. You pour 108 cm³ of ethanol, at a temperature of –10.0 ° C, into a graduated ylinder initially at 20.0 °C, filling it to the very top. The cylinder is made of lass with a specific heat of 840 J/kg•K and a coefficient of volume expansion f 1.2x10-5 1/K; its mass is 0.110 kg. The mass of the ethanol is 0.0873 kg. (a) What will be the final temperature of the ethanol, once thermal equilibrium is reached? (b) How much ethanol will overflow the cylinder before thermal equilibrium is reached?

When 0.8451 g of naphthalene (C10H8) combusts in a bomb calorimeter, the temperature rises by 1.538°C. What is AUrxn for the reaction in kJ/mol naphthalene? The heat capacity of the bomb calorimeter is 22.15 kJ/°C. O Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimale.g. 2.5E5 for 2.5 x 10) Type your numeric answer and submit

If a 136.51 g Al rod (c = 0.900 J/g°C) is at 100.0°C and placed into 250.0 g of water at 21.8°C, what is the temperature of the system (rod + water) at equilibrium assuming %3D no losses to the surroundings? Assume the specific heat of water to be 4.18 J/g°C. (A 46°C 30°C c) 206°C 18°C

Phenol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard heat of combustion of phenol, CH,OH(s), is -3054 kJ/mol. Given that AHICO,(0)) = -393.5 kJ/mol and AH(H,0(01 = -285.8 kJ/mol, what is the standard enthalov of formation of phenol? +328.8 ký/mol -164.4 kj/mal - 164.4 ki/mol -328.8 kj/mol

The thermite reaction, used for welding iron, is the reaction of FegO4 with Al. 8 Al (s) + 3 Fe3O4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 16.5 g of Al with 76.7 g of Fe304? Enter your numerical answer in units of kJ.

and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8

Specific Heat of a Metal Data and Calculations Identity of metal Mass of metal (g) Volume of DI water (mL) Mass of DI water (g) Tinitial metal (°C) Tinitial water (°C) Tfinal of mixture after addition of metal (°C) Specific heat of metal Cmetal (J/(g.°C)) Trial 1 Aluminum 19.657 50.0 50.0 100.4 100.4 30.6

Find the mass of water that vaporizes when 2.10 kg of mercury at 205 °C is added to 0.10 kg of water at 30°C. Assume the following: Cmercury (specific heat capacity of mercury) - 139 J/(kg.°C): Cwater (specific heat capacity of water) = 4186 J/(kg.°C); and L, (water) = 2.26x106 J/kg

When 40 g of a metal at 85 ◦C is added to48 g of water at 23 ◦C, the temperature of thewater rises to 29 ◦C. What is the specific heatcapacity of the metal? Assume no heat waslost to the surroundings.Answer in units of J/g · ◦C

Find the minimum amount of energy it takes to raise 1.00 pound of lead (454g) from room temperature 25 Celsius to its melting point 327 Celsius and then melt it.