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Question 10 2 pts If 15.5 J of heat are removed from 14.6 g of mercury...
A chunk of mercury at 80.8°C was added to 200.0 g of water at 15.5°C. The specific heat of mercury is 0.14 J/gºC, and the specific heat of water is 4.184 J/gºC. When the temperature stabilized, the temperature of the mixture was 20.9°C. Assuming no heat was lost to the surroundings, what was the mass of mercury added? a) 399 g b) 4948 539 g d) 2.08 kg e) 682 g
Question 13 4 pts 734 J of thermal energy is added to a 155 g sample of lead that is initially at 25.0 °C. What will be the final temperature (in °C) if the specific heat capacity of lead is 0.130 J/g °C?
100 J of heat was removed from 50 g of an iron bar at 20 oC. What is the final temperature after the iron bar lost the heat? (The specific heat of iron is 0.5 J/goC.)
If 100. J of heat energy is applied to a 25 g sample of mercury, by how many degrees with the temperature of the sample of mercury increase? (Specific heat of mercury is 0.14 J/goC)
A 143-g sample of mercury is at an initial temperature of 25 °C. If 1067 joules of heat are applied to the sample, what is the final temperature of the mercury? The specific heat capacity of mercury is 0.14 J/(g∙ °C).
A Review | Constar 100 J of heat energy are transferred to 30 g of mercury. By how much does the temperature of mercury increase? The specific heat of mercury is 140 "kek Express your answer in degrees Celsius. AT = 24 °C Submit Previous Answers All attempts used; correct answer displayed Part B How much heat is needed to raise the temperature of 30 g of water by the same amount? The specific heat of water is 4190 Express...
18) 10 J of heat are removed from a gas sample while it is being compressed by a piston that does 30 J of work. Determine, in J, the change in thermal energy of the system. a) 4 b) 10 c) 20 d) 3 Answer_______________ 19) It is possible for a device to transform a given amount of heat completely into work. a) true b) false Answer_______________ 20) The density of a block of iron is 7,860 kg/m3. The density...
How much heat must be removed from 456 g of water at 25.0 degree C to change it into ice at -10.0 degree C? The specific heat of ice is 2090 J/kg K. the latent heat of fusion of water is 33.5 times 10^4 J/Kg, and the specific heat of water is 4186 J/kg K.
Question 10 1 pts The specific heat capacity of lead is 0.13 J/g °C. How much heat (in J) is required to raise the temperature of 16.9 g of lead from 27.3°C to 35.7°C? Keep three significant figures in your answer.
2. (10 pts) If 56.0 k) of heat is added to a 41.0-g sample of liquid temperature of -170 °C, what is the final state final temperature once the system equilibrates? 108 sample of liquid methane under 1 atm of pressure at a methane once the system equilibrates? What is the Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5.C. AHvap = 8.20 * The specific heats of liquid and gaseous methane are...