A metal sample weighing 42.6 g and at a temperature of 100.0 oC was placed in...
A metal sample weighing 42.6 g and at a temperature of 100.0 oC was placed in 40.6 g of water at 24.8oC. At equilibrium the final temperature of the water and metal was 35.0oC. a. What was the change in temperature for the water? oC b. What was the temperature change for the metal? oC c. Taking the specific heat of water to be 4.184J/goC,caculate the specific heat of the metal. J/goC d. What is the approximate molar mass of the metal? g/mol
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A metal sample weighing 42.6 g and at a temperature of 100.0 oC
was placed in...
A metal sample weighing 43.5 g at a temperature of 100.0 °C was placed in 39.9...
A metal sample weighing 43.5 g at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1°C. At equilibrium, the temperature of the water and metal was 33.5°C. What was ΔT for the water? (ΔT = Tfinal - Tinitial) What was ΔT for the metal? Using the specific heat of water (4.184 J/g°C), calculate how much heat flowed into the water. Calculate the specific heat of the metal.
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in...
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium, the temperature of the water and metal was 33.5 °C. Determine the specific heat capacity of the metal.
Pre lab Q8 A piece of metal weighing 1.00 g at a temperature of 46.9 oC...
Pre lab Q8 A piece of metal weighing 1.00 g at a temperature of 46.9 oC was placed in a calorimeter in 20.20 mL of water at 16.7 oC . The final equilibrium temperature was found to be 28.8 oC . What is the specific heat of the metal? (----------) J/K-g
Show complete calculations for each question. 1. A metal sample weighing 35.0 g and at a...
Show complete calculations for each question. 1. A metal sample weighing 35.0 g and at a temperature of 99.1°C was placed in 50.0 g of water in a calorimeter at 200°C. The calorimeter reached a final temperature of 233°C. a. What was ar,ater. (T,inal-T,nitial) b. What was Δ7,etal. c. How much heat flowed into the water? d. Calculate the specific heat capacity of the metal. J/(g·°C) oC C(water) = 4.18 J/(g·°C) e. What is the approximate molar mass of the...
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in...
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium the temperature of the water and metal was 33.5 °C. 1. What is the unknown metal?
A metal sample weighinh 45.2 g and at a temperature of 100.0 C was placed in...
A metal sample weighinh 45.2 g and at a temperature of 100.0 C was placed in 38.6 g of water in an aluminum calorimeter at 25.2 C. The mass of the calorimeter is 70.4 g and its specific heat is 0.900 J/gC. At equilibrium the temperature of the water, metal and calorimeter was 33.0 C. A. How much heat flowed into the water and calorimeter? Total heat gained = heat gained by calorimeter + heat gained by water OR q=(mass)(s)(changeT)...
a) A 430 mL sample of water was cooled from 100.0 oC to 30.0 oC . How much...
a) A 430 mL sample of water was cooled from 100.0 oC to 30.0 oC . How much heat was lost? b) How many kilojoules are required to change the temperature of 26.5 g of water from 19.8 oC to 29.0 oC ? c) Calculate the final temperature when 10 mL of water at 80 oC are added to 20 mL of water at 25 oC d) A piece of metal weighing 2.00 g at a temperature of 41.0 oC was placed in a calorimeter in 19.10 mL of water...
A metal sample weighing 24.000 g is heated to 100.0 degrees celsius and then transferred into a calorimeter containing 3...
A metal sample weighing 24.000 g is heated to 100.0 degrees celsius and then transferred into a calorimeter containing 30.0 mL of water at a temperature of 22.8 degrees celsius. If the specific heat of the metal is 0.105 J/g*C, what is the final temperature of the metal sample plus water?
A piece of metal of mass 35.0 g at 100.0°C was placed in 150.0 g of...
A piece of metal of mass 35.0 g at 100.0°C was placed in 150.0 g of water at 20.0 °C. After stirring, the final temperature of the water and the metal is 23.8°C. What is the specific heat capacity of the metal? (specific heat capacity for H2O = 4.184 J/g °C) O-0.89 J 8°C 19.6 J/g °C 1.96J/g °C O 0.89 J/g °C
A piece of metal weighing 5.50 g at a temperature of 34.5 °C was placed in a calorimeter in 32.35 mL of water at 22.5 °...
A piece of metal weighing 5.50 g at a temperature of 34.5 °C was placed in a calorimeter in 32.35 mL of water at 22.5 °C. The final equilibrium temperature was found to be 27.5 °C. What is the specific heat of the metal? IVO AQ * R 0 O ? J/K-g
Show complete calculations for each question. 1. A metal sample weighing 35.0 g and at a temperature of 99.1°C was placed in 50.0 g of water in a calorimeter at 200°C. The calorimeter reached a final temperature of 233°C. a. What was ar,ater. (T,inal-T,nitial) b. What was Δ7,etal. c. How much heat flowed into the water? d. Calculate the specific heat capacity of the metal. J/(g·°C) oC C(water) = 4.18 J/(g·°C) e. What is the approximate molar mass of the...
A piece of metal of mass 35.0 g at 100.0°C was placed in 150.0 g of water at 20.0 °C. After stirring, the final temperature of the water and the metal is 23.8°C. What is the specific heat capacity of the metal? (specific heat capacity for H2O = 4.184 J/g °C) O-0.89 J 8°C 19.6 J/g °C 1.96J/g °C O 0.89 J/g °C
A piece of metal weighing 5.50 g at a temperature of 34.5 °C was placed in a calorimeter in 32.35 mL of water at 22.5 °C. The final equilibrium temperature was found to be 27.5 °C. What is the specific heat of the metal? IVO AQ * R 0 O ? J/K-g
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