A 12.5 g sample of granite initially at 82.0oC is immersed into a 25.0 g of...
A 12.5 g sample of granite initially at 82.0oC is immersed into a 25.0 g of water initially at 22.0oC. What is the final temperature of both substances when they reach thermal equilibrium? (For water, c = 4.184 J/g.oC, and for granite, c = 0.790 J/g.oC.)
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A 12.5 g sample of granite initially at 82.0oC is
immersed into a 25.0 g of...
Part A A 11.5-g sample of granite initially at 83.0 °C is immersed into 29.0 g...
Part A A 11.5-g sample of granite initially at 83.0 °C is immersed into 29.0 g of water initially at 24.0 °C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, Cs = 4.18 J/g °C and for granite, Cs = 0.790 J/g °C.) O 3.66 x 103 °C O 19.2°C 53.5 °C 28.1°C
Part A A 12.0 x sample of granite initially at 83.0 is immersed into 250 g...
Part A A 12.0 x sample of granite initially at 83.0 is immersed into 250 g of water initially at 25.0°C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, C. = 4.18J/g and for granite, C, = 0.790J/gºC.) Express your answer using three significant figures. AED + O ? 19.21 Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining
1. A 31.6 g wafer of pure gold initially at 69.4 ∘C is submerged into 63.8...
1. A 31.6 g wafer of pure gold initially at 69.4 ∘C is submerged into 63.8 g of water at 27.7 ∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium? 2.Two substances, A and B, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of substance A is 6.04 gand its initial temperature is 21.0 ∘C . The mass of substance B is 25.5 gand its initial temperature is...
A hot 105.8 g lump of an unknown substance initially at 179.7 °C is placed in 35.0 mL of water initially at 25.0 °C and...
A hot 105.8 g lump of an unknown substance initially at 179.7 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 77.4 °C. Substance Specific heat (J/(g·°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184 Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no...
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10...
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00...
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
A 32.5 g cube of aluminum initially at 45.8 oC is submerged into 105.3 g of...
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)
A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed...
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL H2O 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/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°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...
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 hot lump of 32.3g of Copper at an initial temperature of 96.5 degrees Celsius in...
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
Part A A 11.5-g sample of granite initially at 83.0 °C is immersed into 29.0 g of water initially at 24.0 °C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, Cs = 4.18 J/g °C and for granite, Cs = 0.790 J/g °C.) O 3.66 x 103 °C O 19.2°C 53.5 °C 28.1°C
Part A A 12.0 x sample of granite initially at 83.0 is immersed into 250 g of water initially at 25.0°C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, C. = 4.18J/g and for granite, C, = 0.790J/gºC.) Express your answer using three significant figures. AED + O ? 19.21 Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL H2O 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/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
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