1) For part A, calculate q (the heat lost in calories) for copper and lead. The...
1) For part A, calculate q (the heat lost in calories) for copper and lead. The specific heats of these metals are in the background section. Then calculate q (the heat gained in calories) for the water in each case. Remember that you used 25.0 g of water in the experiment. Show your calculations
2)The heat lost by the metal and the heat gained by the water should be the same. Are they? If not, list possible sources of error.
Mass of copper: 28.43g
Mass of lead: 22.00g
Initial temp of water: 23 C
Initial temp of all metals: 98C
Final temp of copper + water: 27C
Final temp of lead + water: 23C
Specific heat of water is 1.000 cal/g C
specific heat of copper is 0.092 cal/g C
Specific heat of lead is 0.031 cal/g C
Homework Answers
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1) For part A, calculate q (the heat lost in calories) for
copper and lead. The...
Data: Part A: Assuming Perfectly Insulated System where QlostQgained Round all values to 1 decimal place...
Data: Part A: Assuming Perfectly Insulated System where QlostQgained Round all values to 1 decimal place (don’t worry about significant figures) Find Swater and Scopper in the background section of your lab manual. Specific heat of water is (1.000 cal/g degree celsius). Specific heat of copper is (0.092 cal/g degree celsius). Heat of fusion of water is (80.0 cal/g degree celsius). Mass of Copper 20 g Volume of water (assume density of 1g/mL to get mass) 25 mL Initial temperature...
Lab-10: Calorimetry: Specific Heat of a Metal DATA SHEETS: Reference: Chapter Notes-10 and Lab Manual (Pages...
Lab-10: Calorimetry: Specific Heat of a Metal DATA SHEETS: Reference: Chapter Notes-10 and Lab Manual (Pages 64 to 70) Use the following You Tubes to get more information https://youtu.be/8gHFOL2990U https://youtu.be/HlvilF6MI9c Calculate the Specific Heat and identify the Metal Observation Mass Mass of Metal (ml): 87.87 g Mass of polystyrene cup (m2): 2.32 g Mass of cup with water (m3): 72.82 g Mass of water in the cup (m3-m2): 70.5 g Temperature Initial temp. of Metal (the boiling water temperature (t1):...
What is als? Assume that no heat is lost to the surroundings (Hint: The heat gained...
What is als? Assume that no heat is lost to the surroundings (Hint: The heat gained by the gold must be equal to the heat lost by the iron. The specific heats of the metals are given in Table 6.2.) To a sample of water at 23.4°C in a constant- 6.36 pressure calorimeter of negligible heat capacity is added a 12.1-g piece of aluminum whose tempera- ture is 81.7°C. If the final temperature of water is 24.9°C, calculate the mass...
2.3. V 2.40 How many calories of heat are required to change 12 g of ice...
2.3. V 2.40 How many calories of heat are required to change 12 g of ice from -10°C to water at 25°C? [Given: Cice=0.5 cal/g/°C; Cwater = 1 cal/g/°C] Calorimeter problem to find the specific heat of lead: If 110 g of lead shot at 120°C is dropped into 60 g of water at 25°C contained in a copper calorimeter of 45 g mass, what is the resulting temperature? [Given: Cwater I cal/g/°C; Cpb*** 0.031 cal/g/°C; Ccu = 0.093 cal/g/°C]
2.4. Calorimeter problem to find the specific heat of lead: If 110 g of lead shot...
2.4. Calorimeter problem to find the specific heat of lead: If 110 g of lead shot at 120°C is dropped into 60 g of water at 25°C contained in a copper calorimeter of 45 g mass, what is the resulting temperature? [Given: Cwater = 1 cal/g/°C; Cpb = 0.031 cal/g/°C; Ccu = 0.093 cal/g/°C]
Use the heat equation to calculate the energy, in joules and calories, for each of the...
Use the heat equation to calculate the energy, in joules and calories, for each of the following (see the table): Specific Heats for Some Substances Substance cal/g ∘Ccal/g ∘C J/g ∘CJ/g ∘C Elements Aluminum, Al(s)Al(s) 0.214 0.897 Copper, Cu(s)Cu(s) 0.0920 0.385 Gold, Au(s)Au(s) 0.0308 0.129 Iron, Fe(s)Fe(s) 0.108 0.452 Silver, Ag(s)Ag(s) 0.0562 0.235 Titanium, Ti(s)Ti(s) 0.125 0.523 Compounds Ammonia, NH3(s)NH3(s) 0.488 2.04 Ethanol, C2H6O(s)C2H6O(s) 0.588 2.46 Sodium chloride, NaCl(s)NaCl(s) 0.207 0.864 Water, H2O(s)H2O(s) 1.00 4.184 Water, H2O(s)H2O(s) 0.485 2.03 a.)...
what is the heat lost by copper snd the heat capacity of calorimeter? EXPERIMENT 7 Thermochemistry:...
what is the heat lost by copper snd the heat capacity of
calorimeter?
