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December 18, 2014

Search: specific heat

Number of results: 9,640

chemistry
An electric range burner weighing 614 grams is turned off after reaching a temperature of 499.0oC, and is allowed to cool down to 22.2oC. Calculate the specific heat of the burner if all the heat evolved from the burner is used to heat 565 grams of water from 22.2oC to 80.9oC.
January 25, 2012 by jayla

Chemistry
An 850 gram chunk of ice at 0 degrees Celsius is dropped into a container holding 1.7 kg of water at an initial temperature of 35 degrees Celsius. Due to the presence of the ice, the temperature of the water eventually drops to 0 degrees Celsius. Show a mathematical solution ...
January 29, 2012 by Selena

Chemistry
A 5.80 g sample of SiH4 and an excess of oxygen were placed in a reaction container surrounded by 3.40 kg of water. The initial temperature of the water was 14.10C. At the end of the reaction, the temperature of the water was 48.90C. Assume the heat was completely absorbed ...
March 8, 2010 by Megan

physics
When 1180 J of heat are added to one mole of an ideal monatomic gas, its temperature increases from 272 to 292 K. Find the work done by the gas during this process. I know the specific heat is Q/delta T, so C = (1180 J)/(20K) = 59. This seems like any easy problem, but now I'm...
June 22, 2007 by tmaria

Science
A 50 gram ice cube is cooled to -10oC in the freezer. How many calories of heat are required to heat it until it becomes liquid water at 20oC? (The specific heat of ice is 0.5 cal/goC.) Answer A) 1250 cal. B) 4000 cal. C) 5000 cal. D) 5250 cal. Can someone please help me solve...
September 26, 2011 by Anonymous

physics
A 50 gram ice cube is cooled to -10oC in the freezer. How many calories of heat are required to heat it until it becomes liquid water at 20oC? (The specific heat of ice is 0.5 cal/goC.) Answer A) 1250 cal. B) 4000 cal. C) 5000 cal. D) 5250 cal. Can someone please help me solve...
September 26, 2011 by Allison

Physics
When 2.1x10^3 J of heat is added to 100.g of a substance, its temperature increases from 15 C to 40 C. What is the specific heat capacity of the substance? Answer is 8.4x10^2 but I need to see the work involved in how to solve the problem
December 8, 2011 by Dorrito

Chemistry lab
In my lab class I am having to write a lab experiment and preform it tomorrow. It deals with specific heat of unknown metal and density. the first part you have boil water with the metal in it, and then put it in a cup and measure the temp change. I have completed to specific ...
November 5, 2012 by Paco

Chemistry
Need help with my lab report for specific heat of unknown metal! I need to Find the Specific Heat of Al! I know its Q= M x Cs x Change in Temp I am getting a such a high number am just confused if its right. Here is what I got in Lab: Aluminum Mass of Metal (Mm): 6.128g Mass ...
June 24, 2011 by Tc

Chemistry - General, Hess's Law
In an experiment, 11.6g of a salt was dissolved in 100.0ml of water contained in the above calorimeter, all at an initial tmperature of 24.5 degrees Celsius. After dissolution was complete, the temperatur was 31.8C. The specific heat of the solution is 3.63J/gxC and the ...
July 24, 2009 by Sahar

physics
Dry saturated steam at 100 degree C is passed into 250 gm of a mixture of ice and water contained in a calorimeter of thermal capacity 45J/K.When all the ice has just melted,the mass of the content has increased by 10 gm due to condensed steam.Assuming no heat exchange between...
March 15, 2012 by AFOLABI .O.

physics
In lab, Will burns a 0.6 g peanut beneath 48 g of water, which increases in temperature from 22 degree C to 55 degree C. The amount of heat absorbed by the water can be found with the equation Q =cm \Delta T, where Q is the amount of heat, c the specific heat of water, m the ...
March 31, 2012 by christy

Chemistry
If 150.0 grams of iron at 95.0 degrees Celcius, is placed in an insulated container containing 500.0 grams of water at 25.0 degrees Celcius, and both are allowed to come to the same temperature, what will that temperature be? The specific heat of water is 4.18 J/g degrees ...
February 22, 2012 by Chloe

Chemistry Help!!!
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

chemistry
a chunk of pure silver has a heat capacity of 42.8J/degrees celsius and a mass of 181g. calculate the specific heat of silver. can you show me how to solve it? please dont just give an answer
January 20, 2010 by verlee

