Calorimeter constant is defined as the quantity of heat capacity of calorimeter.
it simple baised on the concept
Heat lost by hot body = heat gained by cold body
If 100 g of aluminum at 90°C were placed in a calorimeter with 50 g of...
An aluminium block is heated to 100 °C and then placed immediately in 100 g of water which is initially at a temperature of 25.0 °C in a coffee cup calorimeter. Once the system reaches thermal equilibrium, the temperature of the water that surrounds the block is 28.0 °C. Calculate the mass of the aluminium block. The specific heat capacity of Al is 0.900 J g^–1 K^–1 and for H2O is 4.184 J g^–1 K^–1
A 100 g aluminum calorimeter contains 250 g of water. The two substances are in thermal equilibrium at 10°C. Two metallic blocks are placed in the water. One is a 50 g piece of copper at 76°C. The other sample has a mass of 73 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20°C. Determine the specific heat of the unknown second sample. J/kg·°C
A 100. g sample of water at 25.3 C was placed in a calorimeter. 45.0 g of lead shots (at 100 C) was added to the calorimeter and the final temperature of the mixture was 34.4 C. What is the specific heat of lead? 100.0g
6. During a calorimetry experiment, 50 ml of H2O is placed in the calorimeter at 20° C. Specific heat of H2O is 4.184 (J/g °C). Upon placing 8.0g of compound X, the temperature of the H2O in the calorimeter increases to 30.5* C. Calculate the heat of dissolution for compound X? Assume no heat exchange with the calorimeter
An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10°C. Two metallic blocks are placed into the water. One is a 51.0-g piece of copper at 80°C. The other has a mass of 544 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20°C. (a) Determine the specific heat of the unknown sample. (J/Kg*C) (b) Using the...
2. Steam at a temperature of 110 C is added to an aluminum calorimeter containing 250g of water at 30°C. The mass of the calorimeter is 140g and of specific heat 0.22 calg.Co. Find the mass of steam specitic hea needed that will produce a mixture of temperature 50°C. (Assume no heat is lost or gained from the surrounding.)
4. You placed 43.1 g of an unknown metal at 100 °C into a coffee cup calorimeter that contained 50.0 g of water that was initially at 22.0 °C. The equilibrium temperature of mixing (T0) was determined to be 23.7 °C. The calorimeter constant was known to be 51.5 J/°C. Specific HeatH2O = 4.184 J/g·°C a. What is the total amount of heat (J) lost by the metal? NG 1.5 b. What was the specific heat (J/g·°C) of the metal?...
A
100 g aluminum calorimeter contains 250 g of water. The two
substances are in thermal equilibrium at 10°C. Two metallic blacks
are placed in water. One is a 50 gram piece of copper at 82°C. The
other sample has a mass of 57 g and is originally at a temperature
of 100°C. The entire system stabilizes at a final temperature of
20°C. Determine the specific heat of the unknown second sample.
A 100 g aluminum calorimeter contains 250 g...
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 10.95 g sample of lead at 88.0°C was placed into a styrofoam cup calorimeter which contained 15 mL of water at 22.0°C. The final temperature in the calorimeter reached 23.5°C. Calculate the specific heat of lead. The specific heat of water is 4.184 J/g°C.