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April 18, 2014

Search: Calculate the amount of heat (in kJ) required to convert 87.5 g of water to steam at 100°C.

Number of results: 79,700

Chemistry
Portions may be right but most steps leave out something. Here is how you do it. q1 = heat to move T of ice from -20 to zero C. q1 = mass ice x specific heat ice x (Tfinal-Tinitial). Tfinal = 0 and Tinitial = -20; therefore, Tfinal-Tinitial = 0 -(-20) = +20. q2 = heat to melt ...
Monday, November 15, 2010 at 7:40pm by DrBob222

Chemistry
A 2.839-g sample of C2H4O was burned in a bomb calorimeter whose total heat capacity is 16.77 kJ/C. The temperature of the calorimeter increases from 22.62C to 26.87C. What is the heat of combustion per mole of C2H4O?
Monday, September 17, 2012 at 9:08pm by Nisah

chemistry
1. a) 50ml of water at 46.9C were mixed with 50ml of water at 25.1C in a calorimeter also at 25.1C. The final temperature was 30.1C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the ...
Monday, November 12, 2012 at 2:21pm by Cicily

chemistry/please double check
Hi, I just need to know if I finally got this exercise right. Calculate the amount of heat in kilojoules released when 50 grams of steam at 125 Celsius are converted to 50 grams of ice at -125 Celsius. so, qw= 50*4.184J/g C (125 C-o)= 26.15 x 10^3 qi= 50*2.09*(-125)=-13.065 KJ...
Tuesday, October 28, 2008 at 8:02pm by Joshua

Chemistry
ok on the 4.19. The middle term is negative because it is losing heat. Remember something giving off heat is -. Absorbing heat is +. The mass*C*delta T thing takes care of the sign automatically when you use Tfinal-Tinitial (it makes both of those terms negative BECAUSE Tfinal...
Wednesday, February 17, 2010 at 11:07pm by DrBob222

Chemistry
A 300.0g sample of ice at -30.OC is mixed with 300.0G of water at 90C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capazities of H2O(s) and H20(L) are 2.03 and 4.18 j/g*C respectivly, and the entahply fusion for ice is 6....
Friday, February 24, 2012 at 12:47am by Keru

Check 1 question.
Help please!i'm not sure if i'm right. Honestly i'm not that confident about most of my work. In which of the following thermochemical equations would the deltaH be considered a heat of solution? C6H6 (s)--> C6H6 (l), deltaH = +9.87 kJ 2C8H18(l) + 25O2 (g)-->16CO2 (g...
Friday, June 22, 2012 at 1:39pm by Anonymous

chemistry
An insulated beaker with negligible mass contains liquid water with a mass of 0.255{kg} and a temperature of 76.0{C} How much ice at a temperature of -19.9 C must be dropped into the water so that the final temperature of the system will be 32.2? Take the specific heat of ...
Monday, December 7, 2009 at 12:58pm by dan

chemistry
Given the thermochemical equation 2SO2(g) + O2(g) → 2SO3(g), ΔH= -198 kJ/mol, how much heat is evolved when 600. g of SO2 is burned? A. 5.46 x 10-2 kJ B. 928 kJ C. 1.85 x 103 kJ D. 59,400 kJ E. 3.71 x 103 kJ
Tuesday, October 9, 2012 at 5:21pm by Anonymous

chemistry
When 0.667 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 108C is observed. Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC. what is the molar heat of reaction, H rxn, for the ...
Wednesday, February 17, 2010 at 6:14pm by blasting

Chemistry
One mole of carbon (12.0 g) in the form of crystalline graphite is burned at 25 ◦ C and 1.000 atm pressure to form CO2(g). All of the heat produced is used to heat a 4560 g bath of liquid water, originally at 25 ◦ C. What is the final temperature of the water...
Sunday, October 7, 2012 at 7:53pm by Austin

chemistry
calculate the amount of heat necessary ti raise the temperature of 8.5kg of water from 12.5 to 84 degrees C
Tuesday, May 4, 2010 at 8:18pm by Quentin

