Using the equations 2 H2 (g) + O2 (g) → 2 H¿0 (I) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH° = -635 kJ/mol CaO (s) + H2O (1) → Ca(OH)2 (s) AH° = -64 kJ/mol %3D Determine the enthalpy (in kJ/mol) for the reaction Ca (s) + 2 H20 (1) → Ca(OH)2 (s) + H2 (g).

A solution is made by mixing 197.3 g of ethanol initially at 10.5°C with 250.0 g of water initially at 21.3 °C. What is the final temperature of the solution assuming that no heat is lost? The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184J/g·°C.

of the resulting solution is Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter  at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the heat capacity 4.18 J/g °C?

You wish to find the enthalpy for the reaction 6 Gel (s) + 14 NH:1 (s) → 3 Ge:H6 (1) + 7 N2 (g) + 38 HI (g) kJ/mol Given the following equations Equation 1: 2 Ge (s) + 3 H2 (g) → Ge:H6 (1) AH = 137.3 kJ/mol Equation 2: Ge (s) + 4 HI (g) – Gel: (s) + 2 H2(g) AH = -247.8 kJ/mol Equation 3: 2 NH&| (s) → N2 (g) + 2 HI (g) + 3 H2(g) AH = 455.8 kJ/mol 2 4 C What would be the enthalpy change, in kJ/mol, for 6 Gel4 (s) + 12 H2(g) - 6 Ge (s) + 24 HI (g)? 7 8 9. +/- x 100 3. 1,

When 1.0 g of sodium hydroxide (40.00 g/mol) is added to a calorimeter containing 50.0 g water at 20.0 °C, the heat of solution (ΔHsoln) is -3.8x10^4 J/mol.   A)What is the final temperature reached by the mixture in the calorimeter? Assume the mass of the solution is equal to the mass of water and that Cp(solution)=4.18 J/(g•°C). Show all work.   B) Is the reaction endothermic or exothermic?

Dissolving 2.97 g of CaCl2(s) in 143.8 g of water in a calorimeter at 22.3 °C causes the temperature to rise to 25.9 °C. What is the change in enthalpy for this dissolution (in J), assuming the specific heat of the resulting solution is 4.184 J/g °C?

50.0 mL of hot water (49.6 oC) is added to 50.0 mL of cold water (24.7 oC).  Upon mixing the water reaches an equilibrium temperature of 36.3 oC.  Calculate the heat absorbed by the calorimeter in units of kJ/oC.  Heat capacity for water is 4.184 J/(g·oC). -0.0267 kJ/oC -0.383 kJ/oC 0.356 kJ/oC -0.449 kJ/oC -0.0307 kJ/oC

67.0 mL of hot water (45.4 oC) is added to 45.0 mL of cold water (22.3 oC).  Upon mixing the water reaches an equilibrium temperature of 35.1 oC.  Calculate the heat absorbed by the calorimeter in units of kJ/oC.  Heat capacity for water is 4.184 J/(g·oC). A-0.514 kJ/oC B-0.0463 kJ/oC C-0.0373 kJ/oC D-0.477 kJ/oC E-0.414 kJ/oC

A 90.0 g piece of metal, initially at 98.6°C, is placed into 120.0 g of water initially at 24.3°C. If the final temperature of the water is 34.0°C, what is the specific heat of the metal? (The specific heat of water is 4.18 J/g. °C).

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol