A 12.88-g block of solid platinum at 61.54 °C is immersed in a 21.78-g pool of liquid ethanol with a temperature of 13.43 °C. When thermal equilibrium is reached, what is the temperature of the platinum and ethanol? Specific heat capacities: platinum = 0.133 J/g °C; ethanol = 2.44 J/g °C
A 12.88-g block of solid platinum at 61.54 °C is immersed in a 21.78-g pool of...
A14.92-g block of solid lead at 67.50 °C is immersed in a 23.82-g pool of liquid ethanol with a temperature of 12.55 °C. When thermal equilibrium is reached, what is the temperature of the lead and ethanol? Specific heat capacities: lead - 0.159 Jig °C; ethanol = 2.44 J/g "C
A 12.87-g block of solid iron at 68.39 °C is immersed in a 21.10-g pool of liquid propylene glycol with a temperature of 12.68 °C. When thermal equilibrium is reached, what is the temperature of the iron and propylene glycol? Specific heat capacities: iron = 0.444 J/g °C; propylene glycol = 2.50 J/g °C
ween Substances: Thermal Equilibrium and Temperature Changes Submit for Grading Tutored Practice Problem 5.3.3 cSOAR A Predict thermal equilibrium temperatures. Close Proh A 10.89-g block of solid chromium at 12.99 °C is immersed in a 21.65-g pool of liquid propylene glycol with a temperature of 6642 °C. When thermal equilibrium is reached, what is the temperature of the chromium and propylene glycol? Specific heat capacities: chromium-0.448 J/g oC; propylene glycol = 2.50 JgC oC Check & Submt Answer Show Approach...
A piece of solid lead weighing 34.2 g at a temperature of 315 °C is placed in 342 g of liquid lead at a temperature of 376 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for...
A piece of solid cadmium weighing 37.6 g at a temperature of 311 °C is placed in 376 g of liquid cadmium at a temperature of 370 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid cadmium is ΔHfus = 6.11 kJ/mol at its melting point of 321 °C, and the molar heat capacities for...
A piece of solid lead weighing 32.6 g at a temperature of 311 °C is placed in 326 g of liquid lead at a temperature of 367 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for...
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g · K and 0.385 J/g · K, respectively.) Final temperature = How much energy is required to raise the temperature of 14.7 grams of gaseous hydrogen from 24.7 °C to 37.7 °C ? Answer: Joules.
A copper block with a mass of 600 grams is cooled to 77K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg °C), and of copper is 385 J/(kg °C). The latent heat of fusion of water is 3.35...
What amount of thermal energy (in kJ) is required to convert 44.1 g of ethanol at -178 °C completely to gaseous ethanol at 119 °C? The melting point of ethanol is -114 °C and its normal boiling point is 78 °C. The heat of fusion of ethanol is 5.0 kJ mol-1 The heat of vaporization of ethanol at its normal boiling point is 35.0 kJ mol-1 The specific heat capacity of solid ethanol is 1.05 J g-1 °C-1 The specific...
What amount of thermal energy (in kJ) is required to convert 42.0 g of ethanol at -171 °C completely to gaseous ethanol at 99 °C? The melting point of ethanol is -114 °C and its normal boiling point is 78 °C. The heat of fusion of ethanol is 5.0 kJ mol-1 The heat of vaporization of ethanol at its normal boiling point is 35.0 kJ mol-1 The specific heat capacity of solid ethanol is 1.05 J g-1 °C-1 The specific...