Physics
Please help! Suppose that a 400 gram copper object (specific heat 0.092 cal/g/degrees Celsius) receives 900 cal. of heat. What is the temperature change? Explain your reasoning. Thanks
March 2, 2011 by A

Physic II
A 992.0-g iron meteor impacts the earth at a speed of 1447.0 m/s. If its energy is entirely converted to heat of the meteorite, what will the resultant temperature rise be? (The specific heat for iron is 113 cal/kg.C)
April 7, 2014 by Guliner

chemist
If 50.0 g of benzene, C6H6, at 25.0 C absorbs 2.71 kJ of energy in the form of heat, what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g ⋅K.
December 26, 2012 by gsdgsd

science
A 15.0 gram lead ball at 25.0C was heated with 40.5 joules of heat. Given the specific heat of lead is 0.128 J/g∙C, what is the final temperature of the lead?
February 6, 2013 by Suizaranne

western michigan university
A 30 gram metal at 100 degrees Celsius was dropped into 132 grams of water at 25 degrees Celsius and the final temperature for the metal in water system was 29 degrees Celsius. Calculate the specific heat capacity of the metal if the specific heat capacity of water is 4.2J/G/C...
December 6, 2012 by lorena

science
as 390 g of hot milk cools in a mug, it transfers 30,000 J of heat to the environment. What is the temperature change of milk? The specific heat of milk is 3.9 J/g degree C.
October 28, 2011 by Justin

ap chemistry
Calculate the energy required to heat 827 g of mercury from 37 ◦C to 42 ◦C. The specific heat capacity of Hg() is 0.138 J/g ◦ C. Answer in units of calories
October 22, 2013 by gabriella

chemistry
A 45 g block of aluminum initially at 28.0 C absorbs 548 J of heat. What is the final temperature of the aluminum? The specific heat of aluminum is 0.902 J/g C.
April 25, 2013 by University of Louisiana at Lafayette

Pam
A 56.59 g sample of a substance is initially at 20.5 C. After absorbing 1267 J of heat, the temperature of the substance is 116.5 C. What is the specific heat (c) of the substance?
December 5, 2013 by Chemistry

Chemistry
When pure sulfuric acid is dissolved in water,heat is evolved.To a calorimeter containing 300g of water at 20degree C,10.65g of sulfuric acid also added at the same temperature.The change in temperature,which was monitored by a digital probe with negligible heat capacity ...
March 22, 2012 by Meenaakshi

Chemistry
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

Chemistry
1) When hydrazine (N2H4) is burned in a 253-g brick container, the temperature of the brick increases by 5.13 degrees Celsius. Calculate the quantity of heat released in this raection. The specific heat of brick is 0.840 J/(gC). 2) A sample of coal is burned in a bomb ...
November 14, 2010 by Sarah

Chemistry
Calculate the number of joules required to melt 57.4g of benzene at 5.5 degrees celsius? The heat of fusion for benzene is 9.87 KJ/mol and specific heat for liquid benzene is 1.63 J/g*deg)
February 19, 2010 by Jake

Chemistry
How much heat is lost when 12.4 g of H2O g at 110 degrees C are converted to liquid at 50.0 degrees C? (The specific heat of steam is 2.02 J/g degrees C. Could someone write the steps? Equation?
May 24, 2010 by Anonymous

science
gold has a specific heat of 0.130j/g. degrees celcuis if 195 joules of heat are added to 15 grans of gold homw much does the tempreature of the gold change
March 1, 2011 by nikita

chemistry
How much heat (in Joules) is gained by the water when a chemical reaction takes place in 100.0 ml aqueous solution, has a temperature increase of 10.20C and a specific heat capacity of 4.180 J/Cg? [Hint: ignore any effects of the calorimeter and solve for qwater]
March 31, 2014 by shelle

Chemistry
If 72.4 kJ of heat is applied to a 95.2 g block of metal, the temperature of the metal increases by 10.7 C. Calculate the specific heat capacity of the metal in J/g C?
May 4, 2011 by Mystery Mania

Physics
why are you not harmed by the greater-than-1000C sparks from a Fourth of July-type sparkler? The sparks, while hot (high temperature), have little heat in them (low thermal capacity, or specific heat).
March 22, 2007 by Naomi

