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21. A 25.0 g of a metal at 195.0°C is dropped into 155 g water at...
Question 21 6 21. A 25.0 g of a metal at 195.0°C is dropped into 155...
Question 21 6 21. A 25.0 g of a metal at 195.0°C is dropped into 155 g water at 25.0°C. After the heat exchange the final temperate is 35.0°C. Calculate the specific of metal. cof H2O(1) = 4.184J/g°C 0.0261 J/goC 1.62 J/goC 0.188 J/goC 3.01 J/goC Question 20 20. Determine the type of intermolecular forces in CHCl3. Z of C = 6, Cl = 17, H = 1 electronegativities: Cl = 3.0, and C = 2.5, H = 2.1 only...
A hot metal at 125 oC was dropped into 75.0 g of water kept at a...
A hot metal at 125 oC was dropped into 75.0 g of water kept at a room temperature of 20.6 oC in a calorimeter. Within a couple of minutes, water’s temperature increased to 26.8 oC? (a) How much heat energy was absorbed by water? [‘c’ for water is 4.184 J/goC] (b) How much heat energy was released by the metal? (c) What information is needed to calculate the specific heat capacity of the metal?
3. A 32.520 g piece of unknown metal was heated in a hot water bath at 99.80°C. The hot metal was then transferred...
3. A 32.520 g piece of unknown metal was heated in a hot water bath at 99.80°C. The hot metal was then transferred to a coffee-cup calorimeter containing 100.0 mL of water. Time-Temperature data was collected and plotted. From the plot, the initial and final tem- peratures for the water were determined to be T 23.76°C and T 26.18°C. and qse (Assume C 21.0 J°C.) a. Calculate cal b. Calculate qnetal Calculate cmetal d. Calculate the molar mass for the...
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker...
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K). 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K) Previous Page Next Page Page 22 of 24 Submit Quiz 0 of 24 questions saved
A hot 105.8 g lump of an unknown substance initially at 179.7 °C is placed in 35.0 mL of water initially at 25.0 °C and...
A hot 105.8 g lump of an unknown substance initially at 179.7 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 77.4 °C. Substance Specific heat (J/(g·°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184 Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no...
Question 19 When 27.0 g of an unknown metal at 88.4 °C is placed in water,...
Question 19 When 27.0 g of an unknown metal at 88.4 °C is placed in water, the metal is cooled and loses 1300 J of energy. If the final temperature of the water and metal is 23.7 °C, what is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 lg-k. O 0.74 J/g-K O 1.4g. O 0.34 J/g-K O 0.98J/g.K Next Question 20 Calculate AH for the following reaction, CaO(s) + CO2(g) - CaCO3(s)...
Only question 4 Pliz!! ULT Appron male equul number of points de 3. A 32.520 g piece of unknown metal was heated...
Only question 4 Pliz!!
ULT Appron male equul number of points de 3. A 32.520 g piece of unknown metal was heated in a hot water bath at 99.80°C. The hot metal was then transferred to a coffee-cup calorimeter containing 100.0 mL of water. Time-Temperature data was collected and plotted. From the plot, the initial and final tem- peratures for the water were determined to be T = 23.76°C and T, = 26.18°C. a. Calculate qcal and water (Assume Cal...
Calorimetry. Specific Heat of a Metal and Heat of Reaction 4. When 25.0 mL of 1.00...
Calorimetry. Specific Heat of a Metal and Heat of Reaction 4. When 25.0 mL of 1.00 M sodium hydroxide, NaOH(aq) is added to 25.0 mL of 1.00 M sulfuric acid, H,SO, (aq), at 22.3°C, the temperature rises to 31.2°C. Assume the solution is sufficiently dilute, so its specific heat is 4.184 J/gºC and its density is 1.00 g/ml. a. Write the balanced chemical equation for the reaction of sulfuric acid with sodium hydroxide. b. Calculate and colution (Assume C =...
Question 21 6 21. A 25.0 g of a metal at 195.0°C is dropped into 155 g water at 25.0°C. After the heat exchange the final temperate is 35.0°C. Calculate the specific of metal. cof H2O(1) = 4.184J/g°C 0.0261 J/goC 1.62 J/goC 0.188 J/goC 3.01 J/goC Question 20 20. Determine the type of intermolecular forces in CHCl3. Z of C = 6, Cl = 17, H = 1 electronegativities: Cl = 3.0, and C = 2.5, H = 2.1 only...
3. A 32.520 g piece of unknown metal was heated in a hot water bath at 99.80°C. The hot metal was then transferred to a coffee-cup calorimeter containing 100.0 mL of water. Time-Temperature data was collected and plotted. From the plot, the initial and final tem- peratures for the water were determined to be T 23.76°C and T 26.18°C. and qse (Assume C 21.0 J°C.) a. Calculate cal b. Calculate qnetal Calculate cmetal d. Calculate the molar mass for the...
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K). 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K) Previous Page Next Page Page 22 of 24 Submit Quiz 0 of 24 questions saved
Question 19 When 27.0 g of an unknown metal at 88.4 °C is placed in water, the metal is cooled and loses 1300 J of energy. If the final temperature of the water and metal is 23.7 °C, what is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 lg-k. O 0.74 J/g-K O 1.4g. O 0.34 J/g-K O 0.98J/g.K Next Question 20 Calculate AH for the following reaction, CaO(s) + CO2(g) - CaCO3(s)...
Only question 4 Pliz!!
ULT Appron male equul number of points de 3. A 32.520 g piece of unknown metal was heated in a hot water bath at 99.80°C. The hot metal was then transferred to a coffee-cup calorimeter containing 100.0 mL of water. Time-Temperature data was collected and plotted. From the plot, the initial and final tem- peratures for the water were determined to be T = 23.76°C and T, = 26.18°C. a. Calculate qcal and water (Assume Cal...
Calorimetry. Specific Heat of a Metal and Heat of Reaction 4. When 25.0 mL of 1.00 M sodium hydroxide, NaOH(aq) is added to 25.0 mL of 1.00 M sulfuric acid, H,SO, (aq), at 22.3°C, the temperature rises to 31.2°C. Assume the solution is sufficiently dilute, so its specific heat is 4.184 J/gºC and its density is 1.00 g/ml. a. Write the balanced chemical equation for the reaction of sulfuric acid with sodium hydroxide. b. Calculate and colution (Assume C =...
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