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September 22, 2014

Search: calculate the final temperature (once the ice has melted) of a mixture made up of initially of 75.0mL liquid water at 29 degrees Celsius and 7.0 g of ice at 0.0 degrees Celsius

Number of results: 60,805

physics
A 87-g ice cube at 0C is placed in 886 g of water at 28C. What is the final temperature of the mixture?
April 17, 2012 by cindy

Physics
A 68-g ice cube at 0C is placed in 796 g of water at 30C. What is the final temperature of the mixture?
September 15, 2012 by shawn

physics
10 kg of ice at -4 C is dropped into 15.1 kg of water at 36 C. What is the final temperature of the mixture? T_final =
May 4, 2014 by Joe

chem
.You have an ice cube that is 150 g and is at a temperature of 0C. You drop the ice into water that is initially at 15C and the ice melts. As a result, the water cools of by exactly 1C to become 14C. How much water was there? In other words, what mass of water at 15C can ...
September 12, 2012 by chuck

Chemistry
Two 20.0g ice cubes at -10.0 C are placed into 275g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
July 9, 2011 by Josh

Physics - ice to liquid
Fifty grams of hot water at 80oC is poured into a cavity in a very large block of ice at 0oC. The final temperature of the water in the cavity is then 0oC. Show that the mass of ice that melts is 50 g. To melt ice to 50g of water, I think that it will take: 50g(334J/g) = 167,...
September 24, 2009 by Ceres

physics
A physical science student adds 500g of 0 degree C ice to 500g of 80 degree C coffee. What is the final temperature of the drink after thermal equilibrium is reached? How much of the ice was melted by the process? Assume coffee has same specific heat as water.
July 17, 2011 by Heat

chemistry
A 2.622 g sample of almonds is ignited and used to melt ice in a can. a. If the almond sample melted 15.24g of ice what is the heat produced in Kcal grams of nuts? d.If the heat from the almond sample was used to heat 100mL of water at 0.0 degree centigrade, what would be the ...
October 15, 2012 by Anthony

physics
A metal container, which has a mass of 9.4 kg contains 14.2 kg of water. A 1.7-kg piece of the same metal, initially at a temperature of 160.0C, is dropped into the water. The container and the water initially have a temperature of 15.0C and the final temperature of the ...
April 16, 2012 by anonymous

Physics
A 10 kg block of ice has a temperature of -13C. The pressure is one atmosphere. The block absorbs 4.10 106 J of heat. What is the final temperature of the liquid water?
April 6, 2008 by Tim

chemistry
A 10 kg block of ice has a temperature of -13C. The pressure is one atmosphere. The block absorbs 4.11 106 J of heat. What is the final temperature of the liquid water?
May 10, 2011 by Anonymous

chemistry (heat of fusion/vaporization)
i need help setting this problem up. You have an insulated container of water that has a temperature of 83.2 C, you continue to add ice until the temperature reaches .6 C and you remove the excess ice, your volume increased by 79.8 mL. What amount of hot water did you have in ...
March 26, 2007 by abby

Chemistry
2. In a calorimeter, 40.0g water at room temperature (20.4 C) was mixed with 60.0 g of water that was initially 48.9 C. The resulting mixture reached a maximum temperature of 37.3 C. Calculate each of the following. a) The heat released by the hot water. b) The heat absorbed ...
April 16, 2013 by Joel

Physics - Heat and phase change
8.94 kJ of energy is available to melt 20 g of ice (initially at 0*C) and subsequently to warm the water. What is the water's final temperature in degrees Celsius?
March 19, 2013 by Jos

chemistry
A 2.622 g sample of almond is ignited and used to melt ice in a can. a. if the almond sample melted 15.24g of ice,What is the heat produced in kcal/gram? b. If the heat from the almond sample was used to heat 100.0 mL of water at 0.0 degree centigrade.What would be the final ...
October 14, 2012 by adonis

physics
If you pour 0.0100 kg of 20.0C water onto a 1.20-kg block of ice (which is initially at −15.0C ), what is the final temperature? You may assume that the water cools so rapidly that effects of the surroundings are negligible.
April 27, 2014 by Mohanad