Chemistry
Calculate the amount of energy in kilojoules needed to change 225 g of water ice at -10 C to steam at 125 C. The following constants may be useful: Cm(ice)=36.57 J/(mol*C) Cm(water)=75.40 J/(mol*C) Cm(steam)=36.04 J/(mol*C) Delta H(fus)=+6.01 kJ/mol Delta H(vap)=+40.67 kJ/mol
Saturday, April 17, 2010 at 8:46pm by Eddie

chemistry
LP gas burns according to the exothermic reaction: C3H8(g) + 5 O2(g) right arrow 3 CO2(g) + 4 H2O(g) ΔHrxn = −2044 kJ What mass of LP gas is necessary to heat 1.2 L of water from room temperature (25.0C) to boiling (100.0C)? Assume that during heating, 18% of ...
Saturday, March 30, 2013 at 4:05pm by Dr. Phil

Chemistry
qv = mass H2O x specific heat x delta T = delta E. This answer will be in J/g. I assume you know how to convert to kJ/g and kJ/mole.
Wednesday, February 17, 2010 at 1:50pm by DrBob222

Chemistry
heat lost = mass H2O x specific heat H2O x (Tfinal-Tinitial) = q delta H NH4NO3 = q/1.70 for delta H/g. Multiply by molar mass NH4NO3 to convert to delta H/mol. Convert from J to kJ.
Monday, July 11, 2011 at 1:15pm by DrBob222

physics
A 1.41-kg aluminum pot contains 2.25 L of water. Both pot and water are initially at 17.5C. How much heat must flow into the pot and the water to bring their temperature up to 92.7C? Assume that the effect of water evaporation during the heating process can be neglected and ...
Friday, December 9, 2011 at 10:43am by maria

Chemistry (entropy)
Calculate the Ksp of CaF2 (2 is subscript). The problem wants it calculated with all or one of the following: G = -1162 kJ/mol H = -1215 kJ/mol S = 68.87 J/mol*k The answer is 1.55*10^(-10). How do I do this?
Thursday, April 24, 2008 at 1:32am by help please

chemistry
How much energy must be put into a system to raise 100 g of solid water from 5.5 degrees Celsius to 75 Degrees Celsius? Heat Capacity of Ice: 2.09 J/g degrees C Heat Capacity of Water: 4.18 J/g degrees C Heat of Fusion: 6.01 kJ/mol
Friday, June 17, 2011 at 1:15am by Britney

chemistry
The value of delata h for the reaction below is -186 kJ. Calculate the heat Kj released from the reaction of 25g of Cl2
Friday, January 27, 2012 at 4:05am by ashely

Grade 12 chemistry
I dont understand. in the formula Q=C*M*deltaT, do you use 4.200 kj/mol as C. Is the answer to question one, calculate the heat involved in the trial, 1.19 KJ?
Sunday, January 1, 2012 at 11:08pm by tessa

chemistry
The change of T of water is the way you get to the dH soln. q = mass H2O x specific heat H2O x (28.5-26.9) = ? in joules if sp.j. in joules. q/50.0 g = delta H/gram (delta H/gram) x (molar mass NH4Br) = delta H in J/mol. The usual way of expressing this is in kJ/mol convert J ...
Saturday, November 17, 2012 at 8:21am by DrBob222

Thermochemistry
Heat formation CaF2 is 30.3 kJ/1.95 g CaF2. Convert 1.95 g to moles if you want the answer in kJ/mol which is the usual way you find it in table.
Saturday, June 19, 2010 at 12:43am by DrBob222

chemistry
q1 = heat required to move T from zero C to 100 C. q1 = mass water x specific heat water x (Tfinal-Tinitial). Tf = 100 C; Ti = 0 C. q2 = heat to vaporize liquid water @ 100 C to steam at 100 C. q2 = mass water x delta Hvap. qtotal = q1 + q2.
Monday, November 29, 2010 at 5:29pm by DrBob222

science
You wish to heat 30 kg of water from 60C to 80C. How many kcal of heat are necessary to do this? To how many kJ does this correspond?
Friday, October 12, 2012 at 5:09pm by LeAnne

