A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.60 kg of water at 25.3 °C. During the reaction 80.6 kJ of heat flows out of the flask and into the bath. -1 Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J-g K¹ 7. Be sure your answer has the correct number of significant digits. 1°C 5

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.61 kg sample of a pure substance from 3.0 °C to 24.2 °C. The experiment shows that 32. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. 1 - 1 ·K x10

The specific heat capacity of solid iodine is 0.427 J/g⋅⋅oC.  Calculate the final temperature (°C) when 747.0 J of heat is added to a 186.5g sample of solid iodine initially at 13.3°C. Please use the correct significant digit   I got my answer as 22.3; however, it is incorrect. I am a bit lost on why.

Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J J cal kJ 678 109 0.843

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.55 kg sample of a pure substance from 7.7 °C to 14.6 °C. The experiment shows that 5.5 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. DJ-g`1 - K-1 ☐ x10 X

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains  8.80kg  of water at  20.5°C . During the reaction  66.3kJ  of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is  4.18·J·g−1K−1 . Be sure your answer has the correct number of significant digits.   °C

Calculate the energy required to heat 141.0mg of mercury from −1.1°C to 17.8°C . Assume the specific heat capacity of mercury under these conditions is 0.139J·g−1K−1 . Be sure your answer has the correct number of significant digits.

The heat change of the reaction Al2Cl6(s) + 6 Na(s) ⎯→ 2Al(s) + 6 NaCl(s) is –256.2 kcal. The heat of formation of solid NaCl is –98.3 kcal ; calculate the heat of formation of solid Al2Cl6.  Observe proper number of significant figures.

A piece of metal with a mass of 59.047 g was heated to 98.0 °C and then put it into 100.0 g of water initially at 23.7 °C.  The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C.  Assuming no heat lost to the environment, calculate the specific heat (J/g⋅⋅oC) of the metal.  Please round to correct significant figures. I answered 0.414 J/g*c and got it wrong.

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.46 kg sample of a pure substance from 36.2 °C to 51.6 °C. The experiment shows that 33. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.