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When 90 kJ is removed from a 2-kg copper bar its temperature drops from 200 degrees Celsius to 85 degrees Celsius what is the specific heat of the iron?
Wiki User
∙ 13y ago
q( Joules) = mass grams * specific heat * change in temperature
90 kj = 90000 Joules
2 kg = 2000 grams
90000 Joules = (2000 g)( SP )(200 C - 80 C)
90000 = 240000(SP)
0.375 J/gC
( The actual specific heat of copper is 0.385 J/gC, so close enough for the problem type )
Wiki User
∙ 13y ago
Anonymous
O.39
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What mass of water can be heated from 25 degrees celsius to 5 degrees celsius by the addition of 2825 joules?
None. Changing water from 25 degrees C to 5 degrees C requires heat to be REMOVED, not added!
When heat is removed from liquid water at 0 degrees C what happens to its temperature?
It gets colder and freezes Actually it first freezes then it gets colder only after it is all frozen.
What is colder water at 0 degrees or ice at 0 degrees?
When you touch some ice, a lot of heat from your skin is first needed to melt the ice. This so-called phase-transition requires a relatively large amount of heat. Once molten, the resulting liquid water will still be 0 deg C, so at that point you have already lost a lot of heat and still have to heat up the 0 deg C water, hence ice appears colder.
If one pound of water is at a temperature of 32 degrees Fahrenheit, how many BTU’s must be removed in order to create a block of ice at 17 degrees?
LATENT HEAT OF FUSION When one pound of ice melts, it absorbs 144 BTUs at a constant temperature of 32°F. If one pound of water is to be frozen into ice, 144 BTUs must be removed from the water at a constant temperature of 32°F.
What are different ways to measure temperature?
You can measure relative heat with a thermometer.The units of temperature (degrees Celsius / kelvins) indicate molecular heat content, while the actual heat energy being generated, added, or removed is measured in joules(newton-meters), a unit of work.
The temperature at which no more energy can be removed from a substance?
The temperature at which no more energy can be removed from a substance is absolute zero, which is 0 Kelvins or -273.15 degrees Celsius.
How much heat in kilojoules must be removed from glass of water that contains 100g of water to lower its temperature from 30 degrees Celsius to 15 degrees Celsius?
6.276 kJ
How much heat in kilojoules must be removed from a glass of water that contains 100g of water to lower it's temperature from 30 degrees Celsius to 15 degrees Celsius?
6.276 kJ
What is the temperature called at no more energy can be removed from matter?
-273.15 degrees Celsius (-459.67 degrees Fahrenheit) is the temperature at which no more energy can be removed from matter.It is called Absolute Zero and marks the 0 for the Kelvin and Rankine scale.
What is the temperature called at which no more energy can be removed from matter?
-273.15 degrees Celsius (-459.67 degrees Fahrenheit) is the temperature at which no more energy can be removed from matter.It is called Absolute Zero and marks the 0 for the Kelvin and Rankine scale.
How many btu's must be removed from 1lb of water at 200 degrees for it to end up as ice at 30 degrees?
There are no units for the temperature. The temperature change could be 230 Celsius degrees or 170 Fahrenheit degrees (94 Celsius degrees). In fact they could be in less commonly used units: eg Reaumur.
What is the temperature called when no Energy can be removed from matter?
That sounds like a description of the temperature known as "absolute zero". This temperature is zero kelvin; it is also approximately -273 degrees Celsius.
How much heat must be removed from a 200 g block of copper to lower its temperature from 150 celsius to 30 celsius?
0.385 Joules/Gram Celsius is the specific heat of copper. So, q(Joules) = mass * specific heat * change in temperature q = (200 g Cu)(0.385 J/gC)(30 C - 150 C) = - 9240 Joules -------------------------amount of heat dissipation ( answer can be positive )
What is the final temperature if 4.00 x 104 joules of energy are removed from 500.0g H2O at 10.0 degrees Celsius?
E = mass x sp ht x Δ°tIn order to calculate the final temperature change, we must also find the temperature change.1. Find the temperature change.Divide joules by (mass x specific heat).Δ°t = 40,000J/500.0g x 4.184J/g°CΔ°t = 19.1°C2. Calculate the final temperature.Tf = 10.0 - 19.1Tf = -9.1°CThere was a decrease in temperature, indicating that it was an endothermic reaction (as energy was removed as stated in the question).
Why does ice at 0 degrees Celsius feel colder to the mouth than water at 0 degrees Celsius?
This is because the ice at 0 deg C is colder to the extent that the latent heat of freezing has been removed from the water at 0 deg C.
What is the final temperature if 200 Joule of heat is removed from 50N block of ice initially at 25 degrees Celsius?
If you can find a block of ice at 25ºC ... or even a picture or a folk legend of one ... I'll go look up the conversion of joules to calories and work this out for you.
What is the melting point of pure ice?
The boiling point of pure water is typically about 100 degrees Celsius. This value can vary based on factors such as pressure. Additionally, impurities in a sample of water can alter its boiling point.
