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Fullform of c g s

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Anonymous

15y ago
Updated: 5/23/2024

c Centimeter
g grams
s seconds

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How much heat is necessary to change 380 g of ice at -7C to water at 20C?

Heat is used in three stages 1. To rise the temperature of ice from -7 to 0 deg celsius 2. To change ice into water - melting 3. To rise temperature of water from 0 to 20 deg Celsius Hence Heat = 0.380*S*7 + 0.380*L+0.380*s*20 S - specific heat capacity of ice s- specific heat capacity of wate L= Laten heat of fusion of ice. Please get the data from data book, plug and find the heat needed


How much energy is required to raise the temperature of 3-g silver to 15 to 20?

The specific heat capacity of silver is 0.235 J/g°C. To raise the temperature of 3 g of silver by 5 °C (from 15 to 20°C), you would need 3 g x 5 °C x 0.235 J/g°C = 3.525 J of energy.


Heat of formation of water?

The heat of formation of water is the energy released or absorbed when one mole of water is formed from its elements in their standard states. For water, the heat of formation is -285.8 kJ/mol. This negative value indicates that the reaction is exothermic, meaning it releases energy.


What materials has the highest specific heat out of silver carbon sand alcohol?

Silver has the highest specific heat capacity among the materials listed (0.235 J/g°C), followed by alcohol (0.58 J/g°C), sand (0.84 J/g°C), and carbon (0.71 J/g°C).


How much heat is lost when 640 g piece of copper cools from 375 celsius to 26 celsius?

The amount of heat lost can be calculated using the formula: Q = mcΔT, where Q is the heat lost, m is the mass of copper (640 g), c is the specific heat capacity of copper (0.385 J/g°C), and ΔT is the change in temperature (375°C - 26°C = 349°C). Plugging these values into the formula, we get: Q = (640 g)(0.385 J/g°C)(349°C) = 85,328 J. Therefore, 85,328 J of heat is lost when the copper cools from 375°C to 26°C.

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