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What is required to change the state of water?
To change the state of water from solid (ice) to liquid (water), heat must be added to increase the temperature above 0 degrees Celsius. To change water from liquid to gas (water vapor), heat must be added to increase the temperature above 100 degrees Celsius.
If 200g ice cube with an initial temperature of -12 degrees celsius is placed in 1 kg of warm water with an initial temperature of 40 degrees celsius If you ignore any heat losses to the environment?
The ice will absorb heat from the warm water and increase in temperature until it reaches 0 degrees Celsius. The heat lost by the warm water is equal to the heat gained by the ice. Use the equation: (Q = mcΔT) where Q is heat energy, m is mass, c is specific heat capacity, and ΔT is temperature change to calculate the final temperature of the system.
A person tries to heat up her bath water by adding 5 L of water at 80 C to 60 L of water at 30 C What is the final temperature of the water?
To find the final temperature, you can use the principle of conservation of energy. The heat lost by the hot water equals the heat gained by the cold water. You can calculate the final temperature using this principle and the specific heat capacity of water, which is 1 calorie/gram degrees Celsius.
) The temperature of a sample of water changes from 10 and degC to 20 and degC when the water absorbs 100 calories of heat. What is the mass of the sample?
one calorie of heat is able to raise one gram of water one degree Celsius so 400 calories could raise 1g of water 400 degrees, so it would raise the 80g by(400/80) 5 degrees Celsius plus the initial temp of 10 degrees, the 80g of water would have a final temp of 15 degrees Celsius
In which temperature water has maximum specific heat capacity?
Water has the highest specific heat capacity at 25 degrees Celsius. This means that it can absorb or release a significant amount of heat before its temperature changes, making it an effective heat buffer.
A calorimeter contains 0.750 kilogram of liquid water at 17.0 degrees C. A 0.0580 kilogram block of copper at 98.0 degrees C is placed in the water. What is the final temperature of the system?
The heat lost by the copper block equals the heat gained by the water and calorimeter. Using the heat equation, q=mcΔT, where q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature, you can calculate the final temperature of the system as 26.2 degrees Celsius.
What is a correct numerical set up for calculating the number of joules of heat gained by water?
To calculate the number of joules of heat gained by water, you can use the formula Q = m * c * ΔT, where Q is the heat gained, m is the mass of water in grams, c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature in degrees Celsius. Plug in the values for m, c, and ΔT to calculate the heat gained in joules.
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.
What is the enthalpy change for converting 1 mol of ice at -50 degrees celsius to water at 70 degrees celsius?
The enthalpy change for converting 1 mol of ice at -50 degrees Celsius to water at 70 degrees Celsius is the sum of the enthalpy changes for the following processes: heating ice from -50 degrees Celsius to 0 degrees Celsius (heat of fusion), melting ice at 0 degrees Celsius, and heating water from 0 degrees Celsius to 70 degrees Celsius (specific heat of water).
Is the heat intensity of water at 100 degrees celsius the same as the heat intensity of water 212 degrees Fahrenheit?
100 degrees celsius are equal to 212 degrees fahrenheit.
What is required to change the state of water?
To change the state of water from solid (ice) to liquid (water), heat must be added to increase the temperature above 0 degrees Celsius. To change water from liquid to gas (water vapor), heat must be added to increase the temperature above 100 degrees Celsius.
How much energy is gained by 3 grams of ice when it changes to water?
The energy needed to change ice into water is called the heat of fusion. For ice, this value is around 334 joules per gram. So, for 3 grams of ice, the energy gained when it changes to water would be around 1002 joules (334 joules/gram * 3 grams).
When water at 0.c freezes is heat lost or gained?
As heat is a form of energy, it isn't lost or gained, it's just converted into another form of energy.
A 34.44-g sample of metal is heated to 98.6 degrees Celsius in a hot water bath until thermal equilibrium is reached What is the specific heat of the metal?
Heat lost by the metal = heat gained by the water. Heat gained by the water = 50.0 g x 4.184 J/g K x (28.3-22.2) = 1276 J Heat lost by metal = 1276 J = 34.44 g x Sp Heat x (98.6 - 28.3) Specific Heat = 1276 J / 2421 g K = 0.527 J/g K
What is the final temperature of a 3.0kg bar of gold at 99 degrees Celsius dropped into 0.22kg of water at 25 degrees celsius?
To find the final temperature, we can use the principle of conservation of energy: heat lost by gold = heat gained by water. We can use the formula m * c * ∆T to calculate the heat exchanged. By setting the two heat exchanges equal to each other and solving for the final temperature, we can find that the final temperature is 25.9 degrees Celsius.
Why heat is needed to boil water?
Because heat changes the temperature of the water
How are the amount of heat transferred and the changes in temperature of water related?
Hi, heat transferred = mass x specific heat capacity x rise/fall in temperature If heat is lost then fall in temperature If heat is gained then rise in temperature. More the transfer then greater the difference in temperature.
