how much energy (in joules) is needed to heat 200.0 g of water by 10.0 ∘c?
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Expert Answer The energy in joules that is needed to heat 200.0 g of water by 10.0 degrees Celsius is to be calculated. The heat capacity of water is 4.185 joules/grams. °Celsius.
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One liter of water is about 1 Kg or 1000g, giving Q = m x (delta T) x Specific heat of water = 1000g x 80C x 1 cal/g C= 80,000 cal or 80 Kcals. Technically, 80 kcals that is the amount of heat needed to get the liquid water to 100C and anything extra would go into vaporizing the water into steam.
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The total energy (heat) is required to convert 52.0 g of ice at –10.0°C to steam at 100°C is C) 158 kJ.
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Water has a heat of vaporization value of 40.65 kJ/mol. A considerable amount of heat energy (586 calories) is required to accomplish this change in water.
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Quantitative experiments show that 4.18 Joules of heat energy are required to raise the temperature of 1g of water by 1°C. Thus, a liter (1000g) of water that increased from 24 to 25°C has absorbed 4.18 J/g°C x 1000g x 1°C or 4180 Joules of energy.
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The standard molar heat of vaporization for water is 40.79 kJ/mol.
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Energy is always required to break a bond, which is known as bond energy. The electrolysis of water requires a minimum of 237.13 kJ of electrical energy input to dissociate each mole. Each mole of water gives you 2 grams of Hydrogen and 16 grams of Oxygen.
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Answer: The heat energy is 2.48 mega joules. Explanation: To find : How much heat energy (in mega joules) is needed to convert 7 kilograms of ice at -9°C to water at 0°C?
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For water at its normal boiling point of 100 ºC, the heat of vaporization is 2260 J g-1. This means that to convert 1 g of water at 100 ºC to 1 g of steam at 100 ºC, 2260 J of heat must be absorbed by the water.
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Answer: The amount of heat required to melt 25 grams of ice is 8,350 Joules or 2,000 calories.
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It takes about 4200 J per liter/degree. Then you need to crystallize the water. It takes 333 KJ to cristallize 1 kg or 1 l of water (the density of water is 1). So in total you need to extract 417 KJ of energy.
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Convert 1.4923933_10^-10 kg_m^2 /s^2 to joules \"J\" Knowing that 1 kg_m^2 /s^2 = 1 J, the answer will be 1 amu = 1.4923933_10^-10 J.
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How many Joules of energy do you need to melt all the ice into a pure liquid along the path from B to C on the graph? Answer: For 1 kilogram of ice ,which equals 1000 grams, we need 333 Joules/gram x 1000 grams = 333,000 Joules.
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The standard molar heat of vaporization for water is 40.79 kJ/mol. How much energy would be required to vaporize 94.0 g of water? The standard molar heat of vaporization for water is 40.79 kJ/mol.
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The energy released when steam condenses to water is in the range 2000 - 2250 kJ/kg (depending on the pressure) - compared to water with 80 - 120 kJ/kg (with temperature difference 20 - 30 oC).
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A calorie is a unit of thermal energy equal to 4.184 joules or the amount of energy required to raise the temperature of 1 gram of liquid water 1°C at standard pressure. ... The Calorie is 100 calories or the amount of thermal energy needed to heat one kilogram of water one degree Celsius.
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What c in the equation is, the specific heat capacity. So in water it takes 1200 joule's to raise a Kg of water by 1 degree K or in degrees C. If this takes 1 min to boil the power required to boil the water equals 96kilo joules/60 seconds =1600 watts or 1.6 kilo watts.