Suppose that the molar enthalpy of a reaction is -61.27 kJ/mol and 4.799 moles are reacted. How many kilojoules of heat are released by the reaction? Report your answer to three decimal places (ignore significant figures).

3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.)  J What is the specific heat (in J/g·°C) of the metal?  J/g·°C 4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?  J Is the reaction exothermic or endothermic? exothermicendothermic  5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions?  kJ/mol methane 6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much…

The enthalpy change when a strong acid is neutralized by strong base is –56.1 kJ/mol.  If 12.0 mL of 6.00 M HBr at 21.30°C is mixed with 300. mL of 0.250 M NaOH, also at 21.30°C, what will the maximum temperature reached by the resulting solution? (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.)

The ΔH value for the reaction is -90.8 kJ. How much heat is released when 198.1 g Hg is reacted with oxygen?

A metal with a specific heat of 0.899 J/g oC had an initial temperature of 76.67 oC. When it was placed in a coffee-cup calorimeter filled with 26.7 g of water, the temperature of the water increased 5.0 degrees to a final temperature of 35.0 oC. Calculate the mass of the metal sample added. The specific heat of water is 4.18 J/g oC. (Ignore contributions from the cup)

4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).

Heat energy of 566.0 kJ is absorbed when 2 mol carbon dioxide decomposes to carbon monoxide and oxygen gas. What is its thermochemical equation?

When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.

A piece of metal with a specific heat of 1.153 J/gºC is heated to 124.6ºC and then placed in 120.382 g of water which is at a temperature of 2.1 ºC.  After a minute, the temperature of the water has stopped changing and is now 45.5ºC.   Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.