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To calculate the heat required to heat 1 cubic meter of air by 200 degrees Celsius, we can use the specific heat capacity of air, which is approximately 1005 J/(kg·K). The density of air is about 1.225 kg/m³. Thus, the heat required (Q) can be calculated using the formula Q = mass × specific heat × temperature change. For 1 m³ of air, Q = (1.225 kg) × (1005 J/(kg·K)) × (200 K) ≈ 245,000 J, or 245 kJ.
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How much heat is required to evaporate 1 liter of water at 100 degree celsius?
The heat required to evaporate 1 liter of water at 100 degrees Celsius is known as the latent heat of vaporization of water, which is approximately 2260 kJ/kg. Since the density of water is about 1000 kg/m³, the heat required would be around 2260 kJ.
What is the measurement of how much heat energy is required for a substance to melt?
The measurement of how much heat energy is required for a substance to melt is called the heat of fusion. It is the amount of energy required to change a substance from a solid to a liquid at its melting point.
How much heat energy in kilojoules is required to convert 41.0g of ice at -18.0 degrees C to water at 25.0 degrees C?
The total heat energy required can be broken down into two steps: first, raising the temperature of ice from -18.0°C to 0°C, then melting the ice at 0°C to water at 25.0°C. The heat energy required is calculated using the formula: Q = mcΔT, where Q is heat energy, m is mass, c is specific heat capacity, and ΔT is the temperature change. Step 1: Raise temperature of ice to 0°C Q1 = 41.0g * 2.09 J/g°C * 18.0°C = 1552.22 J Step 2: Melt ice at 0°C Q2 = 41.0g * 334 J/g = 13694 J Total heat energy required = Q1 + Q2 = 13694 J + 1552.22 J = 15246.22 J Convert J to kJ: 15246.22 J * (1 kJ / 1000 J) ≈ 15.25 kJ Therefore, approximately 15.25 kJ of heat energy is required to convert 41.0g of ice at -18.0 degrees C to water at 25.0 degrees C.
If 30.86g of H2O is frozen (from liquid to solid) how much heat energy is required?
No heat (energy) is required to freeze water (from liquid to solid). Freezing RELEASES energy (heat), as it is an exothermic event. If you want to know how much energy is release, you need to know the heat of fusion for water, and then multiply that by the mass of water being frozen.
How much heat is lost when 2012 grams of stream at 400 K is changed into ice at 263 K?
To determine the heat lost, we need to calculate the heat required to cool the steam from 400 K to 273 K (its condensation point), then the heat required to change it from steam to liquid water, and finally the heat required to freeze the water into ice at 273 K. These steps involve the specific heat capacities of water and steam, latent heat of vaporization, and latent heat of fusion.
How much heat requerd for 1cubic meter nitrogen to rise temperatore from 35celceous to 1000 celceous?
If you warm it from 35 degrees Celsius to 1000 degrees Celsius, a mas will vastly increase in volume or pressure. Without knowing how you intend to allow for that, your question is unanswerable.
How much heat is required to warm 1.20 kg of sand from 30.0 degrees C to 100.0 degrees C?
7.014*10^4
How much heat in joules is required to convert 92g of ice at 0.00 degrees Celsius to water vapor at 148 degrees Celsius?
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How much energy does it take to heat 1cubic centimetere of water?
It depends on which temperature you want to reach and at which temperature is the water before you start heating it!
How much heat is required to convert 1.00 kg of water at 100 degrees Celsius to steam at 100 degrees Celsius?
Assuming standard atmospheric pressure, 2260 kilojoules.
How much heat is required to change 0.2kg of ice at -5 degrees to water at 5 degrees?
Heat required for this transition is given as the the sum of three heatsheat required for heating the ice from -5 degree Celsius +latent heat(conversion of ice at zero degree to water at zero degrees)+heat required to heat the water from 0 to 5 degree CelsiusHeating of ice=m x s x delta T,where m is the mass ,s is the specific heat of ice=200x0.5x5=500calmelting of ice=mxlatent heat=200x80=16,000calHeating of water=m x s x delta T,where m is the mass ,s is the specific heat of water =200x1x5=1000calTotal heat required=500+16,000+1000=17,500 cal
How much joules does it take to heat water to 100 degrees?
To heat 1 gram of water by 1 degree Celsius, it takes 4.18 joules. So, to heat water from, for example, 20 degrees to 100 degrees, you would need to calculate the total mass of water and apply the specific heat capacity to determine the total energy required.
How much does 1cubic centimeter of gel weigh?
It depends on the density of the gel.
How much energy is needed to change 125g of ice at -32.9 degrees to water at 75 degrees?
To calculate the energy needed to change ice at -32.9 degrees to water at 75 degrees, you need to consider the energy required for three steps: Heating ice from -32.9 degrees to 0 degrees (specific heat capacity of ice) Melting ice at 0 degrees into water at 0 degrees (latent heat of fusion of ice) Heating water from 0 degrees to 75 degrees (specific heat capacity of water) Once you have the energy needed for each step, you can add them together to find the total energy required.
How much heat is required to raise the temperature of 0.25 kg of water from 20 Celsius to 30 Celsius?
The specific heat capacity of water is 4186 J/kg*C. To calculate the heat required, use the formula: heat = mass * specific heat capacity * change in temperature. Plugging in the values, the heat required to raise the temperature of 0.25 kg of water by 10 degrees Celsius is approximately 1046.5 Joules.
How much heat energy is required to raise the temperature of 0.362 kg of copper from 23.0 degrees Celsius to 60.0 degrees Celsius?
The amount of heat energy required can be calculated using the formula: Q = mcΔT. Given m = 0.362 kg, c = 390 J/kg°C for copper, and ΔT = (60.0 - 23.0) = 37.0 °C, plug these values into the formula to find the heat energy required to raise the temperature of the copper.
How much heat is required to evaporate 1 liter of water at 100 degree celsius?
The heat required to evaporate 1 liter of water at 100 degrees Celsius is known as the latent heat of vaporization of water, which is approximately 2260 kJ/kg. Since the density of water is about 1000 kg/m³, the heat required would be around 2260 kJ.