Chem 212
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 16.1 g, and its initial temperature is -13.3 C. The water resulting from the melted ice reaches the temperature of your skin, 31.3 C. How much heat is absorbed by ...
February 19, 2013 by 1231az

college
A quantity of ice at 0C is added to 65.0 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(gC).
July 14, 2010 by Anonymous

physics
A 1.2 kg block of ice is initially at a temperature of -5C. (a) If 5.8 multiplied by 105 J of heat are added to the ice, what is the final temperature of the system? C (b) Suppose the amount of heat added to the ice block is increased by a factor of 3.0. By what factor must ...
November 22, 2008 by lyd

physics
A 1.2 kg block of ice is initially at a temperature of -5C. (a) If 5.8 multiplied by 105 J of heat are added to the ice, what is the final temperature of the system? C (b) Suppose the amount of heat added to the ice block is increased by a factor of 3.0. By what factor must ...
November 22, 2008 by lyd

Chemistry
Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q =mC*Delta T to calculate the temperature change of the 314 g of water. under the following conditions: A 14.7 g ice cube ...
November 18, 2010 by Ricardo

chemistry
25.6 {\rm mL} of ethanol (density =0.789 {\rm g}/{\rm mL}) initially at 8.0^\circ {\rm C} is mixed with 39.5 {\rm mL} of water (density = 1.0 {\rm g}/{\rm mL}) initially at 23.1^\circ {\rm C} in an insulated beaker. Assuming that no heat is lost, what is the final temperature ...
February 22, 2012 by MD

Chemistry. Please help!!
Calculate the final temperature when a 18.7 gram sample of ice at 0 degrees C is placed into a styrofoam cup containing 113 grams of water at 71.6 degrees C. Assume that there is no loss or gain of heat from the surroundings. Heat of fusion of ice = 333 Jg^-1 Specific heat of ...
March 2, 2012 by JJ

physical chemistry
1.) Calculate delta rH for the freezing of water at one bar and -10 degrees C. The heat capacities are H2O(s)=36.9 JK-1mol-1 and H2O(l)=74.5JK-1mol-1. delta H for freezing of water at 0 degree C is -6602Jmol-1 (assume C is independent of temperature). 2.) Assume the hot brick ...
February 21, 2012 by nicole

chemistry
25.6mL of ethanol (density =0.789 g/mL) initially at 5.4∘C is mixed with 30.4mL of water (density = 1.0 g/mL) initially at 20.4∘C in an insulated beaker.Assuming that no heat is lost, what is the final temperature of the mixture?
September 12, 2014 by Lisa

Chemistry
At room temperature, ethanol's density is 0.789 g/mL while water's density is 0.997 g/mL. When a few milliliters of ethanol are added to water, the two liquids mix. A student is given a unknown liquid at room temperature and experimentally determines its density to be 0.947 g/...
January 16, 2013 by John

math
If i place a dish of ice outside in the sun, The ice has a mass of 0.59 kg and a surface area of 0.039 m2. Assuming that the ice is originally at 0 C and using my answer for part b, which was 1370w/m^2 * 49 * 0.039m^2 = 26.18 watts, How long do i have to wait until all the ...
December 16, 2008 by trigger

chem
Calculate the final concentration of a. 4.0 L of a 4.0 M HNO3 solution is added to water so that the final volume is 8.0L b. Water is added to 0.35L of a 6.0M KOH solution to make 2.0L of a diluted KOH solution. c.A 20.0 mL sample of 8.0% (m/v)NaOH is diluted with water so ...
November 8, 2012 by tracy

Science
Why does the temperature remain constant around 0 degrees C and 100 degrees C? For what? For water when it is freezing or boiling? Or do you have another question in mind? Sorry, it's for water when it is freezing or boiling. Think of it this way. Start with a cup of water. ...
January 4, 2007 by Katie

Physics
Glass of water has mass of 240g at room temp (25C). Add 50g of 0C ice. What final temp after ice is melted. (at equilibrium).
April 26, 2011 by Sue

