
If 15.0 mL of a 1.5M HCl solution at 22.5 degrees C is mixed with 25.0mL of a 1.5M NaOH solution at 21.5 degrees C that is in a calorimeter, and the final mixed solution temperature ends up at 28.5 degrees C, 1.)what is the balanced equation for this

3. If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mL of a 1.5M NaOH solution at 21.50C that is in a calorimeter, and the final mixed solution temperature rises to 28.50C, what is the ΔHrxn for this process? Assume that Ccalorimeter =

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

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

Water with a mass of 1000kg leaves a hose at 20oC and is converted by the heat from the fire into steam at 300oC. List the steps needed in order to determine the amount of heat that is added to the water. For each step show the formula that must be used


. Water with a mass of 1000kg leaves a hose at 20oC and is converted by the heat from the fire into steam at 300oC. List the steps needed in order to determine the amount of heat that is added to the water. For each step show the formula that must be used

Water with a mass of 1000kg leaves a hose at 20oC and is converted by the heat from the fire into steam at 300oC. List the steps needed in order to determine the amount of heat that is added to the water. For each step show the formula that must be used

1) A 0.1375g sample of solid magnesium is burned in a constantvolume bomb calorimeter that has a heat capacity of 3024 J/C. The temperature increases by 1.126 degrees C. Calculate the heat given off by the burning Mg, in kJ/g and kJ/mol. 2) Determine the

A 0.260kg piece of aluminum that has a temperature of 165 °C is added to 1.4 kg of water that has a temperature of 3.0 °C. At equilibrium the temperature is 0 °C. Ignoring the container and assuming that the heat exchanged with the surroundings is

Why would you subtract the heat of a calorimeter when calculating heat of the reaction? hint: the heat of the calorimeter is the amount of heat that the calorimeter absorbs from the solutioneach calorimeter will absorb a certain amount of heat, which

Use your value for the heat of neutralization, ∆H, 9490, to determine the amount of heat evolved when 10.00mL of 0.4091 M HCL reacts with 10.00mL of 0.4037 M NaOH.

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

1 litre of coffee at 80oC need to be cooled to 40oC. Assuming that all the ice melts and no heat is lost to the environment. Take the specific heat capacity of coffee to be 4200J/kgK, density of coffee to be 1000kg/m3 and latent heat of fusion of water to

When your body breaks down sugar completely, how much heat is released compared to burning the same amount of sugar in a flame? The body releases___ less heat than the flame*** more heat than the flame same amount of heat as a flame the body releases so

Determine the amount of heat needed to raise 20.0 g of ice at 0 degrees C to steam at 100 degrees C. (ΔHfusion = 334 J/g; Specific heat of (H2O) = 4.18 J/gc; ΔHvap = 2.25 kJ/g)


Determine the amount of heat needed to raise 20.0 g of ice at 0 degrees C to steam at 100 degrees C. (ΔHfusion = 334 J/g; Specific heat of (H2O) = 4.18 J/gc; ΔHvap = 2.25 kJ/g)

1) Determine the amount of heat in kJ given off when 1.26 x 10^4 g of NO2 are produced according to the equation: 2NO (g) + O2 (g) > 2NO2 (g) and delta (H) = 483.6 kJ/mol 2) A sheet of gold weighing 10 g and at a temperature of 18 degrees C is placed

A researcher determined the amount of electrical energy entering a toaster and the amount of heat given off by the toaster. The amount of heat was less than the amount of electrical energy. How can this observation be explained?

Plan,design and conduct an investion to find out whether the amount of heat produced will depend on increase on concentration of Hcl when Hcl reacts with an excess zn.you may investigate either the amount of heat produced or the amount of gas produced(make

design and conduct an investion to find out whether the amount of heat produced will depend on increase on concentration of Hcl when Hcl reacts with an excess zn.hint...you may investigate either the amount of heat produced or the amount of gas

design and conduct an investion to find out whether the amount of heat produced will depend on increase on concentration of Hcl when Hcl reacts with an excess zn.hint...you may investigate either the amount of heat produced or the amount of gas

Record the amount of heat needed to change phases for waterice to steam using graphical analysis. Is there a one accurate amount of heat needed to change phases, I thought it varied depending the problem... Would the question be asking for the heat needed

Which statement is wrong? 1. Adding the same amount of heat to two different objects will produce the same increase in temperature. 2. When the same amount of heat produces different changes in temperature in two substances of the same mass, we say that

Why is a measured amount of water needed to determine the specific heat of a metal object?

