unit of heat?

For example, air conditioning can be provided more economically by using low-cost electricity at night to freeze water into ice, then using the cooling capacity of ice in the afternoon to reduce the electricity needed to handle air conditioning demands. What was the temperature of the oven? Then initial temperature is noted. Answer: (i) AB part of the graph represents time in t seconds taken by ice at 0°C to convert into water at 0°C. In a temperate climate like that of the Netherlands, an average low-energy household requires about 6.7 GJ/winter. Question 10: Calculate the amount of heat released when 5.0 g of water at 20°C is changed into ice at 0°C. During night, land as well as sea radiates heat energy. This is because it is the heat needed to raise the temperature of a unit of the substance by one degree. Expression for the heat energy liberated by hot body = mcΔQ i.e.,         H = mcΔQ where m is mass, c is specific heat capacity, ΔQ is the change in temperature. Question 4: Discuss how high specific heat capacity of water helps in formation of land and sea breeze.

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