
1.55 g of penatanol 250ml water Heat from 10 to 38 degrees Find hear of combustion

Assume you can heat water with perfect insulation (all the heat from combustion of ethanol is transferred to water). What is the volume of ethanol required to heat 100 mL of water by 10 degrees C? (You will need to look up density of ethanol, specific heat

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.

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.

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.


In a laboratory activity, a student team measures the heat released by burning heptane. Using the following data, calculate the molar heat of combustion of heptane in kJ/mol: Mass of water  179.2 g Initial water temperature  11.6 degrees C Final water

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.

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.

Calculate the mass of ethanol that must be burnt to increase the temperature of 150g of water by 75 degrees celsius, if exactly 75% of the heat released by this combustion is lost to the surroundings. Also it is given that the heat of combustion of ethanol

What is the minimum amount of ice (at 0 degress C) that must be added to 250mL of water at 23 degrees C in order to cool it to 0 degrees celsius? (Density of water= .98 g/cm^3; heat of fusion= 333J/g; heat capacity of water= 4.184J/g C; and heat capacity

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

The combustion of 0.0222g of isooctane vapor, C8H18(g), at constant pressure raises the temperature of a calorimeter 0.400 degrees C. The heat capacity of the calorimeter and water combined is 2.48kJ/degrees C. Find the molar heat of combustion of gaseous

Principles of heat: How many kilograms of water can be evaporated at 100 degrees Celsius by the combustion of 470 litres of fuel oil whose heat of combustion is 37 MJ/Litre

When 47.5J of heat are added to 13.2 g of liquid, its temperature rises by 1.72 degrees C. What is the heat capacity of the liquid? A cook wants to heat 1.35kg of water from 32.0 degrees C to 100 degrees C. If he uses combustion of natural gas to heat the

the heat of combustion of propane is 5.47MJ/mol. there is 1.50kg of propane available to burn. how many litres of water could be heated from 18.0 degrees Celcius to 63.0 degrees Celcius using the heat from the burning propane. assume that all heat lost by


The combustion of how many moles of ethane would be required to heat 838 grams of water from 25.0 to 93.0 degrees C? Assume liquid water is formed during the combustion.

How many kilograms of water can be evaporated at 100 degrees Celsius by the combustion of 470 litres of fuel oil whose heat of combustion is 37 MJ/Litre

How many kilograms of water can be evaporated at 100 degrees Celsius by the combustion of 470 litres of fuel oil whose heat of combustion is 37 MJ/Litre

Sucrose is commonly known as table sugar. The formula is C12H22O11. You burn 7.29 grams of sucrose in a bomb calorimeter. The temperature of the calorimeter and the water in it rises from 23.24 degrees celsius to 29.77 degrees celsius. The bomb's heat

The complete combustion of 0.100 mol of CH4 in oxygen in a bomb calorimeter caused the water of the calorimeter to rise in temperature from 25.00 degrees Celsius to 37.70 degrees Celsius. Suppose that the combustion of the 0.1 mol of CH4 was instead run at

how many calories of heat energy are required to warm 250ml of water from 35 degrees celsius to 64 degrees celsius?

Propane gas is used to heat a tank of water. If the tank contains 200 L of water, what mass of propane will be required to raise its temperature from 20 degrees C to 65 degrees C. The heat of combustion for propane is 2220 kJ/mol.

While researching energy values of fuels, a chemist designed an experiment to find out the heat of combustion of pentane. Using the known hexane heat of combustion of hexane = 4650kJ/mol and the data below calculate the heat of combustion of pentane. Set

While researching energy values of fuels, a chemist designed an experiment to find out the heat of combustion of pentane. Using the known hexane heat of combustion of hexane = 4650kJ/mol and the data below calculate the heat of combustion of pentane. Set

3.6 g of a hydrocarbon fuel is burned in a calorimeter that contains a 244 grams of water initally at 25.00 degrees C. After the combustion the temperature is 26.55 degrees C. How much heat is evolved per gram of fuel burned? The heat capacity of the


A 35.00 mL sample of water at 30.0°C is placed in an open container with an external pressure of 1.00 atm. 30.0 kJ of heat is added to the water sample. The density of water is 1 g/mL. (a) How many grams of liquid water remain at the end of the process?

