A student is using a calorimeter to determine the specific heat of a metallic sample. She measures out 162.5 grams of her metal and heats it to 86.9 degrees Celsius. Then, she puts the sample into a calorimeter containing 10.77 grams of water at 47.5 degrees Celsius. She measures the temperature of the water in the calorimeter until the number stops changing, then records the final temperature to be 55.3 degrees Celsius. What is the specific heat of the metal?

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 6.10kg of water at 22.7°C. During the reaction 61.9kJ 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 is4.18·J·g−1K−1. Be sure your answer has the correct number of significant digits.

A piece of unknown metal with a mass of 24.31 g is heated in boiling water to 90.51°C and then dropped into a coffee cup calorimeter containing 71.4 g of water at 18.67°C. When thermal equilibrium is reached, the final temperature is 25.22°C. Calculate the specific heat capacity of the unknown metal. The specific heat of water is 4.184 J/g/°C.   Round your answer to 2 decimal places.

A hot 101.5 g lump of an unknown substance initially at 157.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 36.1 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. O zinc O graphite O tungsten O titanium O rhodium O aluminum Substance Specific heat (J/(g-°C)) 0.897 0.709 0.243 0.523 0.132 0.388 4.184 aluminum graphite rhodium titanium tungsten zinc water

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A 500.0g sample of an unknown substance, initially at 20.2 degree celsius, was heated with 1.55kJ of energy. the final temperature of the substance was 125.0 degree celsius. Determine the specific heat of this substance.

A chemist carefully measures the amount of heat needed to raise the temperature of a  539.0g  sample of a pure substance from  −1.8°C  to  4.4°C . The experiment shows that  1.5kJ  of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.

A chemist carefully measures the amount of heat needed to raise the temperature of a 112.0 g sample of a pure substance from 27.4 °C to 44.1 °C. The experiment shows that 8.79 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits. 1 J.g¹.K - 1 x10 X S ? 0⁰

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.40kg of water at 30.9°C. During the reaction 130.kJ 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

A 56.43 g sample of iron (with a heat capacity of 0.450 J/g·°C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 47.87 g of water (specific heat of 4.184 J/g·°C) initially at 20.63 °C. If the final temperature of the system is 23.59 °C, how much heat was absorbed by the calorimeter? Record your answer as a whole number in joules, and assume the sign is positive.