Material Science
A polystyrene ice chest contains 3 kg of ice at 0 degrees Celsius. Triangle H for melting = 3.34 x 10 to the 5 power J/kg p = 1000 kg/m cubed, CP =4190 J/ (kg K). Heat transfer is limited by conduction (k=0.06W/m K)) from the outside wall at 30 degrees Celsius. This means that...
August 24, 2013 by Joy

physics
A 49-g bullet traveling at 290m/s penetrates a block of ice at 0∘C and comes to rest within the ice.Assuming that the temperature of the bullet doesn't change appreciably, how much ice is melted as a result of the collision? The heat of fusion of water is 333 kJ/kg.
June 4, 2014 by Anonymous

chemistry
29.8 ml of ethanol (density = 0.789 g/ ml) initially at 9.9 degree celsius is mixed with 33.8 mL of water (density = 1.0 g/mL) initially at 27.8 degree celcius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of mixture? How do I start this ...
June 22, 2014 by June

Physics
what is the general relationship between the density of solids and the density of liquids? Are you talking about the density of substance X in the solid state vs the density of the same substance in the liquid state. GENERALLY, solids have a higher density than the ...
October 1, 2006 by Katrina

Chemistry
Several years ago a company invented plastic ice cubes. These were colored plastic cubes with frozen water (or another substances) inside. That way, as the solid melted, it could cool your drink, but did not dilute it with extra water (from the melted ice). If plastic cubes ...
April 24, 2011 by Kat

physics
Suppose that 90 g of hot water at a temperature of 75 degrees C is poured into a cavity in a very large block of ice at 0 degrees C. (a) What will be the final temperature of the water in the cavity? (b) What mass of ice must melt in order for the water to cool down to the ...
April 7, 2011 by sara

chemistry
what is the final temperature of amixture containning 25 grams of ice at -20 degree celciusadded to water at room temperature 22oC mass of water is 50g followed the steps given by you but not getting the answer (0degree celsius) ice at -20 to ice at 0 degree=mcdelta T=25*2.06*...
May 12, 2014 by treasa

physics please help!
Suppose that 90 g of hot water at a temperature of 75 degrees C is poured into a cavity in a very large block of ice at 0 degrees C. (a) What will be the final temperature of the water in the cavity? (b) What mass of ice must melt in order for the water to cool down to the ...
April 8, 2011 by Dan

Science
125 mL of water at 10 C is poured onto a 500 g block of ice at -35 C. Assuming it is a perfectly insulated container, what will be the final temperature of the mixture?
February 10, 2010 by James

Chemistry
When 112 g of water at a temperature of 22.5C is mixed with 65.1 g of water at an unknown temperature, the final temperature of the resulting mixture is 46.3C. What was the initial temperature of the second sample of water?
October 8, 2010 by Noelle

chemistry
A 115 g piece of metal, initially at 60.0 C, is submerged into 100.0 g of water at 25.0 C. At thermal equilibrium, this mixture had a final temperature of 27.0 C. The specific heat capacity of water is 4.18 (J/gC). Use this information to determine the specific heat ...
March 1, 2013 by Brandi

Physics
A 43 g ice cube at 0 C is placed in 882 g of water at 81 C. What is the final temperature of the mixture? The specific heat of water is 4186 J/kg C and its latent heat of fusion is 3.33 105 J/kg . Answer in units of C
April 23, 2013 by dallas

Chemistry
In a thermochemistry experiment the reaction of 0.0857 g of an unknown metal and an excess of 4.0 M HCl resulted in a 0.210 mL decrease in the volume of an ice/water mixture. Calculate the enthalpy of this reaction per 1 g of metal reacted. Needed data: density of water at 273...
December 1, 2007 by Raj

Chemistry HEAT OF FUSION
What is the final temperature, in oC, after a 15.0 g piece of ice, at 0oC, is placed in a styrofoam cup with 128 g of water initially at 74.0oC. Assume there is no transfer of heat to or from the surroundings. The specific heat of water = 4.184 JK-1g-1 The heat of fusion of ...
October 6, 2011 by tanner

Chemistry
Consider the process where 1.3 moles of ice, initially at -30.0 C, is heated to 140.0 C at constant pressure of 1.00 atm. The molar heat capacities (Cp) for solid, liquid, and gaseous water (37.5 J K-1 mol-1, 75.3 J K-1 mol-1, 36.4 J K-1 mol-1, respectively) are assumed to be ...
January 30, 2014 by Bryan Josten