80.0 mL of water is initially at room temperature (22degrees C). A chilled steel rod at 2 degrees C is placed in the water. If the final temperature of the system is 21.2 degrees C, what is the mass of the steel bar? Specific heat of water =

The heat of fusion for water is 80cal/g. The specific heat of liquid water is 1.00cal/g. How many calories of heat are released when 20g of water at 30 degrees is cooled to 0 degrees and frozen to ice at 0 degrees?

A 1.55 gram sample of methanol (CH3OH) is combusted in a bomb calorimeter. The molar heat of combustion of methanol is 725KJ/mole, assuming that 2.0L of water initially at 25.0 C absorbs all of the heat of combustion, what is the final temperature of the

The temperature of 100.0 mL of water was raised from 26.7 degrees C to 62.3 degrees C. How much heat in calories was added to the water? (The specific heat of water is 1.000 cal/g degrees C and the density of water at 26.7 degrees C is 0.996626 g/mL)

So I am writing a lab report and Im stuck with calculating the enthalpy change of combustion of the following reaction: Mg+2HCl> MgCl2+H2 .I am given the mass of Mg which is 5g and the concentration of HCl which is 2M and the volume of HCl which is 50

1. How much heat energy is lost by 3 kg of water when it cools from 80 degrees C to 10 degrees C? 2. A 300 g piece of aluminum is heated from 30 degrees C to 150 degrees C. What amount of heat energy is absorbed? 3. Determine the temperature change in each

Spent steam from an electric generating plant leaves the turbines at 120.0 degrees Celsius and is cooled to 90.0 degrees Celsuius liquid water by water from a cooling tower in a heat exchanger. How much heat is removed by the cooling tower water for each

1) A quantity of 85 mL of .900 M HCl is mixed with 85 mL of .900 M KOH in a constantpressure calorimeter that has a heat capacity of 325 J/C. If the initial temperatures of both solutions are the same at 18.24 degrees C, what is the final temperature of

Find the heat necessary to change 2.5kg of water (ice) at 2 degrees C to steam at 105 degrees C. specific heat ice= 2060 specific heat water= 4180 specific heat steam= 2020 heat of fusion= 3.34X10^5 heat of vaporization= 2.26X10^6


The combustion of 0.0222g of isooctane vapor, C8H18(g), at constant pressure raises the temperature of a calorimeter 0.400 C. The heat capacity of the calorimeter and water combined is 2.48 kJ/C. Find the molar heat of combustion of gasdeous isooctane.

A 1.20g sample of benzoic acid is burned in excess of )2 in a bomb calorimeter immersed in 1300 g of water. The temperature of the water rises from 25 to 30.2 degrees C. The heat of combustion of benzoic acid is 26.4 kJ/g. The heat capacity of water is

When 0.320 moles of NH4Cl is dissolved in 1.00 L of water, the temperature drops by 13.7 degrees C. What is the heat of solution of ammonium chloride? The solution has a density of 1.0012 g/mL and a specific heat of 0.9818 cal/g degrees C. How do you find

How many kilograms of water at 15oC can be heated to 95oC by burning 143 grams of methane, CH4, assuming that 100% of the heat is used to heat the water. The heat of combustion of methane is 891 kJ per mole of methane. (The specific heat of water is 4.184

the heat of fusion water is 335J/g,the heat of vaporization of water is 2.26kJ/g, the specific heat of water is 4.184J/deg/g. how many grams of ice at 0 degrees could be converted to steam at 100 degrees C by 9,574J

The heat of combustion of C2H4 at 27 C at constant prssure is 333.3 Kcal. What will be the heat of combustion at constant volume considering the water to be in liquid state? (R=1.987 cal)

How many liters of , measured at 20 , must be burned to provide enough heat to warm 28.3 of water from 15.5 to 31.3 , assuming that all the heat of combustion is transferred to the water, which has a specific heat of 4.18 ? Recall that .

