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.5 M H2O4 17) A 100-gram sample of copper at 100.0°C is added to 50.0 grams...
5) A 70.5 gram piece of metal, initially at 255 °C, is rapidly transferred to 100.0...
5) A 70.5 gram piece of metal, initially at 255 °C, is rapidly transferred to 100.0 mL of distilled water, which is initially at 19.6 °C. The temperature of the water increases to 30.8 °C. Given that the density of the water = 1.00 g/mL, calculate the specific heat (J/g °C) of the metal. The specific heat of water is 4.184 J/g °C. 9- (SH)(m)(AT) A) 0.632 B) 3.37 C) 5.17 D) 0.0234 E) 0.296
1211 L postlab Calorimetry - in both cases ignore the calorimeter A 248-8 sample of copper...
1211 L postlab Calorimetry - in both cases ignore the calorimeter A 248-8 sample of copper is dropped into 390 to be 39.9"C. Calculate the initial temperature of the copper. Density of water 1.00/mL. Specific heat of copper - 384 1/8" 590 R of water at 22.500 The final temperature wash When 50.0 mL of .10 M HCl and 50,0 mL of .10 M NAOH, both at 22°C. are added to a calorimeter, the temperature of the mixture reaches 28.9°C....
A 30.5 g sample of copper at 99.8 °C is carefully placed into an insulated container...
A 30.5 g sample of copper at 99.8 °C is carefully placed into an insulated container containing 207 g of water at 18.5 °C. Calculate the final temperature when thermal equilibrium is reached. Assume there is no energy transferred to or from the container. Specific heat capacities: Cu =0.385 Jg-loc- H20 - 4.184 Jgloc!
When 50.0 mL of .10 M HCl and 50.0 mL of .10 M NaOH, both at...
When 50.0 mL of .10 M HCl and 50.0 mL of .10 M NaOH, both at 22 oC, are added to a calorimeter, the temperature of the mixture reaches 28.9 oC. Calculate the heat produced by this reaction. Density of water 1.00g/mL. Specific heat of water = 4.184 J/g oC
18. When a piece of copper at a temperature of 256.0 °C is added to 255...
18. When a piece of copper at a temperature of 256.0 °C is added to 255 grams of water at a temperature of 20.0 °C, the final temperature of the resulting mixture is 24.0 °C. If the specific heat capacity of copper is 0.385 J/g°C, calculate the mass of the piece of copper used in the experiment? The specific heat capacity of water is 4.184 J/ g• °C. (5 points)
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
In a constant-pressure calorimeter, 50.0mL of 0.340 M Ba(OH)2 was added to 50.0 mL of 0.680...
In a constant-pressure calorimeter, 50.0mL of 0.340 M Ba(OH)2 was added to 50.0 mL of 0.680 M HCı The reaction caused the temperature of the solution to the same density and specific heat as water (1.00 g/mL and 4.184 J g ℃ respectively), what is dH for this reaction (per mole of H20 produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/ mol H,O
In a constant pressure calorimeter 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL...
In a constant pressure calorimeter 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL of 0.620 M HCl. the reactions caused the temperature of the solution to rise from 23.77 c to 27.99 c if the solution has the same density and same specific heat as water (1.00 g/mL and 4.184 j/g c ) what is triangle H for this reaction (per mole of H2O produced) assume that the total volume is the sum of the individual volumes
In a constant-pressure calorimeter, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of...
In a constant-pressure calorimeter, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 24.49 C to 29.26 C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g• C) respectively), what is ?H for this reaction (per mole H2O produced)? Assume and the total volume is the sum of the individual volumes. ?H= _______ kJ/mol H2O
175.0 grams of an unknown metal at 85.0°C is added to 75.00 grams of water (cs...
175.0 grams of an unknown metal at 85.0°C is added to 75.00 grams of water (cs = 4.184 J/g.°C) at 21.0°C in an insulated container. If the final temperature of the metal and water is 26.2°C then what is the specific heat capacity (Cs) of the metal? Select one: a. -0.16 J/g.°C b. 0.16 J/g.°C c. 6.3 J/g.°C O d.-6.3 J/g.°C e. 1.4 J/g.°C
5) A 70.5 gram piece of metal, initially at 255 °C, is rapidly transferred to 100.0 mL of distilled water, which is initially at 19.6 °C. The temperature of the water increases to 30.8 °C. Given that the density of the water = 1.00 g/mL, calculate the specific heat (J/g °C) of the metal. The specific heat of water is 4.184 J/g °C. 9- (SH)(m)(AT) A) 0.632 B) 3.37 C) 5.17 D) 0.0234 E) 0.296
1211 L postlab Calorimetry - in both cases ignore the calorimeter A 248-8 sample of copper is dropped into 390 to be 39.9"C. Calculate the initial temperature of the copper. Density of water 1.00/mL. Specific heat of copper - 384 1/8" 590 R of water at 22.500 The final temperature wash When 50.0 mL of .10 M HCl and 50,0 mL of .10 M NAOH, both at 22°C. are added to a calorimeter, the temperature of the mixture reaches 28.9°C....
A 30.5 g sample of copper at 99.8 °C is carefully placed into an insulated container containing 207 g of water at 18.5 °C. Calculate the final temperature when thermal equilibrium is reached. Assume there is no energy transferred to or from the container. Specific heat capacities: Cu =0.385 Jg-loc- H20 - 4.184 Jgloc!
18. When a piece of copper at a temperature of 256.0 °C is added to 255 grams of water at a temperature of 20.0 °C, the final temperature of the resulting mixture is 24.0 °C. If the specific heat capacity of copper is 0.385 J/g°C, calculate the mass of the piece of copper used in the experiment? The specific heat capacity of water is 4.184 J/ g• °C. (5 points)
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
In a constant-pressure calorimeter, 50.0mL of 0.340 M Ba(OH)2 was added to 50.0 mL of 0.680 M HCı The reaction caused the temperature of the solution to the same density and specific heat as water (1.00 g/mL and 4.184 J g ℃ respectively), what is dH for this reaction (per mole of H20 produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/ mol H,O
175.0 grams of an unknown metal at 85.0°C is added to 75.00 grams of water (cs = 4.184 J/g.°C) at 21.0°C in an insulated container. If the final temperature of the metal and water is 26.2°C then what is the specific heat capacity (Cs) of the metal? Select one: a. -0.16 J/g.°C b. 0.16 J/g.°C c. 6.3 J/g.°C O d.-6.3 J/g.°C e. 1.4 J/g.°C
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