Chemistry
Consider the process where 1.3 moles of ice, initially at -30.0 C, is heated to 140.0 C at constant pressure of 1.00 atm. The molar heat capacities (Cp) for solid, liquid, and gaseous water (37.5 J K-1 mol-1, 75.3 J K-1 mol-1, 36.4 J K-1 mol-1, respectively) are assumed to be ...
January 31, 2014 by Bryan Josten

chemistry
A 32.2 g iron rod, initially at 22.3 C, is submerged into an unknown mass of water at 63.9 C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 58.6 C. What is the mass of the water?
March 19, 2012 by HELP

Chemistry
A 35.0-g iron rod, initially at 25.6C, is submerged into an unknown mass of water at 67.7C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 63.5C. What is the mass of the water?
November 17, 2012 by Matt

Chem...one more time
Ok ok I swear after this I'm done asking questions. It's just that I'm trying so hard to understand all of this, but sometimes it just doesn't make sense to me! So here we go: How many J of energy must be removed when 124.0 g of steam, at a temp. of 167.0 C, is cooled into 124...
May 14, 2007 by Lindsay

Chem
1) A 15.0 g sample of nickel metal is heated to 100.0 C and dropped into 55.0 g of water, initially at 23.0 C. Calculate the final temperature of the nickel and the water, if the specific heat capacity of nickel is 0.444 j / g x C. 2) In a coffee-cup calorimeter, 1.60 g of ...
November 11, 2008 by Kim

CHEMISTRY
Consider the following reaction: 2H2S+SO2=S(s)+H2O A reaction mixture initially containing 0.500M H2S and 0.500M SO2 was found to contain 1.010−3M at a certain temperature. A second reaction mixture at the same temperature initially contains 0.255M H2S and 0.320M SO2. ...
February 14, 2010 by bf

Thermochemistry
A sample of liquid mercury (mass 58 g and temperature 149.0 C) is poured into 79 g of H2O at 19 C. Calculate the final temperature of the mixture, assuming no heat is lost. The heat capacities of Hg and H2O are 27.98 and 75.33 J/mol/K, respectively.
December 2, 2011 by LaurenB

Chemistry
If 75 g of ice at 0.0 Celsius were added to 1.5 L of water at 75 Celsius, what would the final temperature of the mixture be?
July 27, 2010 by Kelly

college chemistry
if 75 g of ice at 0.0 degrees C were added to 1.5 L of water at 75 degrees C what would be the final temperature of the mixture
May 13, 2014 by ashley

Chemistry
25.0 mL of ethanol (density = 0.789 g/mL) initially at 7.0 degrees celsius is mixed with 35.0 mL of water (density = 1.0 g/mL) initially at 25.3 degrees celsius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?
February 9, 2012 by Elle

chemistry
a 14.7g ice cube is placed into 324g og water. calvulate the temperature change in the water upon complete melting of the ice. hint: determine how ,uch heat is absorbed by the melting ice and then use q=mc delta T to calculate the temperature change. use the heat of fusiion ...
May 4, 2010 by janny

chemistry
Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q =mC*Delta T to calculate the temperature change of the 314 g of water. under the following conditions: A 14.7 g ice cube ...
November 17, 2010 by jose

chemistry
A 32.0-g sample of water at 290. K is mixed with 51.0 g water at 310. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
April 21, 2013 by David

Chem
A student measures the following data regarding the heat of fusion of ice: 25.8 g ice at 0.0C is placed into the calorimeter which contains 100.0 g water at 21.7C. The final temperature comes to 1.5C. The calorimeter has a heat capacity of 15.6 J/C. (a) Calculate the ...
January 23, 2013 by Susie

science
3. Liquefied air (assuming it is only O2 and N2) is kept in a container where pressure and temperature can be controlled. a. What is the maximum temperature at which the mixture exists as a liquid? If this temperature is kept constant, what is the minimum pressure to keep the ...
March 11, 2014 by haha

Chemistry (Thermo)
High quality coal (anthracite) is almost pure carbon. The combustion of carbon to carbon dioxide releases 393kJ per mol of carbon burnt. If 1kg of anthracite is burnt: a) How much heat is released? b) How much ice (in kg) at 273K could be melted to give water at 273K? c) How ...
September 10, 2010 by Amy

