Question

1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C.

2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C).

3. You order a 16 oz glass of tea (where the mass of water is 474 grams) from a local restaurant. The tea is freshly brewed and has an initial temperature of 21.67 °C. You add ice to cool it. If the heat of fusion of ice is 6.020 kJ/mol and each ice cube contains exactly 1 mol of water, how many ice cubes are necessary to cool the tea to 1.13 °C? The specific heat of the "tea" is 4.184 J/g*C. Record your answer as a whole number.

4. A 63.57 gram sample of iron (with a specific heat of 0.450 J/g^oC) is heated to 100.0 ºC. It is then transferred to a coffee cup calorimeter containing 30.97 g of water (specific heat of 4.184 J/ g ºC) initially at 20.63 ºC. If the final temperature of the system is 23.59, what was the heat absorbed (q) of the calorimeter? (Hint: remember that the total heat absorbed by the water AND the calorimeter = the heat released by the iron.) Record your answer as a whole number (assume the sign is positive).

Answer 1

my dear student you posted multiple questions as per HOMEWORKLIB RULES I have solved the first one question Thank you.