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How much heat in kilojoules is released when 25.0 g of water is cooled from 85.0ºC to 40.0ºC The specific heat of water is 4.184 J(gC).?
Wiki User
∙ 7y ago
q = mC∆T where q=heat; m=mass of water; C=sp.heat; ∆T=change in temp.q = (25.0g)(4.184 J/g/deg)(45 deg)
q = 4707 J of heat released
Wiki User
∙ 7y ago
The heat released can be calculated using the formula: Q = m * c * ΔT, where Q is the heat released, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. Converting the units, the heat released is approximately 2.44 kJ.
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Fifty grams of water cooled from 50 degrees to 10 degrees if the specific heat of wayer is 4.2 hoe much was released?
The amount of heat released can be calculated using the formula: Q = mcΔT, where Q is the heat released, m is the mass (50g), c is the specific heat (4.2 J/g°C for water), and ΔT is the change in temperature (50°C - 10°C). Substituting the values, we get Q = 50g * 4.2 J/g°C * (50°C - 10°C) = 8400 J (or 8.4 kJ) of heat released.
Which gas forms the liquid first when the air is cooled?
When air is cooled, the gas that typically condenses first to form a liquid is water vapor. This process occurs at a specific temperature known as the dew point, where the air becomes saturated with moisture and water vapor condenses into liquid water droplets.
How many joules of heat are released when 50 grams of water are cooled from 70. to 60.?
The specific heat capacity of water is 4.18 J/g°C. To calculate the heat released when cooling 50 grams of water from 70°C to 60°C, you would use the formula: q = mcΔT, where q is the heat released, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Plugging in the values, the heat released is 2090 Joules.
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To find the rise in temperature of water in a calorimeter, you would measure the initial temperature of the water, then add a known quantity of heat to the system (e.g. by burning a fuel), and measure the final temperature. The change in temperature of the water is a measure of the heat released or absorbed by the system.
Fifty grams of water cooled from 50 degrees to 10 degrees if the specific heat of wayer is 4.2 hoe much was released?
The amount of heat released can be calculated using the formula: Q = mcΔT, where Q is the heat released, m is the mass (50g), c is the specific heat (4.2 J/g°C for water), and ΔT is the change in temperature (50°C - 10°C). Substituting the values, we get Q = 50g * 4.2 J/g°C * (50°C - 10°C) = 8400 J (or 8.4 kJ) of heat released.
How much heat in kilojoules must be removed from a glass of water that contains 100g of water to lower it's temperature from 30c to 30c?
~ 6.3 kilojoules When 1 g of water is cooled down by 1°C it releases 1 calorie so cooling 100g of water 15 times 1°C releases 1500 calories worth of heat. The transfer factor from calorie to joule is ~ 4.2 joules/calorie 1500 calories * 4.2 joules/calorie = 6300 joules = 6.3 kilojoules
How much kilojoules are in water?
3
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There are approximately 4.18 kilojoules (kJ) in 1 liter of water.
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How much heat in kilojoules must be removed from a glass of water that contains 100g of water to lower its temperature from?
We need the initial temperature and the final temperature to calculate the heat removed using the specific heat capacity of water, which is 4.18 J/g°C or 4.18 kJ/kg°C. As a rough estimate, assuming the initial temperature is around room temperature (20°C) and the final temperature is near freezing (0°C), the heat removed would be about 83.6 kJ based on the given mass of water (100g).
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The thermal energy of a solid is the internal energy stored within the atoms and molecules of the solid due to their motion and vibration. It is a measure of the kinetic energy of the particles in the solid and is related to the temperature of the solid. In essence, it represents the energy associated with the random motion of particles within the structure of the solid.
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