Physics
The latent heat of vaporizaiton of H2O at body temperature (37.0C) is 2.42 106 J/kg. To cool the body of a 89 kg jogger (average specific heat capacity = 3500 J/(kgC)) by 1.4 C, how many kilograms of water in the form of sweat have to be evaporated?
April 4, 2008 by Pierce

Chemistry105
When 50.0 Ml of 1.00 m chi was mixed with 50.0 ml of 1.00 m NaOH in a calorimeter the temperature rose from 25.0 c to 32.0 c calculate the heat change for the reaction assuming that the total volume of the solution is 100.0 ml and the specific heat is 1.00 cal/ (g.c). Is the ...
December 2, 2012 by Mira

Chemistry105
When 50.0 Ml of 1.00 m chi was mixed with 50.0 ml of 1.00 m NaOH in a calorimeter the temperature rose from 25.0 c to 32.0 c calculate the heat change for the reaction assuming that the total volume of the solution is 100.0 ml and the specific heat is 1.00 cal/ (g.c). Is the ...
December 2, 2012 by Mira

Physics
The latent heat of vaporization of H2O at body temperature (37C) is 2.42 x 106 J/kg. To cool the body of a 77.6-kg jogger [average specific heat capacity = 3500 J/(kg C)] by 2.78 C, how many kilograms of water in the form of sweat have to be evaporated?
December 5, 2012 by StressedStudent

Physics
The latent heat of fusion of alcohol is 50 kcal/kg and its melting point is -54oC. It has a specific heat of 0.60 in its liquid state. Calculate the energy needed to melt 2.0 kg of solid alcohol at -54o and raise it to a temperature of -4C.
June 18, 2013 by Isis

Chemistry
I don't know how to do this question, or even start it. Please Help. 2 kg copper kettle (specific heat capacity 0.385j/gC) has .0500 kg of water at 20C. How much heat is needed to raise the temperature of the kettle and content to 80C?
November 27, 2014 by Sandy

chemistry
How many calories must be supplied to 59 g of ice at −6 C to melt it and raise the temperature of the water to 61 C? The specific heat of ice is 0.49 kcal/kg K and of water is 1 kcal/kg K; the heat of fusion of water is 79.7 kcal/kg, and its heat of vaporization is ...
March 1, 2012 by anonymous

chemistry
When hydrazine (N2H4) is burned in a 259-g brick container, the temperature of the brick increases by 5.13 C. Calculate the quantity of heat released in this reaction. The specific heat of the brick is .840 J/(g C)
October 20, 2011 by n

ap chemistry
Consider the specific heats H2O(s) =2.09 J/g ◦C,H2O () = 4.18 J/g ◦C, and H2O(g) = 2.03 J/g ◦C. The heat of fusion for water is 334 J/g and its heat of vaporization is 2260 J/g. Calculate the amount of heat required to convert 92 g of ice at −13...
October 22, 2013 by gabriella

chemistry
How many gallons of C6H12 , measured at 20 degrees Celsius, must be burned to provide enough heat to warm 26.4m3 of water from 17.4 degrees Celsius to 32.8 degrees Celsious , assuming that all the heat of combustion is transferred to the water, which has a specific heat of 4....
December 9, 2012 by Anonymous

ap chemistry
Consider the specific heats CH2O(s) = 2.09 J/g ◦ C. CH2O() =4.18 J/g ◦ C. CH2O(g) = 2.03 J/g ◦ C. The heat of fusion for water is 334 J/g and the heat of vaporization for water is 2260 J/g. Calculate the amount of heat absorbed when 86 g of steam at ...
October 22, 2013 by gabriella

Physics
Dry saturated steam at 100'C is passed into 250gm of a mixture of ice and water contained in a calorimeter of thermal capacity 45J/K.When all the ice has just melted,the mass of the content of the calorimeter has increased by 10gm due to condensed steam.Assuming no heat ...
March 11, 2012 by O.E Olaleye