Chemistry
A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C)
Friday, February 1, 2008 at 4:41pm by Lauren

CHEMISTRY
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
Sunday, September 30, 2007 at 10:37pm by Jake

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).
Wednesday, July 14, 2010 at 6:59pm by Anonymous

Physicis
melting point of copper = 1083.0 C heat capacity of copper = .39 kJ/kg-K heat of fusion of copper = 207 kJ/kg so to warm it up Qin = .39 kJ/kgK(1083-83)K(3kg) = 1170 kJ then to melt it Qin = 207kJ/kg (3 kg) = 621 kJ total Qin = 1791 kJ or 179,100 J
Monday, December 10, 2012 at 10:11am by Damon

chemistry
You need the heat of combustion per mol of propane. Then kJ/mol x mol = 188.23 kJ. Solve for mol and convert that to grams. g = mols x molar mass.
Saturday, August 11, 2012 at 10:41am by DrBob222

physics
A certain heat engine does 8.0 kJ of work and dissipates 8.00 kJ of waste heat in a cyclical process. (a) What was the heat input to this engine? (b) What was its efficiency?
Wednesday, July 24, 2013 at 6:08pm by Alice

physics
A certain heat engine does 8.0 kJ of work and dissipates 8.00 kJ of waste heat in a cyclical process. (a) What was the heat input to this engine? (b) What was its efficiency?
Wednesday, July 24, 2013 at 9:52pm by Eric

physics
Calculate the quantity of heat required to raise the temperature of 2.00 g of water 4.00◦C.
Tuesday, July 5, 2011 at 9:10pm by angel

phisic
Treating air as an ideal gas of diatomic molecules, calculate how much heat is required to raise the temperature of the air in an 7.47 m by 14.9 m by 2.87 m room from 19.9C to 21.7C at 101 kPa. Neglect the change in the number of moles of air in the room
Tuesday, May 3, 2011 at 10:18am by please help me

science
"How many calories of heat are required to raise the temperature of 650 g of water from 13.0C to 20.0C? (Heat of water is 1.00cal/g X C) "
Sunday, April 3, 2011 at 7:21pm by sharon

AP Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
Sunday, September 30, 2007 at 5:09pm by Kate

AP CHEMISTRY
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
Sunday, September 30, 2007 at 5:51pm by Kate

Chemistry
calculate the total amount of heat needed to change 500g of ice at -10*C into 500g of steam at 120*C. do this by calculating the ehat required for each of the following steps and adding to get the total: step 1. ice (-10C)-> ice (0C) step 2. ice (0C) -> water (0C) step 3...
Saturday, May 21, 2011 at 10:20am by Lyila

CHemistry Dr. Bob please?
Yes, you calculate kJ/mol when you do this. If you want kJ per half mole, then multiply by 1/2 and that gives you kJ for whatever problem you are solving. However, it will ALWAYS be kJ/something; i.e., kJ/mol, kJ/g, kJ/500 mg or what have you. If you want to type in your ...
Tuesday, November 11, 2008 at 5:16pm by DrBob222

Chemistry
A .25 g chunk of sodium metal is cautiously dropped into a mixture of 50g of water and 50 g of ice both at 0 C 2Na(s)+ 2h2o(l) -> 2naoh(aq)+ H2 Delta H = -368 kj Will the ice melt Assuming the final mixture has a heat capacity of 4.18 J/g C calculate the final ...
Sunday, January 15, 2012 at 3:29pm by Adriths

Chemistry
A .25 g chunk of sodium metal is cautiously dropped into a mixture of 50g of water and 50 g of ice both at 0 C 2Na(s)+ 2h2o(l) -> 2naoh(aq)+ H2 Delta H = -368 kj Will the ice melt Assuming the final mixture has a heat capacity of 4.18 J/g C calculate the final ...
Monday, January 16, 2012 at 2:33pm by Adriths

