1. If equal masses of aluminum and copper are heated with same amount of heat, which...
Equal masses of aluminum and copper are heated to 100°C and placed in water. Which would cause the water to reach the higher temperature? Explain.
14. Answer this question: suppose equal masses of hot copper and hot aluminum are added to equal amounts of water. The initial temperatures of the metals are the same and the water samples also start with the same temperature. If the systems are isolated, which system, the one with copper or the one with aluminum, will end up with the higher equilibrium temperature and why?
If the same amount of heat is supplied to sample of 10.0g each aluminum, iron,and copper all at 15 degrees celsius which sample would reach the highest temperature????
1a. Identify which will be hotter (have a higher final temperature) if you heat equal masses of water and aluminum, each starting at room temperature with 1.0 kJ of electrical energy. Explain your groups answer. 1b. You are holding an Al rod in one hand and an Fe rod in another. The rods have the same mass and temperature (273 K). Assuming the rate of heat transfer is the same for both, identify which one will come to your body...
If a copper and aluminum (with different heat capacity) were both heated to 200C and then dropped into a separate but same water bath(35C), after the temperature stabilizes, what would the temperature in the water baths be like? Would they both have the same temperature or would one of the water baths be warmer than the other? and why?
Which material would cause a more severe burn if equal masses of two distinct metals are heated to a temperature of 100 °C: the one with the higher specific heat capacity or the one with the lower specific heat capacity? Explain your answer using the definition of specific heat.
A 1.6 kg block of iron at 35 ∘C is rapidly heated by a torch such that 14 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (14 kJ ) was quickly transferred to a 890 g pellet of copper at 34 ∘C, what temperature would the copper reach before it begins losing heat to the surroundings?
A pan made of which substance would require the largest amount of heat for equal cooking? Aluminum ( c = 0.22 cal/gCo) Gold ( c = 0.03 cal/gCo) Tin ( c = 0.054 cal/gCo) Copper ( c = 0.093 cal/gCo) Silver ( c = 0.056 cal/gCo)
Metal Cu Ag Mass (g) 15 15 Specific heat (J/g·°C) 0.385 0.240 Density (g/cm3) 8.96 1.049 Both of these metals are heated with the same amount of heat energy for 10 minutes. Which sample will reach the higher temperature and why? Copper because it is less dense Silver becaue it is more dense Silver because it has a lower specific heat Copper because it has a higher specific heat
Our 1 kg samples of aluminum, copper, and iron are all at 100° C and we place each in a separate beaker holding the same amount of water at 20° C. Which beaker of water will have the largest change in temperature? Why? Specific heat of each metal: aluminum: 921.096 J/kg*K copper: 376.812 J/kg*K iron: 460.548 J/kg*K