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How much heat is necessary to change 500 g of ice at -10C to water at 20C?
Wiki User
∙ 10y ago
500*20+500*80+500*250+500*100+500*537+500*150*0.5=1000+4000+125000+50000+268500+37500=486000 Calories=468 K.cal.
Wiki User
∙ 15y ago
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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.
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
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 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
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)
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).
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
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.
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.
