Incandescent light bulbs can get very hot to the touch as they convert much of the electrical energy flowing through them into heat. A 60 W light bulb has a volume of 180.0 mL at SATP. The light bulb is switched on and the heated glass expands slightly to 180.5 mL with an internal pressure of 114.5 kPa. The new temperature of the light bulb in degrees C is:

A hot, 3.00 g metal ball at 140.oC was placed in 8.0 mL of cold water at 12oC. The specific heat capacity of the metal is 3.3 J/g◦C. What was the final temperature of the water? [Hint: Look up the density of water.]

If you combine 230.0 mL230.0 mL of water at 25.00 ∘C25.00⁢ ∘C and 140.0 mL140.0 mL of water at 95.00 ∘C,95.00⁢ ∘C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

1. The formation of gaseous phosphorus trichloride is shown below:   P4 (g) + 6 Cl2 (g) → 4 PCl3 (g)     ΔH = -1207 kJ/mol   If 4.30 kJ of heat are released as the formation reaction above proceeds, how many milliliters of gaseous phosphorus trichloride, measured at 35°C and 712 torr, will be produced?

1 " A 47.0 g sample of aluminum, which has a specific heat capacity of 0.897 J.g •°C is dropped into an insulated container containing 150.0 g of water at 20.0 °C and a constant pressure of 1 atm. The initial temperature of the aluminum is 95.0 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 X

please see the attached image

A sample of iron, which has a specific heat capacity of 0.449 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The iron sample starts off at 85.1 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 24.3 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 08 X S thermometer. insulated container water- sample a calorimeter 區 de

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6334 g sample of acetylsalicylic acid (C9H8O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.100×103 g of water. During the combustion the temperature increases from 22.68 to 25.23 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 929.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of acetylsalicylic acid based on these data. C9H8O4(s) + 9O2(g) 4 H2O(l) + 9 CO2(g) + EnergyMolar Heat of Combustion =   how many kJ/mol

1. The formation of gaseous phosphorus trichloride is shown below:   P4 (g) + 6 Cl2 (g) → 4 PCl3 (g)     ΔH = -1207 kJ/mol   If 4.30 kJ of heat are released as the formation reaction above proceeds, how many milliliters of gaseous phosphorus trichloride, measured at 35°C and 712 torr, will be produced?

A 5.0 g block of metal is heated to 124 °C and added to 145 mL of H2O, initially at 20.4 °C. if the metal is copper, what is the final temperature of the water?