copper calorimeter can with mass 0.100 kg contains 0.160 kg of water and 0.0180 kg of ice in thermal equilibrium at atmospheric pressure. If 0.750 kg of lead at 225 o C is dropped into the calorimeter can, what is the final temperature? Assume no heat is lost to the surroundings.

A high-pressure gas cylinder contains 50 L of toxic gas at a pressure of 1.5.107 N/m² and a temperature of 23 °C. Its valve leaks after the cylinder is dropped. The cylinder is cooled to dry ice temperature -78.5 °C to reduce the leak rate and pressure so that it can be safely repaired. (a) What is the final pressure in the tank, assuming a negligible amount of gas leaks while being cooled and that there is no phase change? P: 9837079 Pa (b) What is the final pressure if one-tenth of the gas escapes? P 8853371 Pa (c) To what temperature must the tank be cooled to reduce the pressure to 1.00 atm (assuming the gas does not change phase and that there is no leakage during cooling)? T: 200.331 K (d) Does cooling the tank appear to be a practical solution to bring the pressure down and reduce the leak? Assume N, N2. Take into account the values calculatesd in parts (a) through (c). No ! No, that's only partially correct

(a) How much heat transfer (in kcal) is required to raise the temperature of a 0.650 kg aluminum pot containing 3.00 kg of water from 10.0°C to the boiling point and then boil away 0.600 kg of water? X kcal Enter a number. (b) How long (in s) does this take if the rate of heat transfer is 600 W (1 watt = 1 joule/second (1 W = 1 J/s))?

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.95-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 60.0°C? Assume any water turned to steam subsequently recondenses. kg

What mass of water at 22.0°C must be allowed to come to thermal equilibrium with a 1:80 kg cube of aluminum Initially at 150"C to lower the Leimperature of the aluminum to 66.0°C? Assune any water turned to steam subsequently recondenses. kg Need Help? Read It

If 4.00 × 104 J of heat energy is required to turn water ice at −10.0º C to steam at 100º C, what was the mass of the block of ice? Note– this is not a sublimation problem.

An insulated beaker of negligible mass contains 0.250 kg of water at a temperatureof 75.0◦C. How much ice at a temperature of 0.00◦C must be dropped in so the finaltemperature of the system will be 30.0◦C?

A 1.19-kg sample of water at 13°C is in a calorimeter. You drop a piece of steel with a mass of 0.31 kg at 224°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation taken together don't affect the outcome, as we'll see later. Hint   The final equilibrium temperature of water and steel is °C. If the water is in a glass beaker with a mass of 0.2 kg, which in turn is in a calorimeter, with the beaker at the same temperature as the water, how will this affect the answer? Try answering before doing a detailed calculation.   Final temperature will be higher but not significantly so. Final temperature will be significantly lower. Final temperature will be lower but not significantly so. Final temperature will be significantly higher.   Using the setup in (b), the final equilibrium temperature of…

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.90-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 70.0°C? Assume any water turned to steam subsequently recondenses. kg

a cup of coffee sits on a table in an insulated mug. to coool the coffee down a ice block is added. the inital mass of coffee in the mug is 90g. the intial temperature of the coffee is 90 degree celsius. the ice block has started to melt and is then put into the coffee. the ice melts and the new temperature of the cofee is 78 degree c and the new mass is 110g. the ice block (final-intital mass) is 20g. what are teh tempeartuare changes for the coffee and ice (started at 0 degree celsius) also if specific heat of water is used for both the coffee and ice waht is the heat energy lost by the coffee and the heat energy gained by the ice after it melted?