A 40.0 g block of ice at 15 degrees C is dropped into a calorimeter (of negligible heat capacity) containing water at 15 degrees C. When equilibrium is reached, the final temperature is 8.0 degrees C. How much water did the calorimeter contain initially?

The sugar arabinose, C5H10O5, Molar Mass = 150.15 g/mole, was completely combusted with excess oxygen in a calorimeter. Combustion of a 0.548 g sample of arabinose caused the temperature to increase from 20.00 degrees C to 20.54 degrees C in a calorimeter

You drop a hot copper penny (500 degrees celsius) that has a mass of 4.5 grams into a glass of cold water (6.0 degrees celsius) with a volume of 120 mL. The water heats up to 7.7 degrees celsius. Find the heat absorbed by the water, then determine the


how would i calculate; a 50g sample of water at 100 degrees is poured into a 50g sample of water at 25 degrees. with a specific heat of water (l) being 4.184 j/g degrees C.what will be the final temperature of the water? heat gained + heat lost = 0

A 500 g piece of metal at 60 degrees celsius is placed in 200g of water at 22 degrees celsius contained in a coffee cup calorimeter. The metal and water come to the same temperature at 32.5 degrees cesius. The specific heat of the water is 4.184

I have to find the molar enthalpy of combustion of pentane. I have this info: 5C(s) + 6H2 >>> C5H12 Hf= 173.5kJ C+O2>>> CO2 Hf= 393.5kJ H2 + 1/2O2 >>> H2O Hf= 241.8kJ H2O >>> H2O Hf= +44.0kJ THEN I am given this: mass

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

using the values for heat of fusion, specific heat of water, or heat of vaporization, calculate the amount of heat energy. Calories needed to warm 20.0g of water at 15 degrees Celsius to 72 degrees Celsius (one step) Show work please

Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is 40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of

You take 2 liters of water at 20 degrees Celsius and remove heat at 200W from it for 5 min. What is the temperature and state of the water after the experiment? Some properties of water: Heat of fusion: 333.55 kJ/kg, Heat of vaporization: 2257 kJ/kg, Heat

A 100g piece of ice at 0 degrees celcius is placed into a container holding 200g of water, initially at temperature 25 degrees celcius. Heat flows from the water to the ice, cooling the water and melting the ice. Calculate a) how many moles of ice and how

Calculate the theoretical amount of CaCl2 that would be required to change the temperature of 50 mL of water from from temperature 20 degrees Celsius to 45 degrees Celsius. Remember that the heat lost during the dissociation is equal to the heat gained by

Calculate the theoretical amount of CaCl2 that would be required to change the temperature of 50 mL of water from from temperature 20 degrees Celsius to 45 degrees Celsius. Remember that the heat lost during the dissociation is equal to the heat gained by


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

Liquid water has a specific heat of 4.184 J/g degrees celcius. If 50 grams of water is heated from10 to 55 degrees celcius, what is the heat energy in joules needed to heat this water

Heat from burning a fuel is absorbed by a copper calorimeter. The calorimeter has a mass of 81.34 g and contains 200.0 g of water initially at 21 degrees Celsius. a) How much heat was absorbed by the calorimeter and the water if the final temperature of

How much energy in kJ is needed to heat 7.0L of water from35 degrees Fahrenheit to boiling point 100 degrees Celsius. If the density of water is 1.0g/cm^3 and the heat capacity of water is Cp= 4.184J/g degrees Celsius

Calculate the molar heat of combustion of paraffin, expressed in units of kJ/mol. First calculate the thermal energy released when one mole of parafin burns) because one mole of parafin (c25h52) has a mass of 325g, the molar heat of combustion will be 352

What would be the final temp when 100 kg of 0 degrees Celcius cold water is mixed with 60 kg of 35 degrees warm water? Ans is in degrees Celcius. The sum of the heats gained is zero (remember one will lose heat, so have a negative heat gained). Heatgained