Physics
What is the final equilibrium temperature when 7 g of milk at 5C is added to 117 g of coffee at 68C? Assume the specific heats of milk and coffee are the same as that of water, and neglect the specific heat of the container. Answer in units of C
March 13, 2013 by Ted

science
A copper calorimeter of mass 150g, was half filled with water of mass 300g and temperature 0 degrees celcius. 5g of ice at 0 degrees celcius was added to the content, later some quanity of steam was passed into the mixture and the temperature rose by 20 degrees celcius. ...
March 2, 2014 by Tomex

chemistry
95.0mLmL of H2O\rm H_2O is initially at room temperature (22.0∘C\rm{} ^{\circ}C). A chilled steel rod at 2.0∘C\rm ^{\circ}C is placed in the water. If the final temperature of the system is 21.3∘C^{\circ}C, what is the mass of the steel bar? Specific heat of ...
March 11, 2014 by Anna

chemistry
A chunck of silver has a heat capacity of 42.81 J/C. If the silver has a mass of 181 g, calculate the specific heat of silver.
May 3, 2011 by Anonymous

CHEM
Suppose that the microwave radiation has a wavelength of 10.8 cm. How many photons are required to heat 225 mL of coffee from 25.0*C to 62.0*C ? Assume that the coffee has the same density, 0.997 g/mL , and specific heat capacity, 4.184 J/(gK), as water over this temperature ...
March 11, 2010 by baubi

chemistry
Suppose that the microwave radiation has a wavelength of 10.8 cm. How many photons are required to heat 225 mL of coffee from 25.0*C to 62.0*C ? Assume that the coffee has the same density, 0.997 g/mL , and specific heat capacity, 4.184 J/(gK), as water over this temperature ...
October 25, 2010 by randy

Chemistry
Suppose that the microwave radiation has a wavelength of 12.4 cm. How many photons are required to heat 255 mL of coffee from 25.0 C to 62.0 C? Assume that the coffee has the same density, 0.997 g/mL, and specific heat capacity, 4.184 J/(g/ K), as water over this temperature ...
October 27, 2010 by tommy

Physics
Please help! Suppose that a 400 gram copper object (specific heat 0.092 cal/g/degrees Celsius) receives 900 cal. of heat. What is the temperature change? Explain your reasoning. Do not use algebra Thanks!
March 1, 2011 by A

chemistry
1. Heat can initiate reaction as well as be a product of chemical reactions. Cite the specific sample from the experiment that show heat acting in the manner. 2. Aluminum chloride was a product in step 6. How could you instruct your lab partner to recover it
March 8, 2012 by jhong

chemistry
1. Heat can initiate reaction as well as be a product of chemical reactions. Cite the specific sample from the experiment that show heat acting in the manner. (this is for recycling a copper using a copper nitrate, sodium hydroxide and HCL)
March 8, 2012 by jhong

chemistry
1. Heat can initiate reaction as well as be a product of chemical reactions. Cite the specific sample from the experiment that show heat acting in the manner we are experimenting a copper II nitrate, sodium hydroxide and HCL for recyling a copper
March 9, 2012 by jhong

Math
I'm trying to help my nephew with some homework and am hopeless. Please help with these questions: If 180 calories of heat were added to 50 grams of copper, what would the change in temperature be? (specific heat of copper = .09) What would the temperature of the copper be if ...
March 4, 2007 by Diane

Chemistry
How much heat is required to convert 32.5 grams of ethanol at 28 C to the vapor phase at 78 C? Ethanol (C2H5OH) boils at 75 C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g-K.
February 11, 2010 by Anonymous

Physics Entropy Project
We did a lab in class where we heated a nail, and our goal was to determine the total increase in entropy of the system. I have all of the measurements but I'm not sure how to go about figuring out the change in heat (delta Q). delta S = delta Q / delta T (S=Q/T) Here are all ...
January 27, 2010 by George

Chemistry
A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20 C. After stirring, the final temperature of both copper and water is 25 C Assuming no heat losses, and that the specific heat (capacity...
November 16, 2012 by Natalie

Chemistry
A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20 C. After stirring, the final temperature of both copper and water is 25 C Assuming no heat losses, and that the specific heat (capacity...
November 16, 2012 by Natalie

Chemistry
A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20 C. After stirring, the final temperature of both copper and water is 25 C Assuming no heat losses, and that the specific heat (capacity...
November 16, 2012 by Natalie

Chemistry
A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20 C. After stirring, the final temperature of both copper and water is 25 C Assuming no heat losses, and that the specific heat (capacity...
November 16, 2012 by Natalie

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat of...
February 27, 2012 by Abby

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat ...
February 27, 2012 by Abby

