Fill the graduated cylinder with hot tap water and let stand for one minute. Pour water...
Fill the graduated cylinder with hot tap water and let stand for one minute. Pour water into the sink. Measure 70 mL of hot water. Pour the water into the foam cup. Measure the temperature of the water. Add an ice cube to the cup of water. Gently swirl the cup. Measure the temperature of the water as soon as the ice cube has completely melted. Pour the water into the graduated cylinder and measure the volume. The initial temperature of the hot water was 54.9 degrees Celcius and the final temperature after the ice cube is 18.3 degrees Celcius.
Questions:
1. Determine the mass of the ice.
2. Calculate the amount of heat transferred from the water to the ice.
3. Determine ∆Hfus of ice (kJ/mol) by dividing the heat transferred from the water by the moles of ice melted.
4. Compare your experimental value of ∆Hfus of ice with the accepted value of 6.01 kJ/mol. Account for any error.
(Thank you so much for your help, I appreciate it!)
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Fill the graduated cylinder with hot tap water and let stand for
one minute. Pour water...
Fill the graduated cylinder with hot tap water and let stand for one minute. Pour water into the sink. Measure 70 mL of...
Fill the graduated cylinder with hot tap water and let stand for one minute. Pour water into the sink. Measure 70 mL of hot water. Pour the water into the foam cup. Measure the temperature of the water. Add an ice cube to the cup of water. Gently swirl the cup. Measure the temperature of the water as soon as the ice cube has completely melted. Pour the water into the graduated cylinder and measure the volume. The initial temperature...
Use the 100 mL graduated cylinder to measure and pour 50 mL of distilled water into Beaker 1. Use the 100 mL graduated c...
Use the 100 mL graduated cylinder to measure and pour 50 mL of distilled water into Beaker 1. Use the 100 mL graduated cylinder to measure and pour 48 mL of distilled water into Beaker 2. Use the 10 mL gradated cylinder to measure and pour 1 mL of saturated sodium bicarbonate solution into Beaker 1. Then, add 2 drops of phenol red to Beaker 1. Gently mix the solution. Use the straw to blow bubbles into Beaker 1. Start...
a hot piece of iron at 75 degrees celsius was dropped on a 15g ice cube...
a hot piece of iron at 75 degrees celsius was dropped on a 15g ice cube at 0 degrees celsius. after a few minutes, both the iron and the water stayed at 0 degrees celsius but the ice melted completely. what is the mass of the iron? (Ciron = 0.0449 J/g degrees celsius, △Hfus = 6.00 kJ/mol)
You make a cup of hot coffee and pour it into an insulated container that already...
You make a cup of hot coffee and pour it into an insulated container that already has ice in it. Assume that the insulated container itself has a very small heat capacity so that any energy transferred from it or to it is negligible and can be ignored. What energy systems are changing. starting from when you pour the coffee into the insulated container to when the ice is completely melted and the mixture has a uniform temperature? Ethermal, coffee,...
Fill the ice mold with tap water and put it in a freezer for 24 hours....
Fill the ice mold with tap water and put it in a freezer for
24 hours. Remove the
mold from the freezer, loosen the ice but do not remove the
ice and place the mold upside
down in a thin paper plate and place the plate on a thick
coffee table or dining table (see
Figure 1). Wait for about 30 minutes, using the cell-phone or
digital watch as a timer, and
then measure the amount of water in the...
Fill the ice mold with tap water and put it in a freezer for 24 hours....
Fill the ice mold with tap water and put it in a freezer for
24 hours. Remove the
mold from the freezer, loosen the ice but do not remove the
ice and place the mold upside
down in a thin paper plate and place the plate on a thick
coffee table or dining table (see
Figure 1). Wait for about 30 minutes, using the cell-phone or
digital watch as a timer, and
then measure the amount of water in the...
To cool her 0.200 kg cup of 75.0 C hot chocolate (mostly water), Heidi drops a...
To cool her 0.200 kg cup of 75.0 C hot chocolate (mostly water), Heidi drops a 29,.97 g ice cube at 0 C into her insulated cup. After the ice cube melts, the temperature of the hot chocolate comes down to 54.8 C. a. How much energy was lost by the hot chocolate? The specific heat capacity of water is 1 cal/g C b. How much energy was gained by the ice cube just to melt to 0 C water?...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...
Lab 9 Heat of Reaction OBJECTIVE: To experimentally determine the heat of reaction for two exothermic...
Lab 9 Heat of Reaction
OBJECTIVE:
To experimentally determine the heat of reaction for two
exothermic reactions.
DISCUSSION:
The heat given off or gained in a reaction is called the heat
of reaction (∆?????????).
A reaction that releases heat is known as an exothermic
reaction; an endothermic reaction
is one that absorbs heat.
The heat of the reaction corresponds to one mole of the
reactant and is expressed in
kilocalories per mole of reactant or in kilojoules per mole of...
1. An unknown sample is being evaluated in lab. What is the specific heat of the...
1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C. 2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the...
You make a cup of hot coffee and pour it into an insulated container that already has ice in it. Assume that the insulated container itself has a very small heat capacity so that any energy transferred from it or to it is negligible and can be ignored. What energy systems are changing. starting from when you pour the coffee into the insulated container to when the ice is completely melted and the mixture has a uniform temperature? Ethermal, coffee,...
Fill the ice mold with tap water and put it in a freezer for
24 hours. Remove the
mold from the freezer, loosen the ice but do not remove the
ice and place the mold upside
down in a thin paper plate and place the plate on a thick
coffee table or dining table (see
Figure 1). Wait for about 30 minutes, using the cell-phone or
digital watch as a timer, and
then measure the amount of water in the...
Fill the ice mold with tap water and put it in a freezer for
24 hours. Remove the
mold from the freezer, loosen the ice but do not remove the
ice and place the mold upside
down in a thin paper plate and place the plate on a thick
coffee table or dining table (see
Figure 1). Wait for about 30 minutes, using the cell-phone or
digital watch as a timer, and
then measure the amount of water in the...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...
Lab 9 Heat of Reaction
OBJECTIVE:
To experimentally determine the heat of reaction for two
exothermic reactions.
DISCUSSION:
The heat given off or gained in a reaction is called the heat
of reaction (∆?????????).
A reaction that releases heat is known as an exothermic
reaction; an endothermic reaction
is one that absorbs heat.
The heat of the reaction corresponds to one mole of the
reactant and is expressed in
kilocalories per mole of reactant or in kilojoules per mole of...
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