CaCl2(s) > Ca(aq) + 2Cl(aq) ΔH_rxn = +198.0 KJ "If that g sample of calcium chloride was dissolved in 1000.0g of water, with both substances originally at 25.0C, what would be the final temperature of the solution be? Assume no loss of heat to the


design and conduct an investion to find out whether the amount of heat(gas) produced will depend on an increase on the concentration of Hcl when Hcl reacts with an excess zn.hint...you may investigate either the amount of heat produced or the amount of gas

Calculate the amount of heat (in calories) absorbed when 50.0g of water at 20C spreads over your skin and warms to body temperature, 37C. I don't understand how to figure this out  which number is the specific heat number? 20C or 37C? I know delta temp

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

design and conduct an investion to find out whether the amount of heat(gas) produced will depend on an increase on the concentration of Hcl when Hcl reacts with an excess zn..guidance/hint...you may investigate either the amount of heat produced or the

an ideal system absorbed some amount of heat and gas expand and the piston move to 0.4 meter against than the atmospheric pressure. If the cross sectional area of the container is 0.6 meter2. What is the amount of heat absorbed?

determine the total amount of energy required to heat 25g of ice at 18 C to steam at 125 C

determine the amount of heat generated per minute by a 120 volt lamp which takes 0.5 amperes. thanks!

the specific heat of water is one of the highest of all substances.why does this make water a useful liquid to use in hot water bottles? and could you use a lump of nickel to warm your bed instead of a hot water bottle?which would be better? why? I will be

A heat pump has a coefficient of performance of 4.5. If the heat pump absorbs 46.1 cal of heat from the cold outdoors in each cycle, what is the amount of heat expelled to the warm indoors? (in cal)

The amount of heat required to raise temperature of 55.85 g of iron 1 degrees C is called its A. Change of energy B. Enthalpy C. Molar heat capacity D. Specific heat capacity E. Specific Heat.


A heat pump has a coefficient of performance of 4.5. If the heat pump absorbs 46.1 cal of heat from the cold outdoors in each cycle, what is the amount of heat expelled to the warm indoors? (in cal) tried everything but got nothing.

design and conduct an investion to find out whether the amount of heat(gas) produced will depend on an increase on the concentration of Hcl when Hcl reacts with an excess zn..guidance/hint...you may investigate either the amount of heat produced or the

Plan,design and conduct an investion to find out whether the amount of heat(gas) produced will depend on an increase on the concentration of Hcl when Hcl reacts with an excess zn..guidance/hint...you may investigate either the amount of heat produced or

Use Hess's Law to find the change in heat of 2C(graphite)+H2(g)>C2H2(g)? Given: C(graphite) + O2(g) > CO2(g) change of heat rxn = 393.5 kJ 2H2 (g) + O2(g) > 2H2O (l) change of heat rxn = 571.6 kJ 2C2H2 (g) +5O2(g) > 4CO2(g) +2H2O

Somebody please help me. A friend of mine is trying to figure this out and I don't know how to help her because I haven't learned this. A student heats a 15.0 gram metallic sphere of unknown composition to a temperature of 98°C. The sphere is transferred

What amount of energy is required to melt a 26.9 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg1 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

In lab, Will burns a 0.6 peanut beneath 48 of water, which increases in temperature from 22 to 46. The amount of heat absorbed by the water can be found with the equation , where is the amount of heat, the specific heat of water, the mass of water, and

Use the first law of thermodynamics to determine the amount of heat change, Q, and whther it was added to or removd from the system. W=225J Delta U=600J Q=?

What amount of energy is required to melt a 27.4 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg1 Heat required to melt the ice 9.12e3 = J What amount of energy must be removed from 123 g of water to cool it from 71.6oC to 9.41oC? Specific heat

14. Using the equation of q = nCΔT determine the amount of energy required to raise the temperature of 24g of water 80ᵒC, with a heat capacity of 75.3 J/(mol*ᵒC )


Calculate the amount of heat required to heat 80 grams of water from 10 to 53°C. The specific heat capacity for water is 4.184 J/g°C.

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

Calculate the amount of heat required to heat a 3.8 gold bar from 30 to 67. Specific heat capacity of gold is 0.128 .

