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How much heat must be absorbed by a 500 g pot of water in order to raise the temperature from 20?
To calculate the heat absorbed by a 500 g pot of water to raise its temperature from 20°C, we can use the formula ( Q = mc\Delta T ), where ( Q ) is the heat absorbed, ( m ) is the mass (500 g or 0.5 kg), ( c ) is the specific heat capacity of water (approximately 4,186 J/kg°C), and ( \Delta T ) is the change in temperature. If we want to raise the temperature to, say, 100°C, then ( \Delta T ) would be 80°C. Thus, ( Q = 0.5 , \text{kg} \times 4186 , \text{J/kg°C} \times 80 , \text{°C} ), which equals 167,440 J.
What else can I help you with?
Which is affected more when you increase the temperature?
Water is something that will be affected if you raise the temperature. When cooking, you may need to raise the temperature of water to a boil, in order to cook food.
How much heat must be absorbed by a 500 g pot of water in order to raise the temperature from 20c to 30c?
To calculate the heat absorbed by the water, you can use the formula ( Q = mc\Delta T ), where ( Q ) is the heat absorbed, ( m ) is the mass of the water, ( c ) is the specific heat capacity of water (approximately 4.18 J/g°C), and ( \Delta T ) is the change in temperature. For a 500 g pot of water raising the temperature from 20°C to 30°C (( \Delta T = 10°C )), the calculation would be: [ Q = 500 , \text{g} \times 4.18 , \text{J/g°C} \times 10 , \text{°C} = 20,900 , \text{J} ] Thus, 20,900 joules of heat must be absorbed.
What is the temperature change when 40g of ice is added to 100g of water at room temperature?
To determine the temperature change when 40g of ice is added to 100g of water at room temperature, you must consider the heat transfer involved in melting the ice and warming the resulting water. The heat absorbed by the ice to melt (latent heat of fusion) and then raise its temperature to the final equilibrium temperature will lead to a decrease in the temperature of the warm water. The final temperature will depend on the initial temperature of the water and the specific heat capacity of both water and ice, which typically results in a lower equilibrium temperature than the initial temperature of the water.
How many calories are required to raise the temperature of 1 g of water by 5 degrees C?
1 calorie is the energy required to raise 1 gram of water by 1 degree C. So it would take 5 calories to raise it by 5 degrees C.
Water has a temp of 4.184 and copper has a temp of 0.387. Does it takes more heat to raise the temp of the copper molecule?
These are not temperature numbers but specific heat numbers. They mean that it takes 4.184 Joules and 0.387 Joules respectively to raise water and copper of one gram by one degree celsius. So, as you can see, it takes a lot more heat to raise the temperature of water than it does of copper. Water has a very high specific heat.
Which is affected more when you increase the temperature?
Water is something that will be affected if you raise the temperature. When cooking, you may need to raise the temperature of water to a boil, in order to cook food.
Is it harder to raise the temperature of a rock than it is to raise the temperature of water?
It is harder to raise the temperature of water than it is to raise the temperature of a rock. It takes 1 calorie of energy to raise the temperature of 1 gram of water by 1 degree C, whereas it only takes 0.02 calorie to heat a gram of rock to that temperature.
How much water do dried green beans absorb?
t he amount of water absorbed by raisins depends upon temperature of water .The more the temperature of water the more is the water absorbed.water is absorbed the most in lukewarm water.
How much heat must be absorbed by a 500 g pot of water in order to raise the temperature from 20c to 30c?
To calculate the heat absorbed by the water, you can use the formula ( Q = mc\Delta T ), where ( Q ) is the heat absorbed, ( m ) is the mass of the water, ( c ) is the specific heat capacity of water (approximately 4.18 J/g°C), and ( \Delta T ) is the change in temperature. For a 500 g pot of water raising the temperature from 20°C to 30°C (( \Delta T = 10°C )), the calculation would be: [ Q = 500 , \text{g} \times 4.18 , \text{J/g°C} \times 10 , \text{°C} = 20,900 , \text{J} ] Thus, 20,900 joules of heat must be absorbed.
When liquid water is heated most of the energy that the water initially absorbs is used to do?
It is used to raise the temperature of the water.
How many calories does it take to raise the temperature of a cup of water?
It depends on what temperature is is at and how much water there is.
What is to raise the temperature of 1 gram of water 1 degree Clntigrade?
Depends on how high you want to raise the gram of water ;).
Energy that is absorbed by land and water is changed into?
Heat energy. This absorbed energy warms the land and water, leading to an increase in temperature.
Does the heat per pound to change the temperature of water stay the same regardless if the water is in a solid liquid or vapor state?
No. The quantity of energy required to raise the temperature of water is different depending on the phase of water. This is especially true at or near a phase transition as thermal energy is absorbed during a phase transistion thus altering the amount of energy required to raise the temperature of said water.
Which material woud take the longest to raise its temperature?
water
How do you take out Co2 in water?
If you raise the temperature, solubility decreases
How many degrees will 340 J raise the temperature of 6.8 g of water (Refer to table of constants for water.)?
12 degrees Celsius