Physics
How much heat is required to melt 50 g of mercury at -45 degrees celsius to 425 degrees celsius. (melting point=-38.degree-c, specific heat=0.03325 cal/g-degree c for solid mercury, .2988 cal/g-c degree c for liquid mercury and .2486 cal/g-c degree for gaseous mercury, heat ...
February 27, 2012 by Abby

chem
Suppose that the microwave radiation has a wavelength of 10.8cm . How many photons are required to heat 295ml of coffee from 25.0 C to 62.0 C? Assume that the coffee has the same density, 0.997g/ml , and specific heat capacity, 4.184J/(gk) , as water over this temperature range
November 11, 2011 by Anna

Chemistry
A cup of teat containing 400g of liquid at 20 degrees celsius was heated. If 58.5 kj of heat was absorbed by the tea, what would the final temperature be? Assume that the specific heat of the tea is the same as that of water (4.18). I am not sure how to start this problem.
January 21, 2012 by Hannah

AP Chem
I missed a lab in class a week ago and had to make it up just the other day. My teacher didn't have time to explain the lab to me, so he gave me a brief overview of the procedure. The objective of the lab was to calculate the specific heat of an unknown block of metal. The ...
February 8, 2007 by Jess

chemistry
Calculate the amount of heat absorbed when 58 g of steam at 117◦C are completely converted to ice at −32.5◦C. Specific Heat: H2O(s) = 2.09 J/g◦C H2O(l) = 4.18 J/g◦C H2O(g) = 2.03 J/g◦C Heat of Fusion = 334 J/g Heat of Vaporization = 2260 J/g...
November 15, 2014 by Q

college chemistry
what is the specific heat of a substance that required 800 joules of heat to raise the temperature of 50 grams of it from 20 degrees Celsius to 30 degrees Celsius?
December 4, 2012 by airy

chemistry
If 145 J of heat energy is applied to 34.47 g of an unknown metal, the temperature increases from 61.0 degree C to 78.5 degrees C. What is the specific heat capacity of the unknown metal?
January 31, 2013 by Max

physics
When a lead bullet hits a solid target at high speed, its entire kinetic energy is converted into heat. For simplicity, assume that all the heat is concentrated in the bullet rather than the target. If the bullet's initial temp. is 20` C, how fast should it be moving before ...
February 19, 2010 by elisabeth

chemistry
If a 5.26-g sample of copper at 258 C is placed in 125 mL of water at 21.0 C, how hot will the water get? Assume no heat loss to the surroundings. The specific heat of copper is 0.385 J/g C.
October 23, 2008 by Lilit***

chemistry
If the heat of combustion for a specific compound is -1460.0 kJ/mol and its molar mass is 55.75 g/mol, how many grams of this compound must you burn to release 900.20 kJ of heat?
April 5, 2012 by catey

Chemistry
If the heat of combustion for a specific compound is -1320.0 kJ/mol and its molar mass is 92.41 g/mol, how many grams of this compound must you burn to release 544.30 kJ of heat?
October 9, 2012 by Anonymous

chemistry
If the heat of combustion for a specific compound is -1310.0 kJ/mol and its molar mass is 75.45 g/mol, how many grams of this compound must you burn to release 708.60 kJ of heat?
October 21, 2012 by :)

Chemistry
If the heat of combustion for a specific compound is -1010.0 kJ/mol and its molar mass is 46.03 g/mol, how many grams of this compound must you burn to release 388.00 kJ of heat?
March 27, 2013 by Anonymous

Chem
If the heat of combustion for a specific compound is -1170.0 kJ/mol and its molar mass is 42.75 g/mol, how many grams of this compound must you burn to release 191.90 kJ of heat?
July 13, 2014 by Anonymous

science
100.0g of 4.0c water is heated until its temperature is 37c. if the specific heat of water is 4.18 j/g c, calculate the amount of heat energy needed to cause this rise in temperature.
August 25, 2014 by henry

heat of vaporization
Suppose that 1.00 g of rubbing alcohol (C3H8O) evaporates from a 54.0 g aluminum block. If the aluminum block is initially at 25 C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization of the ...
January 16, 2010 by Kyle

chem-calorimetry
If a 5.26-g sample of copper at 258C is placed in 125mL of water at 21.0C, how hot will the water get? Assume no heat loss to the surroundings. The specific heat of copper is .385 J/g C
March 31, 2008 by natash

chemistry
how do u calculate the specific heat of a metallic element if 314 joules of heat energy are needed to raise the temperature of 50.0g sample from 25.0 degrees Celsius to 50.0 degrees Celsius?
December 17, 2009 by gg

chemistry
Aluminum has a specific heat capacity of 0.903J/g degree celsius. What mass of aluminum in g would require 500j of heat to raise its temperature by 12.5 degrees celsius
March 22, 2011 by mary

