A chemist carefully measures the amount of heat needed to raise the temperature of a 0.73 kg sample of C,H,Cl, from -0.2 °C to 14.5 °C. The experiment shows that 1.28 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,Cl,? Round your answer to 2 significant digits. ) -mol" K - 1 J•mol -1

An electrical heater is used to supply 205.0 J of energy to a 20.0 g sample of silver (specific heat is 0.237 J/(goC)), originally at 305.0 Kelvin. Determine the final temperature in Kelvin.

A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.103 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C.

0,11) G [References] Use the References to access important values if needed for this question. In the laboratory a student finds that it takes 58.2 Joules to increase the temperature of 11.7 grams of solid zinc from 25.0 to 38.6 degrees Celsius. The specific heat of zinc calculated from her data is J/g °C.

The specific heat of a certain type of metal is 0.128 J/(g⋅∘C). What is the final temperature if 305 J of heat is added to 58.2 g of this metal, initially at 20.0 ∘C?

In a calibration of a calorimeter, 50.3 g of water at 60.5 degrees C is added to 48.7g of water at 19.7 degrees C gives a mixture at 39.1 degrees C. What is the heat capacity of the calorimeter used in this experiment?

Calculate the energy required to heat 1.80kg of silver from 5.5°C to 19.1°C. Assume the specific heat capacity of silver under these conditions is 0.235J·g−1K−1. Round your answer to 3 significant digits.

The specific heat of a certain type of metal is 0.128 J/(g.°C). What is the final temperature if 305 J of heat is added to 63.2 g of this metal, initially at 20.0 °C? °C Tfinal ||

The temperature of an 6.95 g sample of an unknown metal increases from 22.0°C to 31.7°C upon the addition of 29.6 J of heat. The specific heat capacity of the metal is J/g-K.

1 . A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.290 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C. 2. 3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 15.41°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･°C and the density of the solution is 1.20 g/mL). 3. Using the equations 2 Fe (s) + 3 Cl₂ (g) → 2 FeCl₃ (s) ∆H° = -800.0 kJ/mol Si(s) + 2 Cl₂ (g) → SiCl₄ (s) ∆H° = -640.1 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s) 4. A sample of 2.30 g of potato chips was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 6.94 kcal/°C. The heat released caused the temperature of the calorimeter to increase 1.75°C. Calculate the food caloric content of…