11 A chemist carefully measures the amount of heat needed to raise the temperature of a 511.0 mg sample of C4H₁₁N from 4.7 °C to 18.2 °C. The experiment shows that 17.7 J of heat are needed. What can the chemist report for the molar heat capacity of C4H₁₁N? Round your answer to 3 significant digits. -1 − 1 ☐ J. mol · K ☐ x10 ☑

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.54 kg sample of C5H₁2S from 5.8 °C to 17.4 °C. The experiment shows that 3.51 × 104 J of heat are needed. What can the chemist report for the molar heat capacity of C5H₁2S? Be sure your answer has the correct number of significant digits. 12 - 1 – 1 K J. mol x10 X Ś 6 0 U

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 38.7 °C. During the reaction 55.6 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 -1 4.18 J∙g¯¹·K¯¹. Be sure your answer has the correct number of significant digits. 心。 °℃ x10 S

An experiment was conducted to determine the specific heat of platinum.  It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC.  Based on these experimental results calculate the specific heat (J/g⋅⋅oC) of platinum.

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

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.65kg sample of C9H10O2 from 25.9°C to 37.9°C. The experiment shows that 3.09 X 104J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2? Round your answer to 3 significant digits.   =   J * mol-1 * K-1

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.

A chemist carefully measures the amount of heat needed to raise the temperature of a 531.0mg sample of C9H10O2 from 40.1°C to 58.2°C . The experiment shows that 15.1J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2 ? Be sure your answer has the correct number of significant digits. ⋅J⋅mol−1K−1

A 158 g sample of gold at some temperature was added to 28.7 g of water. The initial water temperature was 18.4 °C, and the final temperature was 23.2 °C. If the specific heat capacity of gold is 0.128 J/g · °C, what was the initial temperature of the gold sample? The specific heat capacity of water is 4.184 J/g ⋅ K.