Determine the type of chemical reaction, find the limiting reagent, determine the amount of product in grams, and the amount in grams of excess reagent. Calcium nitrate is decomposed with heat to give calcium nitrite and oxygen gas. Start with 15.99g of

A Carnot engine takes an amount of heat QH = 113 J from a hightemperature reservoir at temperature TH = 1170°C, and exhausts the remaining heat into a lowtemperature reservoir at TL = 13.3°C. Find the amount of work that is obtained from this process

help please I keep reading about heat in my book and just cant get it. the amount of heat gained or lost by a substance is equal to the product of its _______ times the change in _______. Within a closed container, the heat lost by one substance must be

Calculate the amount of heat (in calories) required to raise the temperature of 200g of water from 20C to 50C. The specific heat of water is 1.00 cal/g. I have done other spacific heat problems but on this one i don't know how to start...

how to determine the amount of water in the container when you are given a 200g piece of aluminium at 90 degrees celcius is placed in a 100g glass container which holds an unknown amount of water at 20 degrees celcius .if the equilibrium temperature is

Posted by Connie on Saturday, September 10, 2011 at 10:36am. What is the amount of energy of calories to heat 8.5g of water from 15 C to 36 C? I think you take 8.5g x 21 degree C, but then I am stuck. Thank you Chem  Jai, Saturday, September 10, 2011 at

Use the calculation of specific heat for your metal as an example and determine the effect on specific heat if the sample temperature is changed. Does this small loss in heat significantly (>5%) affect your value for the specific heat of the metal? How


An aircooled motorcycle engine loses a significant amount of heat through thermal radiation according to the StefanBoltzmann equation. Assume that the ambient temperature is T0 = 24.5°C (297.65 K). Suppose the engine generates 11.5 hp (8.58 kW) of power

An aircooled motorcycle engine loses a significant amount of heat through thermal radiation according to the StefanBoltzmann equation. Assume that the ambient temperature is T0 = 24.5°C (297.65 K). Suppose the engine generates 11.5 hp (8.58 kW) of power

An aircooled motorcycle engine loses a significant amount of heat through thermal radiation according to the StefanBoltzmann equation. Assume that the ambient temperature is T0 = 22.3°C (295.45 K). Suppose the engine generates 13.5 hp (10.07 kW) of

Can somebody please help me with this question? That'd be great. Thanks! Determine the amount of heat needed in the following: the number of calories to heat 25 grams of water from 22 degrees celcius to 44 degrees celcius. Q= m c deltaTemp =

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

Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the

calculate the amount of heat energy required to raise the temperature of a 5kg block of solid platinum from 0 degrees celsius to 25 degrees celsius. the specific heat of platinum is 133j/kg k. how much heat energy is required to raise 5kg of water by the

For each trial, enter the amount of heat gained by the chemical system of ammonium nitrate, qrxn. The specific heat of water is 4.184 J/goC. Report your answer using 4 digits. The information given is: Trial # Tiwater Tf Masswater #1: 21.2 10.8 24.990 #2:

The body at higher temperature but having low amount of heat gives more severe pain of hotness than a body at low temperature but having high amount of heat. Give some examples.

Determine the amount of heat (in kJ) given off when 2.07 multiplied by 104 g of ammonia are produced according to the following equation. Assume that the reaction takes place under standardstate conditions at 25.0°C. N2(g) + 3 H2(g) 2 NH3(g) ΔH°rxn


135.2 J of heat energy are transferred to 24.75 g of mercury. By how much does the temperature increase? (in K) Specific heat of the mercury is 140 J/kg·°C. How much heat is needed to raise the temperature of 24.75 g of water by the same amount? Specific

how to determine the amount of water in the container when you are given a 200g piece of aluminium at 90 degrees celcius is placed in a 100g glass container which holds an unknown amount of water at 20 degrees celcius .if the equilibrium temperature is

which of the following quantities is not required to calculate the amount of heat energy required to heat water from 25^OC to 55^OC? Athe mass of water sample. Bthe initial temp. Cthe heat of vaporization for water. Dthe final temp. Ethe specific heat

The specific heat of water is 4.184 J/g degree C, and the specific heat of iron is 0.451 J/g degree C, which will reach a higher temperature when exposed to a given amount of heat?

which is false? Consider the following processes: I. Energy flows as heat from a hot object to a colder object II. Work is done on a system and an equivalent amount of energy is rejected as heat by the system III. Energy is absorbed as heat by a system and

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?