Physical Science
Ninety kilojoules of heat were added to a 2.0-kg piece of wood whose temperture then rose from 20 degrees Celsius to 48 degrees Celcius. What was the specific heat of the wood?
September 18, 2011 by Jaskson

Multon Middle
A 5. pellet of aluminum at 20 degrees celcius gains 200 joules of heat. What is its final temperature? [specific heat of Aluminium, c=920 j/Kg. degrees celcius)
February 5, 2012 by j nager

Chemistry (balance)
if the heat of combustion for a specific compound is -1320.0 KJ/mol and its molar mass is 67.53 g/mol how many grams of this compound must you burn to release 791.60 kj of heat
August 20, 2012 by Jacob

intro to physical science
the specific heat of granite is 0.80 KJ/kg . c. I f 1.6 MJ of heat are added to a 100-kg granite statue of James Precott Joule that is originally at 18 C, what is the finale temperature of the statue
February 11, 2013 by Chris

Chemistry
If the heat of combustion for a specific compound is -1080.0 kJ/mol and its molar mass is 58.29 g/mol, how many grams of this compound must you burn to release 300.60kJ of heat?
October 29, 2013 by Patricia

physics
1 kg of ice at 0 C is mixed with 9 kg of water at 50 C (The latent heat of ice is 3.34x105 J/kg and the specific heat capacity of water is 4160 J/kg). What is the resulting temperature?
January 23, 2011 by calous --- HELP PLEASEE!!!

Physical Science
A 100 kg sample of a metal is cooled from 100C to 20C by removing 20 kcal of heat. Calculate the specific heat capacity of the metal.
October 12, 2012 by Anna

Physical Science
A 100 kg sample of a metal is cooled from 100C to 20C by removing 20 kcal of heat. Calculate the specific heat capacity of the metal.
October 12, 2012 by Anna again...help!

Physics
If the air temperature is the same as the temperature of your skin (about 30 degrees Celcius), your body cannot get rid of heat by transferring it to the air. In that case, it gets rid of the heat by evaporating water (sweat). During bicycling, a typical 71.0 kg persons body ...
November 21, 2008 by Angel

Lauren
The specific heat of water is at 4.184J/g * degree C. How much heat is evolved, or absorbed, when the temperature of 9.00 mol of liquid water cools from 38 degrees C to 28 degrees C? How do I start this problem
November 16, 2007 by Chemistry

Chemistry
Calculate the specific heat of a metallic element if 314 jouldes of heat energy are needed to raise the temperature of a 50g sample from 25 degrees Celcius to 50 degrees Celcius?
May 25, 2009 by ASK

physicss
A 0.190 kg piece of copper is heated and fashioned into a bracelet. The amount of energy transferred as heat to the copper is 6.62 x 10^4 J. If the specific heat of copper is 387 J/kg x C, what is the change in temp of the copper?
November 1, 2009 by arriell

phys
A 0.190 kg piece of copper is heated and fashioned into a bracelet. The amount of energy transferred as heat to the copper is 6.62 x 10^4 J. If the specific heat of copper is 387 J/kg x C, what is the change in temp of the copper?
November 2, 2009 by abbigail

physics
The specific heat capacity of copper is 0.092 calories per gram per degree Celsius. How much heat is required to raise the temperature of a 5 g piece of copper from 0C to 80C?
December 13, 2009 by FALLON

Chemistry
Calculate the final temperature when 20.0 g at 60 *C iron is put into 50.0 ml of 20 *C water. The specific heat of iron is 0.449 J/g*C and that of water is 4.184*C. (Assume no heat is lost to the container or the surrounndings.)
November 29, 2010 by Stacy

Oceanography
A 15.75-g piece of unknown metal absorbs 60 cal of heat energy, and its temperature changes form 25 degrees C to 175 degrees C. Calculate the specific heat capacity of this metal.
September 28, 2011 by bj

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