Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? D) Water.  You will need to look up specific heat values.

01. The enthalpy change in a reaction is 1366 kJ per mole. Should the enthalpy of the combustion reaction be positive or negative? Explain. a. Calculate the total energy change when 14.50 grams of carbon dioxide is produced.

A chemist measures the energy change AH during the following reaction: CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(l) Use the information to answer the following questions. This reaction is... Suppose 37.8 g of CH₁ react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. AH = -882. kJ endothermic. O exothermic. OYes, absorbed. O Yes, released. O No. kJ x10 Start over Ś

6. A substance increases in temperature by 55°C when a 98 g sample of it absorbs 80000 J of heat. What is the specific heat capacity of the substance?

If 67.2 J of heat is added to a 24.6 g sample of silver, how much will the temperature increase by?  The specific heat of silver is 0.235 J/goC.

Show work to support your answer to this question. a) In a study of gaseous xenon, a chemist finds that 27.6 J of energy must be added to increase the temperature of 10.7 g of xenon from 22.7° C to 39.9° C.  What is the experimental specific heat value for xenon gas? b) Using the specific heat you calculated for gaseous xenon, how much heat will be required to heat the 10.7 g sample of xenon from 39.9° C to 278.9° C?