When 7.5 g of ethane was completely burned, all the heat produced was used to heat 1.50 kg of water. If the temperature of water rose from 20EC to 80EC, the heat of combustion of ethane is

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 (25.0°C) to boiling (100.0°C)? Assume that

You want to heat 1 kg of water 10 celsius and you have the following methods under consideration. The heat capacity of water is 4.184 J/K g. (a)You can send the water through a solar collector that has an area of 1 m^2. How long will it take if the sun's

A 94.7 g sample of silver (s= 0.237 J/(g x Degree C)), initially at 348.25 Degrees C , is added to an insulated vessel containing 143.6 g of water (s=4.18 J/(g x Degree C)), initially at 13.97 Degrees C. At equilibrium, the finial temperature of the


the pressure is one atmosphere and determine the heat in joules required to produce 5.03 kg of water vapor at 100.0 °C, starting with (a) 5.03 kg of water at 100.0 °C and (b) 5.03 kg of liquid water at 0.0 °C. for part (a) I used the equation Q=mL and L

How much heat is added to a 10.0 g of ice at 20.0 degrees Celsius to convert it to steam at 120.0 degrees Celsius? compute and add the following heats: heat to heat ice from 20C to 0C heat to melt ice at 0C Heat to heat water from 0 to 100C heat to

What would be the final temperature when 125g of 25 degrees Celcius water is mixed with 85g of 45 Degrees Celcius water? ( hint: Equate the heat gained by the cool water with the heat lost by the warm water.)

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) q = mass x specific heat x

A 599 g piece of silver at 150 degrees C is submerged in 1000 g of water at 5 degrees C to be cooled. Determine the final temperature of he silver and water given Heat capacity of water= 4.18 x 10^3 j/kg degrees C Heat capacity of silver= 2.49 x 10^2 j/kg

A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C.

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) q = mass x specific heat x

Suppose you want to heat a mug of H2O (250ml) from room temperature 25 degrees celcius to 100 degrees celcius. How much energy would you need from your microwave?

Calculate the heat released from 61.5 g of steam at 111 degrees C is converted to water at 39 degrees C. Assume the specific heat of water is 4.184 J/g*C, the specific heat of steam is 1.99 J/g*C and the enthalpy.H.vap= 40.79 KJ/mol of water

A 2.461g sample of glutamic acid, C5H9NO4 (147.13 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 23.76 °C; after combustion the calorimeter and the water had a


A mass of 7 kg of water is raised from 8 degrees C to the boiling point 100 degrees C. How much heat is required? The specific heat of water is 1000 cal/kg · degrees C. Answer in units of cal I got 644000, is that right?

How long would it take for 1.50mol of water at 100.0 degrees to be converted completely into steam if heat were added at a constant rate of 23.0J/s ? the constants are: Specific heat of ice: 2.09J(g/degrees celcius) Specific heat of liquid water: 4.18 J

A water heater is fueled by the combustion of propane as described by the following reaction: C3H8(g) + 5 O2(g) > 3 CO2(g) + 4 H2O(l) a) Determine how much heat is released if 11.2 moles of propane are burned at 298 K and at a constant pressure of

If the price of electrical enegy is $0.10 per kilowatt *hour, find the cost of using electrical energy to heat the water in a 12.0m * 9.00m * 1.5m swimming pool from 15 degrees C to 27 degrees C. So the change in temperature is 285.15 , the volume is

tori wants to increase the tempreature of 500 grams of water from 20 degrees celcius to 100 degrees celecius if the specific heat of water is 4.18j/g. degrees celcius how much heat is needed ?