Chemistry
First you multiply 10.0 with 540cal/1 g of H2O. To calculate the amount of heat added to (or removed from) a sample of water, the mass of the sample is mulitipled by the heat of vaporization, which is 2260. As before, no temperature change occurs during a change of state. the ...
Wednesday, January 19, 2011 at 3:02pm by jam

Chemistry
First you multiply 10.0 with 540cal/1 g of H2O. To calculate the amount of heat added to (or removed from) a sample of water, the mass of the sample is mulitipled by the heat of vaporization, which is 2260. As before, no temperature change occurs during a change of state. the ...
Wednesday, January 19, 2011 at 3:02pm by jam

Physics - Heat and phase change
9.4 kJ of energy is available to take a sample of ice initially at -40*C, heat it to it's melting point, melt it, and subsequently heat it to 50*C. What is the mass, in grams, of the largest such sample for which this amount of energy will suffice?
Tuesday, March 19, 2013 at 7:50pm by Jos

Chemistry
What quantity of heat is necessary to convert 50.0 g of ice at 0.0 C into steam 100,0 C? The heat of fusion is 80.0 cal/g, the heat of vaporization is 540 cal/g, and the specific heat of water is 1.00 cal/gC.
Tuesday, March 27, 2012 at 6:08pm by Jill

Chemistry
Lead has a melting point of 327C, its specific heat is J/gdeg, and its molar enthalpy of fusion is 4.80 kJ/mol. How much heat, in kilojoules, will be required to heat a 500.0-g sample of lead from 23.0C to its melting point and then melt it?
Sunday, November 4, 2012 at 9:59pm by steph

Chemistry
Lead has a melting point of 327C, its specific heat is J/gdeg, and its molar enthalpy of fusion is 4.80 kJ/mol. How much heat, in kilojoules, will be required to heat a 500.0-g sample of lead from 23.0C to its melting point and then melt it?
Sunday, November 4, 2012 at 10:30pm by steph

physical science
You wish to heat 30 kg of water from 60C to 80C. How many kcal of heat are necessary to do this? To how many kJ does this correspond?
Saturday, March 2, 2013 at 12:26am by Anonymous

chemistry
Convert 2.40 x 10^5 metric tons to grams. Then heat required is q = mass x heat fusion You have the mass, look up the heat of fusion of ice and do the calculation.
Wednesday, February 11, 2009 at 6:18pm by DrBob222

chemistry
q = mass water x specific heat water x delta T. I would convert heat to Joules and mass sample to grams to start.
Friday, February 5, 2010 at 4:22pm by DrBob222

thermodynamics
Use the Carnot cycle H.C.O.P. and the required house heating rate to get the required heat transfer rate to ground water and the electrical input. Use Rankine temperatures for the HCOP. The mass flow rate of ground water can be computed from the water temperature drop and the ...
Sunday, January 16, 2011 at 10:30am by drwls

Chemistry
True or false? The calorie is defined as the amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius.
Thursday, March 14, 2013 at 4:32pm by LEE

Physics
The specific heat of ice and water is given as 2.06 kJ/(kg K) and 4.19 kJ/(kg K) respectively.
Friday, July 20, 2012 at 11:11am by Vladimir

Chemistry
A quantity of ice at 0.0C was added to 25.6 g of water at 21.0C to give water at 0.0C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C). I dont understand how to set this problem up (what the formula is and where to...
Wednesday, October 8, 2008 at 10:57pm by Ryan

Chemistry
A quantity of ice at 0.0C was added to 25.6 g of water at 21.0C to give water at 0.0C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C). I dont understand how to set this problem up (what the formula is and where to...
Wednesday, October 8, 2008 at 11:00pm by Ryan