EXPERIMENT 7 Thermochemistry: Calorimetry and Hess's Law Data Sheet Part A-Calibration of the Calorimeter Mass of copper Mass of empty, dry calorimeter Mass of calorimeter plus water 172.1146 168.602g 229.0189 60.416g 72.005 23.6 °C Mass of water 39.0°C Temperature of copper (boiling water, T) Initial temperature of calorimeter and water, T. Final temperature of metal/water mixture, T, AT for copper T AD AT for water Heat lost...
Heat of Neutralization: Determine DeltaT in (C) and calculate the total number of calories produced. the...
Heat of Neutralization: Determine DeltaT in (C) and calculate the total number of calories produced. the density of the 0.500 M NaCl produced is 1.02 g/mL, and its specific heat is 0.960 cal/g x C. Calculate the heat of neutralization per mole of water produced. Volume of HCl: 50.0 mL Concentration of HCl: 1.00 M Volume of NaOH: 50.0 mL Concentration of NaOH: 1.00 M Initial temperature: 29.0 C Final Temp 26.8 C
8. Use the data in the Introduction calculate the total amount of heat in kcal required...
8. Use the data in the Introduction calculate the total amount of heat in kcal required to turn 100 g of ice at -20°C to steam at 120°C? liq gas equilibrium (heat goes into phase change) Steam - Water and steam allas (heat goes into temperature change) Temperature (°C) all liquid (heat goes into temperature change) -Water Ice and water all solid Nice solid/liq equilibrium (heat goes into phase change) - Time Heat On the 5 sections of the graph...
1. Calculate the heat (expressed in calories) required to heat 115 g of water from 15.4^C...
1. Calculate the heat (expressed in calories) required to heat 115 g of water from 15.4^C to 91.4^C 2. Calculate the heat (in calories) lost by 115 g of water as it cools from 91.4^C to 15.4^C 3. Calculate the temperature change caused by absorption of 3.85 kcal heat by 75.4 g water 4. Calculate the final temperature of 75.4 g of water originally at 12.6^C after it absorbs 3.85 kcal of heat 5. A 23.9 g piece of metal...
Lab-10: Calorimetry: Specific Heat of a Metal DATA SHEETS: Reference: Chapter Notes-10 and Lab Manual (Pages 64 to 70) Use the following You Tubes to get more information https://youtu.be/8gHFOL2990U https://youtu.be/HlvilF6MI9c Calculate the Specific Heat and identify the Metal Observation Mass Mass of Metal (ml): 87.87 g Mass of polystyrene cup (m2): 2.32 g Mass of cup with water (m3): 72.82 g Mass of water in the cup (m3-m2): 70.5 g Temperature Initial temp. of Metal (the boiling water temperature (t1):...
What is als? Assume that no heat is lost to the surroundings (Hint: The heat gained by the gold must be equal to the heat lost by the iron. The specific heats of the metals are given in Table 6.2.) To a sample of water at 23.4°C in a constant- 6.36 pressure calorimeter of negligible heat capacity is added a 12.1-g piece of aluminum whose tempera- ture is 81.7°C. If the final temperature of water is 24.9°C, calculate the mass...
2.3. V 2.40 How many calories of heat are required to change 12 g of ice from -10°C to water at 25°C? [Given: Cice=0.5 cal/g/°C; Cwater = 1 cal/g/°C] Calorimeter problem to find the specific heat of lead: If 110 g of lead shot at 120°C is dropped into 60 g of water at 25°C contained in a copper calorimeter of 45 g mass, what is the resulting temperature? [Given: Cwater I cal/g/°C; Cpb*** 0.031 cal/g/°C; Ccu = 0.093 cal/g/°C]
2.4. Calorimeter problem to find the specific heat of lead: If 110 g of lead shot at 120°C is dropped into 60 g of water at 25°C contained in a copper calorimeter of 45 g mass, what is the resulting temperature? [Given: Cwater = 1 cal/g/°C; Cpb = 0.031 cal/g/°C; Ccu = 0.093 cal/g/°C]
what is the heat lost by copper snd the heat capacity of
calorimeter?
EXPERIMENT 7 Thermochemistry: Calorimetry and Hess's Law Data Sheet Part A-Calibration of the Calorimeter Mass of copper Mass of empty, dry calorimeter Mass of calorimeter plus water 172.1146 168.602g 229.0189 60.416g 72.005 23.6 °C Mass of water 39.0°C Temperature of copper (boiling water, T) Initial temperature of calorimeter and water, T. Final temperature of metal/water mixture, T, AT for copper T AD AT for water Heat lost...
8. Use the data in the Introduction calculate the total amount of heat in kcal required to turn 100 g of ice at -20°C to steam at 120°C? liq gas equilibrium (heat goes into phase change) Steam - Water and steam allas (heat goes into temperature change) Temperature (°C) all liquid (heat goes into temperature change) -Water Ice and water all solid Nice solid/liq equilibrium (heat goes into phase change) - Time Heat On the 5 sections of the graph...
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