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) 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?
Wiki User
∙ 7y ago
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
Wiki User
∙ 7y ago
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What happens to a fixed sample of gas when its temperature changes?
If a fixed sample of gas has a change of temperature pressure would increase.
Calculate the specific heat of a substance if 44.0 g of the sample absorbs 67.2 J and the temperature change is 11 K?
Determine the specific heat of a material if a 32 g sample of the material absorbs 58 J as it is heated from 298 K to 313 K?
Chemistry calorimetry help?
Calorimetry measures the heat of chemical reactions and physical changes. The steps involved in solving calorimetry problems are as follows: The heat of the reaction is less than the amount of heat measured by the calometer. The heat gained by the calometer is the capacity of the calorimeter and temperature change of the sample undergoing the chemical and/or physical change. The combination of the two are calculated to heat reaction and given temperature change.
What is the purpose of stirring the mixture in the calorimiter after the hot sample was poured into it?
It is doubtful that the walls of the sample holder in the calorimeter start at the same temperature as the sample. By stirring it, you can help equalize the temperature throughout the sample and bring the sample and the sample holder into thermal equilibrium before you start the measurements.
Which sample had the lowest final temperature?
white
What happens to the thermal energy of a substance as its temperature increases?
When a sample of a substance absorbs thermal energy, its temperature rises.
What happens to a fixed sample of gas when its temperature changes?
If a fixed sample of gas has a change of temperature pressure would increase.
Calculate the specific heat of a substance if 44.0 g of the sample absorbs 67.2 J and the temperature change is 11 K?
Determine the specific heat of a material if a 32 g sample of the material absorbs 58 J as it is heated from 298 K to 313 K?
If a 1.0-g sample of steam at 100 degrees Celsius loses 560 calories of heat what would the resulting temperature of the steam sample be?
80
how many calories are required to increase the temperature of a 27.3 g copper sample from 36.2 degrees C to 74.4 degrees C?
80 calories per gram
How many calories are required to raise the temperature of a 35.0g sample of iron from 25 C to 35 C?
38 cal
The temperature of a sample of a substance changes from 10 degree celsius to 20 degree celsius by how many kelvins does the temperature change?
changes 10 degrees C and 283 degrees K if im not mistaken which im bound to be not sure of the esential #
Chemistry calorimetry help?
Calorimetry measures the heat of chemical reactions and physical changes. The steps involved in solving calorimetry problems are as follows: The heat of the reaction is less than the amount of heat measured by the calometer. The heat gained by the calometer is the capacity of the calorimeter and temperature change of the sample undergoing the chemical and/or physical change. The combination of the two are calculated to heat reaction and given temperature change.
Why would water in a 100cm3 and water a 10cm3 cylinder measure the same temperature?
Because they are the same temperature. There are more calories of heat in a 100-ml sample of water that's at a certain temperature than there are in a 10-ml sample that's the same temperature...but 20-degree-Celsius water is 20-degree-Celsius water whether you have a thimbleful, a glassful or a swimming pool full.
What is the point of the range?
The difference between the temperature at which the sample begins to melt and at the temperature at which the sample completely melted-
How much ice water will it take to cool the sample to 20 degrees celsius?
That would depend on the mass of the sample, its temperature, and what the sample is made of.
The specific heat of gold is 0.031 caloriesgram and degC. If 10.0 grams of gold were heated and the temperature of the sample changed by 20.0 and degC how many calories of heat energy were absorbed by?
The needed heat is:Q = 10 x 20 x 0,031 = 6,2 calories
