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How much heat is necessary to change 10 g of ice at 10C into water at 20C?
Wiki User
∙ 10y ago
For 1 gram of water, you need 4.184 Joule to raise the T from 15 degrees Celsius to 16 degrees Celsius. The values are slightly different for other temperatures. So an estimation of the required energy would be 10 * 4.2 * 80. The 10 comes from 10 gram, the 4.2 from the energy required to heat 1 gram of water 1 degrees Celsius. The 80 comes from the starting temperature to the final temperature. The estimated answer is then 3360 J. For 1 gram of water, you need 4.184 Joule to raise the T from 15 degrees Celsius to 16 degrees Celsius. The values are slightly different for other temperatures. So an estimation of the required energy would be 10 * 4.2 * 80. The 10 comes from 10 gram, the 4.2 from the energy required to heat 1 gram of water 1 degrees Celsius. The 80 comes from the starting temperature to the final temperature. The estimated answer is then 3360 J.
Wiki User
∙ 7y ago
Wiki User
∙ 10y ago10 g of ice has to melt at 10 degrees C and the calories required would be 10 times the latent heat of fusion of ice which is approximately 80 cals/gram. Then we have to rise the temperature of 10 g of water from 10 degrees C to 20 degrees C.
This would be 10 x 10 x specific heat of water which is 1 cal per gram
The total energy in calories required would be
(10 x 80) + (10 x 1 x 10) = 800 + 100 = 900cals
Wiki User
∙ 11y ago10*10 calories to raise the temp of ice from -10 deg C to 0 deg C
10*80 calories to melt the ice to water
10*20 calorie to raise the temp of water from 0 deg C to 20 deg C.
= 100 + 800 + 200 = 1100 cals.
Wiki User
∙ 11y agoChange ice to water- 10g ice to water
Equation: Q= m x specific latent heat of ice
Q = 10g * 340
Q = 3400J
Wiki User
∙ 7y agoThe specific heat of ice is 2,05 J/g.K
The specific heat of water is4,186 J/g.K
So the total necessary heat is:
Q = (2,05 x 10 x 1o) + (4,186 x 10 x 20) = 1 042,2 joules
Wiki User
∙ 9y agoThe amount of heat needed to raise temperature of a substance is measure by the equation Q=mc@. The difference of temperature is 30 degrees Celsius. Therefor Q=0.3J.
Wiki User
∙ 7y agoThe specific heat capacity of ice is 2,05 J/g.K.
The specific heat capacity of water is 4,186 J/g.K.
Necessary heat is: (2,05 x 10 x 10) + (4,186 x 20 x 10) = 1042,2 J
Wiki User
∙ 16y ago100 calories
Wiki User
∙ 10y ago6300 jules
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How much heat is necessary to change 220 g of ice at -5C to water at 20C?
You need to add all of the following:* The heat required to heat ice from -5 to 0 degrees. Multiply the mass times the temperature difference times the specific heat of ice. * The heat required to melt ice. Multiply the mass by the heat of fusion. * The heat required to raiste the temperature of water from 0 to 20 degrees. Multiply the mass times the temperature difference times the specific heat of water.
Is water a good conductor for heat?
Water has a high specific heat capacity (relative to metals and other conductors), making it a poor conductor of heat (takes too much energy to change the temperature).
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
Amount of heat necessary to change the state of substance?
Heat of vaporization or enthalpy of vaporization. It is the additional energy, per unit mass, required after vaporization temperature (boiling point) is reached, to accomplish the change in state, from liquid to gas.
Why does melting ice require much less energy than boiling the same mass of water?
Because Water's latent heat of fusion is much less than its latent heat of vaporization. In English: It takes less energy to change a gram of ice at 0°C into a gram of water at the same temperature than it takes to change a gram of water at 100°C into a gram of steam at the same temperature.
How much heat must be transferred to liquid water to change the waters temperature from 27 degrees Celsius to 32 degrees Celsius?
To change the temperature of water from 27ºC to 32ºC will depend on the mass of water that is present. Obviously, the more water, the more heat it will take. This can be calculated as follows:q = heat = mC∆T where m is the mass of water; C is sp. heat = 4.184 J/g/deg and ∆T is 5ºC (change in temp).
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
How much heat is necessary to change 30 grams of water at 40 degrees celsius into water at 60 degrees celsius?
The idea here is to: * Look up the specific heat of water. * Multiply the mass, times the temperature difference, times the specific heat of water. You may need to do some unit conversions first; specifically, if the specific heat is given per kilogram, you can convert the grams to kilograms.
How much heat is necessary to change 220 g of ice at -5C to water at 20C?
You need to add all of the following:* The heat required to heat ice from -5 to 0 degrees. Multiply the mass times the temperature difference times the specific heat of ice. * The heat required to melt ice. Multiply the mass by the heat of fusion. * The heat required to raiste the temperature of water from 0 to 20 degrees. Multiply the mass times the temperature difference times the specific heat of water.
How much more heat needs to be added to water at 100 degrees centigrade in order to change it to steam?
Heat required to have such a change of state is called latent heat. If L J/kg is the latent heat per kg of water then for M kg of water we need M* L joule of heat energy
What properties of water protects organism from overheating?
water has a high heat of vapourization.it absorbs much heat as it changes from liquid to gas.it has the capacity of absorbing heat with minimum of change in its own temperature
Is water a good conductor for heat?
Water has a high specific heat capacity (relative to metals and other conductors), making it a poor conductor of heat (takes too much energy to change the temperature).
In which temperature water has maximum specific heat capacity?
The specific heat capacity of water does not change much within-phase (ie, as a solid it has one specific heat capacity, as a liquid/gas it has another)
Why does water not heat up or cool off as air?
because the specific heat of water is very high
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
What is the equation for calculating how much heat energy (calories) transferred to or from a mass of water.?
The equation is q = mC∆T where q is the heat; m is the mass of water; C is the specific heat of water (1 cal/g/deg); and ∆T is the change in temperature.
Amount of heat necessary to change the state of substance?
Heat of vaporization or enthalpy of vaporization. It is the additional energy, per unit mass, required after vaporization temperature (boiling point) is reached, to accomplish the change in state, from liquid to gas.