Chemistry
to get the heat released or absorbed, Q = mc(T2-T1) where m = mass of substance (units in g) c = specific heat capacity (units in J/g-K) T2 = final temperature T1 = initial temperature **note: if Q is (-), heat is released and if (+), heat is absorbed now we can only apply ...
Thursday, March 31, 2011 at 1:49am by Jai

chemistry
Yes, the 60 is correct. It's the solution that is absorbing the heat; therefore, the mass to use is that of the solution. What you have calculated is Joules for the reaction of 0.524 g Mg. J/g = q/0.524. You can convert to J/mol from J/g x (atomic mass Mg/1 mol) = ??. The ...
Tuesday, March 22, 2011 at 8:05pm by DrBob222

chemistry
the specific heat of water is 4.184 j/g-c(celcius). how much heat is required to raise the temperature of 5.0 g of water by 3.0 c(celcius)?
Sunday, April 4, 2010 at 7:17pm by demond

Chemistry
Based on the results of problems 8 and 9 if the heat of formation of water is -286 kJ/mol, The H ffor CaO(s) is kJ/mol.
Friday, February 11, 2011 at 1:12am by Shawn

Physics
Hi can someone advise whether my methodology is right on this with a potential energy of 589 kJ per tonne, 100 tonnes of water per second are delivered to a turbine. Assuming all the potential energy of this water is used to drive the turbine how much power will be delivered ...
Saturday, October 13, 2007 at 2:25pm by Mark

chemistry
2H2 (g) O2 (g) --> 2H2O (g) if 44 g of O2 are reacted , determine the amount if heat transferred in the reaction when the Heat = -483.6 kJ
Monday, December 12, 2011 at 12:44am by becca

chemistry
2H2 (g) O2 (g) --> 2H2O (g) if 44 g of O2 are reacted , determine the amount if heat transferred in the reaction when the Heat = -483.6 kJ
Monday, December 12, 2011 at 12:44am by becca

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 ...
Friday, July 24, 2009 at 6:26pm by Sahar

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.
Sunday, June 3, 2012 at 11:58pm by shan

chem
How much heat (in {kJ}) evolves when 7.0L of C2H2(d = 1.0967kg/m^3) is mixed with a stoichiometric amount of oxygen gas? The combustion reaction is C2H2+ 5/2 O2-> 2 CO2+ H2O, Delta H=-1299.5 kJ
Monday, November 19, 2012 at 12:57pm by Chironjit

Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
Sunday, September 30, 2007 at 9:37am by Kate

Chemistry
A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C. The final ...
Sunday, September 30, 2007 at 12:33pm by Kate

Thermochemistry
The standard enthalpy of formation of n-octane is -249.95 kJ/mol. Compute the amount of heat liberated when 5.24 g of n-octane is burned completely with excess oxygen to form carbon dioxide and liquid water.
Sunday, December 4, 2011 at 8:58pm by LaurenB

Chemistry
Note the correct spelling of celsius. q = mass H2O x specific heat H2O x (Tfinal-Tinitial) q = heat combustion heat combustion/g = q/1.32g\ heat combustion/mol = (q/1.32)*molar mass. This will be in J/mol. Convert to kJ/mol.
Thursday, February 7, 2013 at 1:10pm by DrBob222

chemistry
calculate the amount of heat released when 50g of water at 100degrees hits the skin, condenses, cools the body to 37 degrees
Tuesday, September 21, 2010 at 2:38pm by christian

Chemistry
Let's see. q = mass x specific heat x delta T. Could you weigh an amount of Na metal, let it react with a known mass of water, measure delta T of water for the heat of reaction, and you know specific heat of water? That would give you q for the mass of Na reacted. Check my ...
Friday, September 14, 2007 at 7:31pm by DrBob222

chemistry
A hydrocarbon sample was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.00 kg of water rose from 20.45C to 23.65C. The heat capacity of the calorimeter, excluding the water, is 2.21 kJ/C. determine the heat released by the combustion.
Saturday, August 15, 2009 at 11:26am by jessica

