A chemist carefully measures the amount of heat needed to raise the temperature of a 748.0 mg sample of a pure substance from 5.2 °C to 25.0 °C. The experiment shows that 13.4 J 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 -1 ?

It took 4.15x 10^3 J energy to raise the temperature of a piece of copper metal from 31 degrees Celcius to 84 degrees Celcius. What is the mass of the piece of metal? The specific heat of copper is .0908 cal/g degrees Celcius.

You will find the final temperature when 5.00 grams of aluminum at 425℃ is placed in 50.0 grams of water at 19.5℃. Aluminum has a specific heat capacity of 0.900 J/g ℃. And water has a specific heat capacity of 4.184 J/g℃. Now set –q(hot) = q(cold) and solve for the final temperature (as done in class) and then give the calculator answer for the final temperature! (Give 7 digits). Select one: a. 8.755643 ℃ b. 26.35996 ℃ c. 12.39981 ℃ d. 28.64197 ℃ e. 29.70363 ℃ f. 10.58574 ℃ g. 30.47036 ℃ h. none of these i. 26.81358 ℃ j. 28.03884 ℃

If 227.9 Joules of heat are added to 25.96 grams of a liquid, raising the temperature of the liquid from 27°C to 33.8°C, what is the specific heat capacity of the liquid with units of J/g•°C? Report your answer with 3 significant figures.

A 325.7 gram sample of copper is initially at 20.8 °C, and it absorbs 17.88 kJ of heat from its surroundings. What is its final temperature? (specific heat = 0.387 J g¹ °C-1 for copper) Do not put units in your answer. Give your answer to one decimal place.

A piece of metal weighing 73.10 g was heated to 99.3°C and then put into 30.00 g of water (initially at 17.4°C ). The metal and water were allowed to come to the same temperature, determined to be 30.6°C . Assuming no heat lost to the environment, calculate the specific heat of the metal. (CH20 = 4.181 J/g°C ) Round your answer to 2 decimal places.

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.98 kg sample of C4H₂O from -0.4 °C to 11.4 °C. The experiment shows that 4.18 × 10* 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. J-mol -1 -1 ☐ x10

In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a metal. She heats 19.7 grams of iron to 99.34°C and then drops it into a cup containing 83.8 grams of water at 20.66°C. She measures the final temperature to be 22.66°C. Assuming that all of the heat is transferred to the water, she calculates the specific heat of iron to be J/g °C.

In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a metal. She heats 18.4 grams of titanium to 98.86°C and then drops it into a cup containing 75.9 grams of water at 23.43°C. She measures the final temperature to be 25.59°C. Assuming that all of the heat is transferred to the water, she calculates the specific heat of titanium to be J/g°C.

For the following questions (Q11-Q14), consider the compound NH4Cl, ammonium chloride, having a molar mass of 53.491 g/mol. Nicole weighs out 12.41g of NH4Cl and also 125.0 g of water for her calorimetry experiment. Nicole dissolves her ammonium chloride in the water and finds that the temperature of the water decreases from 23.7°C to 17.3°C. Assume the specific heat capacity of the water, Cs,water, is 4.184 J/(g °C) and that no energy is transferred to the calorimeter (qcal = 0 J)   Q11. Find the heat (in J) transferred to the water, qwater, during the process NH4Cl (s) ® NH4Cl (aq). Use the equation qwater = mwater Cs,water ∆T.   Q13. Using your result in Q11, calculate the enthalpy of reaction, ∆Hrxn, in units of kJ/mol.