A very hot cube of copper metal (32.5 g) is submerged into 105.3 g of water...
A very hot cube of copper metal (32.5 g) is submerged into 105.3 g of water at 15.4 0C and it reach a thermal equilibrium of 17.3 0C. Calculate the initial temperature of copper (Cs = 0.385 J/g 0C for copper, and 4.18 J/g 0C for water)
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A very hot cube of copper metal (32.5 g) is submerged into 105.3
g of water...
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)
Review I Consta A copper cub0 measuring 1.55 cm on edge and an aluminum cube measuring...
Review I Consta A copper cub0 measuring 1.55 cm on edge and an aluminum cube measuring 1.66 cm on edge are both heated to 60.0 C and submerged in 100.0 ml of water at 21.6 C Part A What is the final temperature of the water when equilibrium is reached? (Assume a density of 0.998 g/mlL for water.) ΑΣφ T C Submit Request Answer Part A A block of copper of unknown mass has an initial temperature of 66.4 C....
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 27.4 g of copper at an initial temperature of 70.3 °C is...
A hot lump of 27.4 g of copper at an initial temperature of 70.3 °C is placed in 50.0 mL of 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 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 30.9 g of copper at an initial temperature of 97.4 °C is...
A hot lump of 30.9 g of copper at an initial temperature of 97.4 °C is placed in 50.0 mL of 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 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 30.7 g of copper at an initial temperature of 83.3 °C is...
A hot lump of 30.7 g of copper at an initial temperature of 83.3 °C is placed in 50.0 mL, H,O 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/(8°C)? Assume no heat is lost to surroundings. Tsinal
A hot lump of 45.1 g of copper at an initial temperature of 58.5 °C is...
A hot lump of 45.1 g of copper at an initial temperature of 58.5 °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 0.385 J/(g•°C)? Assume no heat is lost to surroundings. Tina $ 0.0455ı ned with -Cam Scanner
this is the answer but i dont get why they put (45.8-Tf) instead of (Tf-45.8). shouldnt...
this is the answer but i dont get
why they put (45.8-Tf) instead of (Tf-45.8). shouldnt the format be
(Tf-Ti)? like for the eqution on the other side of the = sign its
(Tf-15.4) and its in the format of (Tf-Ti). help
A 32.5 g cube of aluminum initially at 45.8 Celsius is submerged into 105.3g of water at 15.4 Celsius. What is the final temperture of both substances at thermal equilibrium Best Answer Sharlene J answered this lets tf...
A 35.0 gram cube of a metal initially at 56.2°C was submerged into 1.00 g of...
A 35.0 gram cube of a metal initially at 56.2°C was submerged
into 1.00 g of water at 14.2 degrees * C . The final temperature of
both substances at thermal equilibrium was 43.5 C. What is the heat
capacity in J/g C) of the metal?
A 35.0 gram cube of a metal initially at 56.2°C was submerged into 1.00 g of water at 14.2°C. The final temperature of both substances at thermal equilibrium was 43.5 °C. What is the...
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...
Review I Consta A copper cub0 measuring 1.55 cm on edge and an aluminum cube measuring 1.66 cm on edge are both heated to 60.0 C and submerged in 100.0 ml of water at 21.6 C Part A What is the final temperature of the water when equilibrium is reached? (Assume a density of 0.998 g/mlL for water.) ΑΣφ T C Submit Request Answer Part A A block of copper of unknown mass has an initial temperature of 66.4 C....
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 30.7 g of copper at an initial temperature of 83.3 °C is placed in 50.0 mL, H,O 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/(8°C)? Assume no heat is lost to surroundings. Tsinal
A hot lump of 45.1 g of copper at an initial temperature of 58.5 °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 0.385 J/(g•°C)? Assume no heat is lost to surroundings. Tina $ 0.0455ı ned with -Cam Scanner
this is the answer but i dont get
why they put (45.8-Tf) instead of (Tf-45.8). shouldnt the format be
(Tf-Ti)? like for the eqution on the other side of the = sign its
(Tf-15.4) and its in the format of (Tf-Ti). help
A 32.5 g cube of aluminum initially at 45.8 Celsius is submerged into 105.3g of water at 15.4 Celsius. What is the final temperture of both substances at thermal equilibrium Best Answer Sharlene J answered this lets tf...
A 35.0 gram cube of a metal initially at 56.2°C was submerged
into 1.00 g of water at 14.2 degrees * C . The final temperature of
both substances at thermal equilibrium was 43.5 C. What is the heat
capacity in J/g C) of the metal?
A 35.0 gram cube of a metal initially at 56.2°C was submerged into 1.00 g of water at 14.2°C. The final temperature of both substances at thermal equilibrium was 43.5 °C. What is the...
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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