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If 425 joules are absorbed from the higher temperature reservoir and 295 joules of that is passed on to the lower temperature reservoir how much work has been done by the system?
To calculate the work done by the system, we can use the formula for efficiency: Efficiency = Work output / Heat input. First, let's determine how much heat is not passed on to the lower temperature reservoir: 425 - 295 = 130 J. Thus, the work done by the system is the heat that is not passed on, which is 130 joules.
The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
To calculate the heat absorbed by the water, you can use the formula: heat = mass * specific heat capacity * temperature change. First, determine the specific heat capacity of water (4.18 J/g°C). Then, plug in the values: heat = 15 g * 4.18 J/g°C * 3.0°C. The heat absorbed by the water is 188.1 Joules.
How many joules are required to boil one liter of water?
Any number of joules, no matter how small, will raise the temperatureof the water. The total number required in order to accomplish the jobdepends on the final temperature you want to see. The higher that is,the more energy it will take to reach it.
How many joules are needed to change the temperature of 1 gram of water by 1C?
It takes 4.184 joules of energy to change the temperature of 1 gram of water by 1 degree Celsius.
What the internal energy of a system that does 5000 joules of work and absorbs 20000 joules of heat?
The internal energy change of the system would be the sum of the heat absorbed and the work done on the system. Therefore, the internal energy change would be 20000 J (heat absorbed) + 5000 J (work done) = 25000 J.
If 425 joules are absorbed from the higher temperature reservoir and 295 joules of that is passed on to the lower temperature reservoir how much work has been done by the system?
To calculate the work done by the system, we can use the formula for efficiency: Efficiency = Work output / Heat input. First, let's determine how much heat is not passed on to the lower temperature reservoir: 425 - 295 = 130 J. Thus, the work done by the system is the heat that is not passed on, which is 130 joules.
What is heat and how do you measure heat?
Heat is energy in transit from a higher temperature to a lower temperature. In SI, heat is measured in joules.
How many joules are absorbed by the water with a mass of 8 kg in order to raise the temperature from 20 degrees to 70 degrees?
q(joules) = mass * specific heat * change in temperature ( 8 kg = 8000 grams ) q = (8000 grams H2O)(4.180 J/gC)(70o C - 20o C) = 1.7 X 106 joules ============
How many joules are absorbed by the water with a mass of 5kg in orderto risethe temperature from 30 c to 65 c?
To calculate the energy absorbed by the water, you can use the equation Q = mcΔT, where Q is the energy absorbed, m is the mass of water (5kg), c is the specific heat capacity of water (4186 J/kg°C), and ΔT is the change in temperature (65°C - 30°C). Plugging in the values gives Q = 5kg * 4186 J/kg°C * (65°C - 30°C). Calculate this to find the energy absorbed in joules.
The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
To calculate the heat absorbed by the water, you can use the formula: heat = mass * specific heat capacity * temperature change. First, determine the specific heat capacity of water (4.18 J/g°C). Then, plug in the values: heat = 15 g * 4.18 J/g°C * 3.0°C. The heat absorbed by the water is 188.1 Joules.
How much heat is absorbed by 100 mL of a dilute slution of NH4NO3 as it changes its temperature from 25.3 to 22.4?
To calculate the heat absorbed, you need the specific heat capacity of the solution. Once you have that, you can use the formula: Q = m * c * ΔT, where Q is the heat absorbed, m is the mass of the solution, c is the specific heat capacity, and ΔT is the change in temperature. Plug in the values and calculate to find the amount of heat absorbed.
If an endothermic process absorbs 263 Joules how many kilo-calories are absorbed?
To convert Joules to kilocalories, divide the amount of energy in Joules by 4184 (the conversion factor between Joules and kilocalories). Thus, 263 Joules is equivalent to approximately 0.063 kcal.
How many joules of heart are absorbed by 500.0 g of water when its temperature increases from 20.0 degrees C to 80.0 degrees C?
The specific heat capacity of water is 4.18 J/g°C. The change in temperature is 80.0°C - 20.0°C = 60.0°C. The amount of heat absorbed is calculated using the formula: q = m * c * ΔT. So, q = 500.0g * 4.18 J/g°C * 60.0°C = 12540 J. Thus, 12540 joules of heat are absorbed.
What is the total number of joules absorbed by 65.0g of water when the temperature of the water is raised from 25.0 to 40.0?
The specific heat capacity of water is 4.18 J/g°C. To calculate the total energy absorbed, we use the formula: Q = m * c * ΔT, where Q is the energy absorbed, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. Plugging in the values, we get Q = 65.0g * 4.18 J/g°C * (40.0°C - 25.0°C) = 1313.5 J.
What are the units used is temperature?
calories and joules
What is the total amount of heat energy in joules absorbed by 25.0 grams of water when the temperature of the water increased from 24.0 C to 36.0 C?
To calculate the total amount of heat energy absorbed by the water, you can use the formula: q = mcΔT, where q is the heat energy, m is the mass of the water (25.0 g), c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature (36.0°C - 24.0°C = 12.0°C). Plugging in these values, you get q = 25.0 g * 4.18 J/g°C * 12.0°C = 1257 J. Therefore, the total amount of heat energy absorbed by the water is 1257 joules.
How many joules are required to boil one liter of water?
Any number of joules, no matter how small, will raise the temperatureof the water. The total number required in order to accomplish the jobdepends on the final temperature you want to see. The higher that is,the more energy it will take to reach it.
