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How much heat energy will be required to raise the temperature of 15 grams of water 25 degrees c?
The specific heat capacity of water is 4.18 J/g°C. Using the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature, we can calculate the heat energy as follows: Q = 15g * 4.18 J/g°C * 25°C = 1567.5 J. Therefore, 1567.5 Joules of heat energy will be required to raise the temperature of 15 grams of water by 25 degrees Celsius.
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How many grams of water vapor are required to saturate a kilogram of air at a temperature of -20 degrees Celsius?
At -20 degrees Celsius, the saturation vapor pressure of water is about 2.2 millibars. Therefore, to saturate a kilogram of air at this temperature, you would need about 2.2 grams of water vapor.
How many joules of heat required to raise the temperature of 25 grams of h2o from 21 degrees Celsius to 35.5 degrees?
The specific heat capacity of water is 4.184 J/g°C. The change in temperature is 35.5°C - 21°C = 14.5°C. Using the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature, you can calculate that the heat required is approximately 1554.7 joules.
How do you increase the the temperature of 500 grams of water from 20 degrees Celsius to 100 degrees Celsius?
q(joules) = mass * specific heat * change in temperature q = (500 grams H2O)(4.180 J/goC)(100o C - 20o C) = 1.7 X 105 joules ================add this much heat energy to the water
What is the final temperature when 625 grams of water at 75 degrees loses 7.96?
The final temperature is 59.9°C.
How much heat energy is required to raise the temperature of 0.365 of copper from 23.0 to 60.0 The specific heat of copper is 0.0920?
To calculate the heat energy required, you can use the formula: Q = mcΔT, where Q is the heat energy, m is the mass of the copper (0.365 kg), c is the specific heat capacity of copper (0.0920 J/g°C), and ΔT is the change in temperature (60.0°C - 23.0°C). First, convert the mass to grams and then plug the values into the formula to find the heat energy required.
How much energy is required to raise 21kg of water by 2 degrees Celsius?
The specific heat capacity of water is 4.18 J/g°C. To calculate the energy required to raise 21 kg of water by 2 degrees Celsius, use the formula: Energy = mass x specific heat capacity x temperature change. Plugging in the values, the energy required is 21,084 Joules.
The specific heat of gold is 0.131 Joules per gram. Celsius How much energy is required to heat 1.3 grams of gold from 25 Celsius to 46 Celsius?
The change in temperature is 21 degrees Celsius. To calculate the energy required, we use the formula: Energy = mass * specific heat * change in temperature. Plugging in the values, Energy = 1.3g * 0.131 J/g°C * 21°C = 35.247 Joules. Therefore, 35.247 Joules of energy is required to heat 1.3 grams of gold from 25°C to 46°C.
How many grams of water vapor are required to saturate a kilogram of air at a temperature of -20 degrees Celsius?
At -20 degrees Celsius, the saturation vapor pressure of water is about 2.2 millibars. Therefore, to saturate a kilogram of air at this temperature, you would need about 2.2 grams of water vapor.
How much energy is required to raise the temperature of 5 grams of iron from -10ºC to 30ºC?
The specific heat capacity of iron is 0.45 J/g°C. To calculate the energy required, you can use the formula: Energy = mass x specific heat capacity x change in temperature. Plugging in the values, Energy = 5g x 0.45 J/g°C x (30°C - (-10°C)). This calculation would give you the energy in joules required to raise the temperature of 5 grams of iron from -10ºC to 30ºC.
How much energy is required to raise the temperature of 3 kg aluminum from 18 degrees Celsius to 23 degrees Celsius?
Specific heat af aluminum is 0.89 J/gC, so I will convert to grams for my convince.3 kg Al (1000 g/1 kg) = 3000 grams Alq = mass * specific heat * change in temperatureq = (3000 grams)(0.89 J/gC)(23 C - 18 C)= 1 X 104 Joules==============( as per significant figures )
How much energy is required to raise the temperature of 3kg of aluminum from 18 degrees Celsius to 23 degrees Celsius?
The specific heat capacity of aluminum is 0.902 J/g°C. First, convert 3kg to grams (3000g). Then, calculate the change in temperature (23°C - 18°C = 5°C). Finally, use the formula Q = mcΔT to find the energy required: Q = 3000g * 0.902 J/g°C * 5°C.
How much heat energy will be required to lower the temperature of 2.67kg of steam from 282 degrees Celsius to 105 degrees Celsius?
You mean how much heat energy will be lost/transferred as you are losing Joules here. All in steam, so a simple q problem and no change of state. 2.67 kg = 2670 grams q = (2670 grams steam)(2.0 J/gC)(105 C - 282 C) = - 9.45 X 105 Joules ----------------------------------- This much heat energy must be lost to lower the temperature of the steam.
What would be the final temperature when 250 grams of water at 100 degrees celsius is mixed with 525 grams of water at 30 degrees celsius?
The final temperature would be approximately 54.2 degrees Celsius. This can be calculated using the principle of conservation of energy, where the heat lost by the hot water is equal to the heat gained by the cold water.
How many joules of heat energy are required to raise the temperature of 6 grams of copper of 100 degrees Celsius to 150 degrees Celsius?
The specific heat capacity of copper is 0.385 J/g°C. To calculate the heat energy required, you use the formula: Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Plugging the values in, you get Q = 6g * 0.385 J/g°C * (150°C - 100°C) = 92.4 Joules.
How much energy is required to raise the temperature of 3 kg of aluminum from 18 degrees C to 23 degrees C?
The specific heat capacity of aluminum is 0.897 J/g°C. First we need to convert the mass to grams: 3 kg = 3000 g. Then we can use the formula: energy = mass x specific heat x change in temperature. Plugging in the values: energy = 3000 g x 0.897 J/g°C x (23°C - 18°C) = 13,485 J. So, 13,485 Joules of energy is required.
How much energy is required to raise 3 kg of aluminum from 18 degrees C to 23 degrees C?
The energy required to raise the temperature of a substance can be calculated using the specific heat capacity formula: Q = mcΔT, where Q is the energy transferred, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature. For aluminum, the specific heat capacity is 0.897 J/g°C. Converting the mass to grams (3000 g), the energy required would be: Q = 3000 g * 0.897 J/g°C * 5°C = 13,455 J.
How many joules of heat required to raise the temperature of 25 grams of h2o from 21 degrees Celsius to 35.5 degrees?
The specific heat capacity of water is 4.184 J/g°C. The change in temperature is 35.5°C - 21°C = 14.5°C. Using the formula Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature, you can calculate that the heat required is approximately 1554.7 joules.
