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 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.
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 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 94.1 g metal sample is heated to 102.4°C and transferred to 100.0 g H20 at 22.0°C in a calorimeter. Equilibrium temperature is 26.4°C. Specific heat of metal is? {SH20=4.184 J/gºC; q=smAT; AT=Tfinal-Tinitial} Answer to 2 significant figures. Do not include the unit 18°C
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...
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...
please help me. Thanks A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
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
Part A A piece of metal weighing 3.00 g at a temperature of 47.3°C was placed in a calorimeter in 32.05 mL of water at 23.3°C. The final equilibrium temperature was found to be 28.0°C. What is the specific heat of the metal? O AE ROE?
. A 150.0 g sample of a Metal was heated to 95.0°C. When the hot metal was placed into 100.0 g of water in a calorimeter, the temperature of the water increased from 20.0°C to 35.0°C. The specific heat of water is 4.184 J/g °C. a) What is the specific heat of the metal? Kb) What would the final temperature be if the mass of water was 150.0 q?