Chem
The value of H for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO(g) reacts completely. 2CO(g) + O2(g) 2CO2(g) *I just want to how to solve this problem as in an equation, not the answer. thank you!
Friday, June 8, 2012 at 3:03pm by Harlem

chem
How much energy (in Joules) is required to heat 13.48 g of water from 10.5 oC to 46.2 oC ? Use 4.184 J/goC as the specific heat capacity of water.
Monday, March 26, 2012 at 4:06pm by emily

chem- drbob222 please help
my original question was: how do i figure this out?? How much heat does your body lose when 2.46 g of sweat evaporates from your skin at 25C? chem - DrBob222, Tuesday, February 22, 2011 at 10:52pm q = mass water x delta Hvaporization. chem - Rebekah, Wednesday, February 23, ...
Wednesday, February 23, 2011 at 5:49pm by Rebekah

chemistry
I usually work this type by calculating how much water is required to dissolve 24 g. We know it takes 100 g H2O to dissolve 79 g of x so 100 * (24/79) = ?? is the amount of water required to dissolve 24 g. Then compare that number with the amount of water you have (68g). If ...
Tuesday, August 2, 2011 at 1:47pm by DrBob222

physics
The recovery time of a hot water heater is the time required to heat all the water in the unit to the desired temperature. Suppose that a 62-gal (1.00 gal = 3.79 x 10-3 m3) unit starts with cold water at 11 C and delivers hot water at 53 C. The unit is electric and utilizes ...
Monday, February 18, 2013 at 12:30am by Anonymous

Physics
The recovery time of a hot water heater is the time required to heat all the water in the unit to the desired temperature. Suppose that a 62-gal (1.00 gal = 3.79 x 10-3 m3) unit starts with cold water at 11 C and delivers hot water at 53 C. The unit is electric and utilizes ...
Monday, February 18, 2013 at 6:49pm by Anonymous

chemistry
given the following info for water molar heat of specific heat capacity of liquid water 4.18 j/g degrees calculate the total quanity of heat evolved when 10.0g of steam is condensed,cooled,and frozen to ice at -50 degrees
Tuesday, April 12, 2011 at 5:25pm by jules

Excel Problem
heat lost by hot water + heat gained by cold water = 0 initial volume = 3000 L 30 L/min x 5 min = 150L [mass cold water x specific heat x (Tfinal-Tinitial)] + [mass warm water x specific heat x (Tfinal-Tinitial)] = 0 You know mass cold water (150L = 150kg You know specific ...
Sunday, September 18, 2011 at 11:42pm by DrBob222

Chemistry
Surface area changes the TIME it takes to melt but doesn't change the amount of heat required to melt. I don't know where you got the idea that it requires more heat to melt 10 g than 20 g. And you are right, it IS the opposite. If it takes x amount of heat to melt 10 g it ...
Monday, June 17, 2013 at 12:42am by DrBob222

chemistry
When 1.50 g of calcium chloride is dissolved in 150.0 g of water, the temperature of the water rises from 20.50C to 22.25C. Assume that all the heat is absorbed by the solution. (a) Calculate the heat of solution per gram and per mole of CaCl2 that dissolves. (b) Is this an ...
Tuesday, November 1, 2011 at 4:34pm by john

chemistry
q = mass x heat fusion, convert to kJ.
Friday, April 30, 2010 at 12:28am by DrBob222

molar heat
the molar heat of vaporization for water is 40.79 kJ/mol. How would you express this heat of vaporization in joules per gram.
Wednesday, May 19, 2010 at 8:16pm by Sienna

Physics
How long would it take a kettle with a 1kW heating element to heat 1 litre of water? Watts = Joules / second Mass of 1 litre of water = 1kg 1 kW = 1 k Joule / second or 1000 joules/ second 1g of water needs 4.184J to raise the temperature by 1̊ c. Water ...
Wednesday, December 15, 2010 at 6:56am by Paul

chem
Determine the limiting reagent. Determine how much of the excess reagent is present and how much of (it will be all of it) the limiting reagent reacted. Using the limiting reagent, calculate the amount of heat generated from the -116 kJ. That will be q. Then q = mass x ...
Saturday, December 1, 2007 at 2:29pm by DrBob222

Chemistry
Calculate the amount of heat required to take 3.00kg of ice at -10 degrees Celsius to 115 degrees celsius.
Wednesday, April 25, 2012 at 1:01am by Ahmad

