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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.
What else can I help you with?
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 mass of an object with 2258 joules of heat absorbed?
It could be almost anything. The relationship is: heat = mass x specific heat x temperature change So, if you know any three of these variables, you can calculate the fourth one.
How do you convert Joules To fahrenheit?
Joules and Fahrenheit are two different units that measure different quantities - energy and temperature, respectively. They cannot be directly converted to each other because they are not the same type of measurement.
What is a latent heat energy levels?
Latent heat- the amount of heat required by a system/ substance to change phase. It's also heat absorbed or radiated during a change of phase at a constant temperature and pressure.
If 425 joules are absorbed from the higher temperature reservoir and 295 joules of that is passed onto the lower temperature reservoir how much work has been done by the system?
The work done by the system can be calculated by finding the difference between the heat absorbed from the high-temperature reservoir and the heat passed onto the low-temperature reservoir. In this case, the work done by the system is 130 joules (425 joules - 295 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 ============
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.
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.
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 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.
What are the units used is temperature?
calories and joules
What is the mass of an object with 2258 joules of heat absorbed?
It could be almost anything. The relationship is: heat = mass x specific heat x temperature change So, if you know any three of these variables, you can calculate the fourth one.
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.