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 2.47 kg of steam at 100 °C releases when it

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

If an amount of heat q is applied to an object and its temperature changes by ÄT, the amount of heat that must be applied to change the temperature by 10ÄT is

What is the amount of heat involved in each of the following?kilojoules to heat 240 of gold from 20 to 188


What is the amount of heat involved in each of the following?kilojoules to heat 240 of gold from 20 to 188

Calculate the amount of heat required to heat a 42kg sample of ethanol from 14.0C to 18.0C

how is heat related to temperature? Temperature tells us the DEGREE of heat; i.e., how hot is something. A temperature of 98.6 F is normal body temperature. A hot day is when the temperature is 95 degrees F. A cold day is when it is freezing outside. But

Calculate the amount of heat, in kJ, needed to convert 30.0 g of ice at 5.2 oC to liquid water at 58 oC. Specific heat of ice = 2.10 J/(g oC); heat of fusion of ice = 334 J/g; Specific heat of water = 4.18 J/(g oC)

Determine the amount of heat (in kJ) given off when 2.23 multiplied by 104 g of ammonia are produced according to the following equation. Assume that the reaction takes place under standardstate conditions at 25.0°C. N2(g) + 3 H2(g) 2 NH3(g) ΔH°rxn

Consider the following equation: CO + 2 H2 → CH3OH ΔH rxn = 128 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H2. How would u set that up?

calculate the amount of heat energy required to melt a 1kg iron ingot initially at 20 ¡ãC? (heat of fusion for Fe is 33.0 J/g

The amount of heat required to raise 200 g of aluminum by 10 degrees celsius if its specific heat is 0.897 J/gC ? I need help. This is all confusing.

A heat pump works on the vapor compression refrigeration cycle with 0.2 kg/s of refrigerant134a as the working fluid. The cycle is used to keep a house at 26oC while absorbing heat from the outside at 3oC. R134a enters the compressor at 200 kPa as a

A solid cylindrical rod made from a center cylinder of lead and an outer concentric jacket of copper.Except for its ends,the rod is insulated,so that the loss of heat from the curved surface is negligible.When a temperature difference is maintained between


the amount of heat gained or lost by a substance is equal to the product of its heat capacity times the change in temperaturetimes its _____________

"Most of the solar radiation is absorbed by the atmosphere and much of what reaches the earth's surface is radiated back into the atmosphere to become heat energy." What can you conclude about heat energy? Most of the sun's energy is used to make heat

Assume a piece of hot metal is added to a calorimeter containing 50mL of water at 22C. The amount of heat released by the metal was determined to be 1000J, and the equilibrium temperature in the calorimeter was 26C. Remembering that the specific heat of

Assume a piece of hot metal is added to a calorimeter containing 50mL of water at 22C. The amount of heat released by the metal was determined to be 1000J, and the equilibrium temperature in the calorimeter was 26C. Remembering that the specific heat of

Calculate the amount of heat required to heat a 4.0kg gold bar from 20∘C to 61∘C. Specific heat capacity of gold is 0.128 J/g∘C. How do we figure this out?

27% of heat produced by the stove's gas burner is transferred to the soup in the covered pot, the rest is lost. Determine the total mass in grams of methane that must be burned to heat 800 ml of water from 22 to 90 degrees C. The density is 1.08 g/ml and

When an amount of heat is transferred at a steady temperature, what happens to the entropy of the system gaining the heat? a.It decreases. b.It increases. c.It is lost to its surroundings. >>> d.It is unchanged.

Calculate the amount of heat required to heat a 3.3kg gold bar from 30 ∘ C to 63 ∘ Specific heat capacity of gold is 0.128 J/g ∘ C.

Insolation refers to the amount of solar energy that reaches a body, such as a planet. the amount of heat energy contained in a beam of sunlight. the imaginary line that runs around Earth's middle. the spherical shape of Earth I don't know this one. The

An electric kettle rated accurately at 2.5kw is used to heat 3kg of water from 15% to boiling point it takes 9.5 minute. Then the amount of heat that has been lost is


Calculate the amount of heat energy required to raise the temperature of 2g of mercury[specific heat capacity 0.12J g10 C1] from 10degree C to 30degree C? Options: A. 3.0J. B. 3.5J. C. 4.0J. D. 4.8J

Can someone please help me with the following? How do I find the specific heat of a metal when the only information I have is a temperature change ( of 73 degrees C) and a mass (of 22.53 grams)? And what is the forumla for specific heat? Thanks in

3.98mL of 2.902M HCL are reacted with 15mL of 3.198 M NaOH. Use molar heat of neutralization to determine the kJ of heat produced. molar heat of neutralization is 55.84kJ/mol.

Calculate the amount of heat required to heat a 3.7{\rm kg} gold bar from 30^\circ {\rm C} to 61^\circ {\rm C}. Specific heat capacity of gold is 0.128 \rm J/g ^\circ C

Calculate the amount of heat required to heat a 3.6{\rm kg} gold bar from 20^\circ {\rm C} to 70^\circ {\rm C}. Specific heat capacity of gold is 0.128 \rm J/g ^\circ C