A mass of 7 kg of water is raised from 8 degrees C to the boiling point 100 degrees C. How much heat is required? The specific heat of water is 1000 cal/kg · degrees C. Answer in units of cal

In lab we did thermochemistry, where we are supposed to find the heats of solution, heat change of calorimeter and molar heat solution of the salt. I calculated that the calorimeter constant for the water we had was 883.194 Joules. We took 1/10 of a mole

How many kilojoules of heat are absorbed when 1.00L of water is heated from 18 degrees C to 85 degrees C? Did I do this right? 1000g H2O x 4.18 x 67 = 280060 kilojoules (my book says the specific heat for water in J/g x degrees C = 4.18, and for cal/g x

At a crime scene, police officers find a murder victim in a tub full of warm water. A thermometer shows that the water temperature is 75 degrees F and the air temperature is 70 degrees F. It is known that most people fill a tub with water at 100 degrees F.

A geyser heats water flowing at the rate of 3L/min from 27 deg C to 77 deg C. if the geyser operates on a burner, what is the rate of combustion of the fuel if its heat of combustion is 40000J/g?


A geyser heats water flowing at the rate of 3L/min from 27 deg C to 77 deg C. if the geyser operates on a burner, what is the rate of combustion of the fuel if its heat of combustion is 40000J/g?

The following substances undergo complete combustion in a bomb calorimeter. The calorimeter assembly has a heat capacity of 5.136 ^ C. In each case, what is the final temperature if the initial water temperature is 22.37^ C? 0.3268g caffeine, C8H10N4 (heat

I am lost about where to start on this. "The idea comes to mind to put some hot rocks in your frozen bath water. What mass of rocks at 220 degrees Celsius needs to be added to 500.0L of frozen bath water at 0 degrees celsius to raise its temperature to 55

Calculate the heat released when 42.0 g of water at 35.0 degrees Celsius is converted to ice at 5.0 degrees Celsius. The specific heat of ice is 2.03 J/(g C), the molar heat of fusion of ice is 6010 J/mol, and the specific heat of water is 4.18 J/(g C)

A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C.

A 5.00 g sample of Al pellets (specific heat = .89 J/g degrees c) and a 10.00 g sample of Fe pellets (specific heat = .45 J/g degrees c) are heated to 100.0 degrees C. The mixture of hot Fe and Al is then dropped into 97.3 g of water at 22.0 degrees C.

At a crime scene, police officers find a murder victim in a tub full of warm water. A thermometer shows that the water temperature is 75 degrees F and the air temperature is 70 degrees F. It is known that most people fill a tub with water at 100 degrees F.

I don't understand this: For the temperature vs time graph for heat and changes of state. The graph starts at 2.1 degrees C The heat of fusion is at 2.0 degrees C The heat of vaporization is on 101.0 degrees C. The graph ends at 103.0 degrees C. So to get

Find the specific heat of an unknown metal given this data: Mass of the metal = 120 g Temp of the metal = 220 degrees Mass of the water = 30 g Initial Temp of the water = 20 degrees Final Temp of the water = 85.6 degrees Specific Heat of the water = 4.186

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


Which provides more cooling for a styrofoam cooler, one with 10 lbs of ice at 0 degrees C or one with 10 lbs of ice water at 0 degrees C. Explain. qice=mass*heat of fusion. qH2O=mass*specific heat x delta T However, you aren't given a two temperatures;

I have previously posted this question, but now I am lost question: A calorimeter is filled with 10.0 millimole (mmole) of methane gas and an excess of oxygen. When burned, the ignition wire releases 107.2 J of heat. The heat capacity of the calorimeter

Can someone please explain how to do this problem? I am really confused. Thank you. 3. How much heat does 32.0 grams of water absorb when it is heated from 25.0 degrees Celsius to 80.0 degrees Celsius? q = mass*specific heat water*(TfinalTinitial) = ??.

Any help would be great, even if it is just a way to start or a formula. Calculate the heat necessary to convert 10.0 g of water (just melted) at 0 degrees Celcius to water at 20 degrees Celcius, assuming that the specific heat remains constant at 1

The combustion of 1.00 mol of sucrose,C12H22,O11, evolves 5650 kJ of heat. A bomb calorimeter has a calibrated heat capacity of 1.23 kj/degree Celsius. How many grams of sucrose should be burned to raise the temperature of the calorimeter and its contents