Question 14 5 pts A copper cube with a mass of 25.0 g is initially at...
NEED ANSWERS ASAP QUESTION 5 A 5.00-9 sample of copper metal at 25.0 °C was heated by the addition of 133 J of energy. What is the final temperature of the copper? The specific heat of copper is 0.38 J/g °C Use this equation q = m C AT or AT = q/ mc AT = Tf - Ti O 15.1 °C. 0 62.0 °C. 0 39.0 °C. 0 95.0 °C. 0 80.0 °C. QUESTION 4 What are units of...
4. A hot lump of 44.5 g of copper at an initial temperature of 60.7°C is placed in 50.0 mL H20 initially at 25.0°C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385J/gºC and the specific heat of water is 4.184 J/gºC? a. 23.7°C c. 27.7°C b. 25.7°C d. 29.7°C
A 32.5 g cube of aluminum initially at 45.8 oC is submerged into 105.3 g of water at 15.4 oC. What is the final temperature of both substances at thermal equilibrium? The specific heat of Al is 0.903 J/g • oC. The specific heat of water is 4.184 J/g • oC. (Hint: your answer should not contain any units and have three significant figures)
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0°C. The specific heat of water is 4.18 J/gºC. Show your work Final Answer 4. Aluminum metal has a specific heat of 0.901 J/g C. How much heat is transferred to a 6.75 g piece of aluminum initially at room temperature, 20.0°C, when it is placed into boiling water? The temperature of boiling water is 100°C. Show your work Final Answer 5....
Question 4 of 15 Page 4 of 15 Question 4 (6 points) A piece of copper alloy with a mass of 84.0 g is heated from 30.0°C to 47.0°C. In the process, it absorbs 464 of energy as heat. The specific heat of this copper alloy is J/gºC? (Answer to 3 sig figs) Blank 1:
QUESTION 5 A metal cube loses 3.358 kJ of heat. (.e., q = -3.358 kJ) The metal has mass of 135.6 grams. The initial temperature of the metal before the heat loss is is 158 °C, the final temperature (after heat loss) is 35.0 °C. What is the specific heat, c, of the metal in units of J/g °C? (watch units! Units must match!) 1.93 J/gºc 3.25 J/gºC 2.51 J/gºc 0.986 J/gºC 0.529 J/9°C 0.201 J/gºC 0.408/9°C
A hot lump of 35.6 g of copper at an initial temperature of 86.3 C is placed in 50.0 mL initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(gxC). Assume no heat is lost to surroundings.
A 20-g ice cube floats in 210 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 92°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C,...
A 38-g ice cube floats in 190 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 96°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C,...
Question 10 of 20 A 141.9 g piece of copper (specific heat 0.38 J/g.°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature of the copper? (The specific heat of water is 4.18 J/g °C).