Calculate the heat (in Joules) involved in the process when 124 grams of water goes from a temperature of 11.5°C to 21.5°C.  The specific heat capacity of water is 4.184 J/(g °C).

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.39 kg sample of C4H₂O from -8.1 °C to 11.7 °C. The experiment shows that 4.58 × 104 J of heat are needed. What can the chemist report for the molar heat capacity of C4H₂O? Be sure your answer has the correct number of significant digits. - 1 .K J. mol - 1 x10 X Ś

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 1.65kg 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

A 151.6-g sample of a metal at 74.7°C is added to 151.6 g  at 15.9°C. The temperature of the water rises to 18.2°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C ⋅ g. Specific heat capacity =  ________J/°C ⋅ g

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.57 kg sample of a pure substance from 18.0 °C to 35.9 °C. The experiment shows that 19. 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 J. g x10

An unknown substance has a mass of 10.1 g. The temperature of the substance increases from 27.5 °C to 43.1 °C when 37.0 J of heat is added to the substance. The table lists the specific heats of select substances. Substance Specific heat [J/(g °C)] What is the most likely identity of the unknown substance? lead 0.128 aluminum silver 0.235 silver сорper 0.385 сорper iron 0.449 aluminum 0.903 lead water 4.184 iron water

Part A A silver block, initially at 55.8 °C, is submerged into 100.0 g of water at 24.1°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.3 °C. The specific heat capacities for water and silver are = 4.18 J/(g ·°C) and 0.235 J/(g·°C). What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units. Cs, water • View Available Hint(s) Cs, silver = HA ? Value Units m =

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 5.30 kg of water at 26.9 °C. During the reaction 78.1 kJ of heat flows out of the flask and into the bath. -1 -1 Round your 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 ¹·K answer to 3 significant digits. 1°C x10 X Ś ?

Can you explain where did I go wrong, I keep getting the same answer.