a) Heat is often used as a sterilization method for stainless steel medical tools. Calculate the the final temperature that would be measured when 25.56 kJ is absorbed by a 500 g stainless steel dental tool if its initial temperature is 285 K. Use 54.9 g mol-1 as the molar mass of stainless steel, and 24.2 J mol-1 K-1 as the constant pressure heat capacity of stainless steel. Be sure to indicate the correct units in your final answer. b) Is this experiment measuring the change in internal energy or the change in enthalpy? Provide an explanation to support your answer.

A 46.9-g iron rod, initially at 18.6 oC is submerged into 50.4 g of water at an unknown initial temperature.  The final temperature of the mixture upon reaching thermal equilibrium is 69.6 oC.  What is the initial temperature of the water (in oC)? The specific heat capacity of iron is 0.449 J/g.oC The specific heat capacity of water is 4.184 J/g.oC

A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC.  After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams.  For this problem, assume the  specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures.  What is the heat transferred by this reaction, in Joules?

the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

Measurements show that the enthalpy of a mixture of gaseous reactants increases by 195.kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 69.kJ of work is done on the mixture during the reaction.  Calculate the change in energy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. Is the reaction exothermic or endothermic?

A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 6.30 kg of water at 21.7 °C. During the reaction 143. kJ of heat flows out of the bath and into the flask. 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¯¹. Round your answer to 3 significant digits.