Physics 2
An unknown substance has a mass of 0.125 kg and an initial temperature of 98.0C. The substance is then dropped into a calorimeter made of aluminum containing 0.285 kg of water initially at 30.0C. The mass of the aluminum container is 0.150 kg, and the temperature of the ...
September 9, 2013 by Emily

Chemistry
If 82.4 g of cold water (initially at 22 C) is mixed in an insulated container with 96 g of hot water (initially at 88 C), what will be the final temperature of the water in C?
April 30, 2014 by Rachel

Chemistry HEAT OF FUSION
What amount of energy is required to melt a 26.9 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg-1 Heat required to melt the ice = J What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC? Specific heat of water = 4.184 JK-1g-1 ...
October 6, 2011 by tanner

physics
Years ago, a block of ice with a mass of about 22kg was used daily in a home icebox. The temperature of the ice was 0.0 degrees Celsius when delivered. As it melted, how much heat did a block of ice that size absorb? The latent heat of fusion of water is 3.34 x 10 ^ 5 J/kg. ...
November 20, 2010 by Norah

physics
A 0.200 kg block of ice at 15C is placed into a pan on a stove, heated to a liquid, and then to vapour with a final temperature of 115C. Calculate the total amount of heat required for this process.
June 3, 2012 by shan

Physics
A 10 kg block of ice has a temperature of -13C. The pressure is one atmosphere. The block absorbs 4.10 106 J of heat. What is the final temperature of the liquid water? I multiplied 10kg by -13 and divided by the heat absored by the block 4.10*10^6 but i can get the right answer
April 5, 2008 by Chris

Chemistry
A 30.0 gram sample of water at 280. K is mixed with 50.0 grams of water at 330. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
October 12, 2010 by Anonymous

chemistry
Calculate the final temperature of 289 of water initially at 35 upon absorption of 20 of heat.
October 7, 2011 by jasmin

Chemistry
Calculate the final temperature of 244 of water initially at 35 upon absorption of 20 of heat
February 5, 2013 by KJ

chemistry
When 86.7 g of water at a temperature of 73 C is mixed with an unknown mass of water at a temperature of 22.3 C the final temperature of the resulting mixture is 61.7 C. What was the mass of the second sample of water? (Specific heat of water 4.184 Jg-1C-1)
April 9, 2013 by Anonymous

chemistry
When 86.7 g of water at a temperature of 73 C is mixed with an unknown mass of water at a temperature of 22.3 C the final temperature of the resulting mixture is 61.7 C. What was the mass of the second sample of water? (Specific heat of water 4.184 Jg-1C-1)
April 9, 2013 by Anonymous

chemistry
What is the melting point of a mixture of 2.00 lb of NaCl and 12.00 pounds of ice if exactly half of the ice melts? Assume that all the NaCl disolves in the melted ice and that the van't Hoff factor for resulting solution is 1.44.
September 11, 2012 by Wiped

Science
The total amount of ice in the Greenland ice sheet is estimated to be 2.85 million cubic km. Assume the Earth's surface is 70% covered by ocean, and that the Earth's radius is 6300 km. How many meters would sea level rise if the entire Greenland ice sheet were to melt? (You ...
March 19, 2014 by Bane Havoc

chemistry
cold water mass of calimeter+ water: 68.66g mass of calimeter: 19.19g mass of water: 49.47g final temperature of water: 39.1C initial temperature of water: 25.5C delta(T) of water: 13.6C hot water mass of calimeter+ water: 79.55g mass of calimeter: 20.61g mass of water: 58.94g...
November 30, 2011 by Yuli

Chemistry Urgent
95.0mL of H2O is initially at room temperature (22.0∘C ). A chilled steel rod at 2.0∘C is placed in the water. If the final temperature of the system is 21.3∘C , what is the mass of the steel bar? Specific heat of water = 4.18 J/g⋅∘C Specific heat...
March 11, 2014 by Anna

chemistry
Data collected from the calorimetry of a metal mass of the metal = 110.62g initial temperature of the water in the cup = 23.0 C initial temperature of the metal in the boiling water = 99.02 C final temperature of the metal AND water in the cup=25.54C volume of the water =100....
June 5, 2010 by coco

physics
Given: latent heat of fusion of water 3.33x10^5 J/kg. A 147 g cube of ice at 0 degress C is dropped into 1.3 kg of water that was originally at 79 degrees C. What is the final temperature of the water after the ice melts.
December 8, 2009 by Ericka

