2.10 kg of mercury (Hg) at 205 °C is mixed with 0.110 kg of water at 80.0 °C A in a well-insulated bucket of negligible heat capacity. What mass of water in grams that will transform to vapor?

A(n) 80-g ice cube at 0°C is placed in 990 g of water at 22°C. What is the final temperature of the mixture? °C

What quantity of heat (in J) would be required to convert 2.65 mol of a pure substance from a liquid at 40.0 °C to a gas at 113.0 °C? A Cliquid = 1.45 J/mol °C Tboiling = 88.5 °C Cgas = 0.65 J/mol °C AHvaporization = 1.23 kJ/mol

A copper sample (ccu = 387 J/kg•K) of mass mẹ = 75 g and temperature Te = 312ºC is dropped into a glass beaker that contains a mass of water me = 220 g (cw = 4190 J/kg•K). %3D The initial temperature of the water and the beaker is Tw,b = 12.0°C. What is the final temperature of the copper, beaker, and water? * The heat capacity (the specific heat times the mass) of the beaker is Cb' = 190 J/K.

9. A rigid tank contains 73.5 g of chlorine gas (Cl2) at a temperature of 74 °C and an absolute pressure of 5.30 × 10° Pa. Later, the temperature of the tank has dropped to 40 °C and, due to a leak, the pressure has dropped to 3.40 × 10° Pa. How many grams of chlorine gas have leaked out of the tank? (The mass per mole of Cl2 is 70.9 g/mol.) SSI f60 ssfo 50 ssf60 sf60 ssi

8. A rigid tank contains 71.5 g of chlorine gas (Cl₂). a temperature of 70 °C and an absolute pressure of 5.80 x 105 Pa. Later, the temperature of the tank has dropped to 32 °C and, due to a leak, the pressure has dropped to 3.30 x 105 Pa. How many grams of chlorine gas have leaked out of the tank? (The mass per mole of Cl₂ is 70.9 g/mol.) 9 6 ntm 2

A 0.150-kg sample of a metal alloy is heated at 540 Celsius an then plunged into a 0.400-kg of water at 10.0 Celsius, which is contained in a 0.200-kg aluminum calorimeter cup. The final temperature of the system is 30.5 Celsius. What is the specific heat of the metal alloy in J/Kg.Celsius? 497 74.60 50.00 3316 994

275 g of cold water at 5.00 °C is mixed with 125 g of hot water at 80.0 °C. Assuming no energy is lost, what is the final temperature of the mixture? 21.6°C O 37.5 °C Ⓒ 28.4 °C 56.6 °C QUESTION 13 75 g of metal at 100 °C is mixed with 250 g of water at 20 °C and reaches an equilibrium temperature of 25 °C. What was the specific heat of the metal? 0.049 cal/g °C 9.8x10-3 cal/g °C 1.5 cal/g °C 0.22 cal/g °c

Water at 30.0 °C is sprayed onto 0.144 kg of molten gold at 1063 °C (its melting point). The water boils away, forming steam at 100.0 °C and leaving solid gold at 1063 °C. What is the minimum mass of water that must be used? mw =