Physics- LOST!
Convert 500 watts to joules/sec. That is 500 J/sec. The problem states about 80% is converted to heat so 500 J/sec x 0.8 = ?? heat produced in 1 sec. How many J is that per hour. 500 J/sec x (60 sec/min) x (60 min/hour) = ?? J/hour. Then q = mass H2O in kg x heat of vap of ...
Monday, December 3, 2007 at 12:30pm by DrBob222

Chem
How much heat is liberated at constant pressure if .928 g of Fe reacts with 26.2 mL of .238 M HCl? Delta H = -87.9 kJ
Monday, July 25, 2011 at 10:50am by Anonymous

Physical Science
Hello, Can you tell me if I have the correct answer? Thank You How much heat is required to convert 0.3 kilogram of ice at 0 degrees celsius to water at the same temperature? My answer: 100,375 J
Thursday, February 7, 2008 at 11:49pm by Mandi

Chem 100
q1 = heat to move ice at -22 to the melting point of zero C. q1 = mass x specific heat ice x (Tfinal-Tinital) q2 = heat to convert solid water (ice) at zero C to liquid water at zero C. q2 = mass x heat fusion. q3 = heat to move liquid water at zero C to the boiling point at ...
Sunday, May 1, 2011 at 4:49pm by DrBob222

chem
Am I missing something? First, what's the question? Is it to calculate the heat released by the reaction? Or is it something else? 56.2 kJ/mol x 0.120 mol = 6.744 kJ which rounds to 6.74 kJ to three significant figures (s.f.). I OFTEN find that when students are keying answers...
Sunday, February 28, 2010 at 11:36pm by DrBob222

chemistry
1(a) when 25.0ml of 0.500 mol.dm3 H2SO4(AQ) SOLUTION IS added to 0.025dm3 of 1.00 moldm3 KOH SOLUTION , THE TEMPERATURE OF THE REACTION MIXTURE RISES FROM 23.50 CELCIUS TO 30.17 CELCIUS . THE SPECIFIC HEAT CAPACITY AND DENSITY OF WATER 4.20j.g.celcius and 1.00 g.cm. the ...
Thursday, February 9, 2012 at 12:02pm by mustafe

chemistry
Given that for the vaporization of benzene Hvap= 30.7 kj/mol and Svap= 87.0 J(K * mol) , calculate Delta G (in kJ/mol) for the vaporization of benzene at 13 Celcius.
Monday, April 29, 2013 at 10:29pm by Chloe

specific heat capacity
How much heat would be required to heat 1 gram of pure liquid water from 10C to 20C? How would i approach this problem?
Monday, September 26, 2011 at 1:33am by D

chemistry
Calculate the mass of ethanol required to heat 200mL of water from 21 degrees celcius to 45 degress celcius
Tuesday, November 9, 2010 at 1:44am by Kate

chemistry
calculate the quantity of heat (cal, J) required to change the temperature of 1500g water from 25C to 75C. do i have this right 1500 X 4.18J/g C X 50C = 313500
Thursday, November 3, 2011 at 4:37pm by Doss

Thermochemistry
How many grams of water at 0 degrees C can be frozen into ice at 0 degrees C if 55.0 kJ of heat is removed? delta Hsolid= -6.01 kJ/mol
Tuesday, December 14, 2010 at 11:23pm by Hannah

chemistry
You need to know the delta H for the reaction. That isn't listed in the problem but you can look it up. How much heat do you need? That's q = mass H2O x specific heat H2O x (Tfinal-Tintial) You have the data to calculate q needed. Then 24.3 g Mg x (q in kJ/delta H iin kJ) = g ...
Tuesday, May 14, 2013 at 3:49pm by DrBob222

physics
The latent heat of fusion for water is 33.5 104 J/kg, while the latent heat of vaporization is 22.6 105 J/kg. What mass m of water at 0 C must be frozen in order to release the amount of heat that 2.32 kg of steam at 100 C releases when it condenses?
Tuesday, July 30, 2013 at 10:22pm by damon

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