Chemistry
22.) The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/gC. (1) What quantity of heat is required to melt 25.0 g of ice at 0C? (2) What quantity of heat is required to ...
March 5, 2013 by Adriana

THERMOCHEMISTRY
An ice hotel that is made of 410 metric tons of ice and 12200 metric tons of snow is being melted. The company is going to siphon the melted water into nearby streams. The company is using large industrial sized acethylene to do the job. Your job is to order the rigth amount ...
February 21, 2012 by JAMES

Chemistry
Two 20.0-g ice cubes at 20.0 C are placed into 295 g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Heat capacity of H2O(s)=37.7J Heat capacity of H2O(l)=75.3J Enthalpy...
June 27, 2013 by Jessica

Chemistry
A dry mixture of kno3 and sand could be separated by 1. adding water to the mixture and filtering 2. adding water to the mixture and evaporating 3. heating the mixture to a high temperature 4. cooling the mixture to a low temperature
April 13, 2009 by .

Physics
5) An insulated Thermos contains 190 cm3 of hot coffee at 79.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it ...
November 14, 2010 by john

physics
An insulated Thermos contains 140 cm3 of hot coffee at 89.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were ...
December 4, 2011 by mar13

physics
An insulated Thermos contains 140 cm3 of hot coffee at 89.0C. You put in a 11.0 g ice cube at its melting point to cool the coffee. By how many degrees (in Celsius) has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were ...
December 4, 2011 by mar13

Thermochemistry
If a chalice made of pure gold weighing 1.24 kg and initially at 15 C is filled with 100.0 mL of water at 89 C, what is the final equilibrium temperature of the system? The heat capacities of water and gold are 75.29 and 25.42 J/mol/K, respectively.
December 2, 2011 by LaurenB

Chemistry
When preparing home-made ice cream, salt is added to the ice-water mixture. What is its function and why does it work?
March 8, 2012 by teetee

Final Temperature
A sample of steam with a mass of 0.553 g and at a temperature of 100 degrees C condenses into an insulated container holding 4.25 g of water at 4.0 degrees C. Assuming that no heat is lost to the surroundings, what will be the final temperature of the mixture?
January 15, 2013 by Amy

thermodynamice
A cylinder contain 3 kg of water and water vapor mixture in equilibrium at a pressure of 500 KN/m^2. If the volume of the cylinder is 1.0 m^3, calculate the following. A)temperature of the mixture B) the volume and mass of the liquid C)The volume and mass of the vapor
January 8, 2011 by chris

Chemistry
Calculate the final temperature of 283 mL of water initially at 30 degrees celcius upon absorption of 19 kJ of heat
September 15, 2010 by Anonymous

Reading
How do I Calculate the final temperature of 299ml of water initially at 31 degrees upon absorption of 19kj of heat?
March 4, 2012 by Denise

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

Melting Ice Chemistry
You have an ice cube (H2O) that weighs 5 grams and is at a temperature of -10 degrees Celsius. How much heat energy(in joules) is required to melt the ice cube and raise the temperature of the resulting liquid water to 15 degrees Celsius? A. 1803 J B. 2088.5 J C. 257.5 J D. ...
June 14, 2013 by Josh

physics
Consider 60 g of hot water at 70 degree C poured into a cavity in a very large block of ice at 0 degree C. A)What will be the final temperature of the water in the cavity? B)Find what mass of ice must melt in order to cool the hot water down to this temperature
April 3, 2012 by christy

Chemistry
How would I calculate this? 30.0 mL of pure water at 280. K is mixed with 50.0 mL of pure water at 307 K. What is the final temperature of the mixture?
June 30, 2013 by Mary

chemistry
Two 20.0 g ice cubes at -16.0 C are placed into 285 g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of H2o(s)-->37.7 heat capacity of H2o()-->75.3 ...
June 27, 2013 by Jill

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