A 25.Og block of gold (Cs = 0.129 J/g.°C) is heated to 155 °C and then placed on top of a 100.0g block of silver (Cs = 0.240 J/g.°C) at 25°C. Assuming that heat is only transferred between the metals (no heat lost to the surroundings) what is the final temperature of the metal blocks after they reach equilibrium?
3. A 60.0 g block of iron that has an initial temperature of 250. "C and 60.0 g block of gold that has an initial temperature of 45.0°C are brought into contact with one another. Assuming no heat is lost to the surroundings, what will be the temperature when the two metals reach thermal equilibrium? The specific heat capacity of iron +0.449 J/g C and gold -0.128 J/g °C.
Two 20.0 g ice cubes at −18.0 ∘C are placed into 275 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, ?f, of the water after all the ice melts.
A 275-g sample of nickel at 100.0°C is placed in 100.0 g of water at 22.0°C. What is the final temperature of the water? Assume no heat transfer with the surroundings. The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C. Hint: The final temp for both the system and surroundings will be the same.
Two 20.0-g ice cubes at –10.0 °C are placed into 255 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of water s = 37.7 heat capacity of water q =75.3 fusion = 6.01
Assume that you have 10.0 g of each of the following substances. To which substance would you have to add the smallest amount of energy to change the temperature by the same amount? a. Copper (specific heat capacity = 0.387 J/g°C) b. Lead (specific heat capacity = 0.128 J/g°C) c. Gold (specific heat capacity = 0.129 J/g°C) d. Iron (specific heat capacity = 0.4998 J/g°C) e. Silver (specific heat capacity = 0.235 J/g°C)
A calorimeter contained 79.0 g of water at 15.75°C. A 120.-g sample of iron at 63.82°C was placed in it, giving a final temperature of 19.06°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184 J/g·°C for and 0.444 J/g·°C for . Heat capacity of the calorimeter = ________J/°C
Question 9 of15 The temperature of an object increases by 41.6 °C when it absorbs 3641 J of heat. Calculate the heat capacity of the object. The mass of the object is 365 g. Use the table of specific heat values to identify the composition of the object Substance Specific heat (J/(g . ! gold silver iron aluminum 0.129 0.240 0.444 0.900
The object is composed of _________? The temperature of an object increases by 60.1 °C when it absorbs 3657 J of heat. Calculate the heat capacity of the object. C= J/°C The mass of the object is 385 g. Use the table of specific heat values to identify the composition of the object. Substance Specific heat (J/(g. °C)) 0.129 gold lead 0.158 iron 0.444 0.900 aluminum
(b) If 3.0% of the heat being measured was being lost to the universe, determine whether they could they distinguish between iron (s = 0.444 J/g · °C) and Ni (s = 0.449 J/g · °C). What is the percent difference between the specific heats of the two metals? Use the specific heat of iron as the theoretical value. % (b) Is this difference large enough to differentiate between the metals? Yes No This cannot be determined with the information...