If a student used a sample of metal that was wet, a significant percentage of the...
Homework Answers
Calorimetry is the science associated with determining the changes in energy of a system by measuring the heat exchanged with the surroundings. The heat capacity of metal would be too high than really it is because water has higher heat capacity than any metal.
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If
a student used a sample of metal that was wet, a significant
percentage of the...
subject: calorimetry Post Laboratory Questions 1. A student places 138 g of an unknown metal at...
subject: calorimetry
Post Laboratory Questions 1. A student places 138 g of an unknown metal at 99.9°C into 60.00 g of water at 22.2 °C. The entire system reaches a uniform temperature of 31.5 °C. Calculate the specific heat capacity of the metal. 2. If the correct specific heat of the metal in problem 1 is 0.25 J/gºC, calculate the percent crror. 3. While transferring the piece of unknown metal to the calorimeter, the student dropped the metal into the...
A student measured a mass of a metal bar as 57.21 g. The student filled a...
A student measured a mass of a metal bar as 57.21 g. The student filled a graduated cylinder with water and determined the volume of water to be 48.60 ml Then the student placed the metal bar into the graduated cylinder and determined the new volume to be 53.70 mL Calculate the density of the metal and identify its name from the choices that appear in Table 1.2. A chemist has a 9.50 ml, sample of rubbing alcohol (isopropyl alcohol)....
A wet aggregate sample was weighed with 305.2 N. Its dry weight after 24 hours in...
A wet aggregate sample was weighed with 305.2 N. Its dry weight after 24 hours in an oven was measured with 285.2 N. The used aggregate has an absorption of 2.75 %. a)Determine the percentage of free water in the wet sample.
A 48.79 g sample of metal is heated to 98.77oC and then quickly transferred to 88.34...
A 48.79 g sample of metal is heated to 98.77oC and then quickly transferred to 88.34 mL of water at 24.65oC contained in a new calorimeter. This calorimeter has a calorimeter constant (heat capacity) with a numerical value of 55.7 (see problem 2e above for appropriate units). The thermal equilibrium temperature of the metal sample plus water mixture was 27.49oC. Assume the density of the water is 1.00 g/mL. a. How much heat in Joules is gained by the water?...
2) A student boils a metal block for 2 minutes and the temperature of the boiling...
2) A student boils a metal block for 2 minutes and the temperature of the boiling water is 105.1 °C. the metal block has a mass of 250.42 g. The metal object is removed from the boiling water and submerged in 130.00 mL of water at 23.7 °C. The equilibrium temperature was 36.9 °C. a) Assuming no heat was lost to the surrounding, determine the specific heat capacity of the metal. (6 points) b) Calculate the percent error if the...
The experiment this is in reference to is the determination of molar mass of a metal....
The experiment this is in
reference to is the determination of molar mass of a metal. a piece
of magnesium ribbon was dangled on a copper wire into a tube with
tap water and hydrochloric acid then placed into a beaker of water
that was at room temperature.
Questions 1. Practice: Oxygen can be generated by thermal decomposition of potassium chlorate: 2 KClO3 (s) —> 2 KCl (s) + 3 O2 (g) Calculate the volume of oxygen (in liters) produced...
help Error Analysis 1. In parts A, B, and C, if the calorimeter was not dry,...
help
Error Analysis 1. In parts A, B, and C, if the calorimeter was not dry, the change in temperature would be too (high/low). This would make the |AH| appear too _(high/low). 2. If a reaction is exothermic, the sign of AH is and heat is 3. If a reaction is endothermic, the sign of AH is and heat is 4. In the determination of the specific heat of the metal, if some of the water that was used to...
1. The crucible is not fired, as the procedure suggests. The mass of the dirty crucible...
1. The crucible is not fired, as the procedure suggests. The mass of the dirty crucible is recorded. However, the impurities are burned off in the experiment. Will the reported mass of the final product be too high, too low, or unchanged as a result of this technique error? Too high Too low Unaffected 2. If you put more water than is needed for reaction 3, and then did not dry out this excess water, what effect (if any) would...
Following the procedure in lab, a student heated their 36.353 g metal sample to 100.0°C ....
Following the procedure in lab, a student heated their 36.353 g metal sample to 100.0°C . The metal was added to a coffee cup calorimeter containing 20.079 g of water at 21.9 *C . The final temperature of the water was 36 "С . Assuming no heat was absorbed by the calorimeter, calculate the specific heat of the metal. Report your answer in units of
1. for each of the given situations, tell how the error will affect the calculated specific...
1. for each of the given situations, tell how the error will affect the calculated specific heat. Will it be too high, too low, or have no effect on the result? explain your answer. a. the balance used to determine the mass of the metal was in error by 10g on the high side. In other words, the balance gave a larger mass than the true mass. b. it was thought that the metal was in the boiling water long...
subject: calorimetry
Post Laboratory Questions 1. A student places 138 g of an unknown metal at 99.9°C into 60.00 g of water at 22.2 °C. The entire system reaches a uniform temperature of 31.5 °C. Calculate the specific heat capacity of the metal. 2. If the correct specific heat of the metal in problem 1 is 0.25 J/gºC, calculate the percent crror. 3. While transferring the piece of unknown metal to the calorimeter, the student dropped the metal into the...
A student measured a mass of a metal bar as 57.21 g. The student filled a graduated cylinder with water and determined the volume of water to be 48.60 ml Then the student placed the metal bar into the graduated cylinder and determined the new volume to be 53.70 mL Calculate the density of the metal and identify its name from the choices that appear in Table 1.2. A chemist has a 9.50 ml, sample of rubbing alcohol (isopropyl alcohol)....
2) A student boils a metal block for 2 minutes and the temperature of the boiling water is 105.1 °C. the metal block has a mass of 250.42 g. The metal object is removed from the boiling water and submerged in 130.00 mL of water at 23.7 °C. The equilibrium temperature was 36.9 °C. a) Assuming no heat was lost to the surrounding, determine the specific heat capacity of the metal. (6 points) b) Calculate the percent error if the...
The experiment this is in
reference to is the determination of molar mass of a metal. a piece
of magnesium ribbon was dangled on a copper wire into a tube with
tap water and hydrochloric acid then placed into a beaker of water
that was at room temperature.
Questions 1. Practice: Oxygen can be generated by thermal decomposition of potassium chlorate: 2 KClO3 (s) —> 2 KCl (s) + 3 O2 (g) Calculate the volume of oxygen (in liters) produced...
help
Error Analysis 1. In parts A, B, and C, if the calorimeter was not dry, the change in temperature would be too (high/low). This would make the |AH| appear too _(high/low). 2. If a reaction is exothermic, the sign of AH is and heat is 3. If a reaction is endothermic, the sign of AH is and heat is 4. In the determination of the specific heat of the metal, if some of the water that was used to...
Following the procedure in lab, a student heated their 36.353 g metal sample to 100.0°C . The metal was added to a coffee cup calorimeter containing 20.079 g of water at 21.9 *C . The final temperature of the water was 36 "С . Assuming no heat was absorbed by the calorimeter, calculate the specific heat of the metal. Report your answer in units of
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