A hot piece of aluminum weighing 50.0 grams at 350°C is dropped into 500. grams of...
A hot piece of aluminum weighing 50.0 grams at 350°C is dropped into 500. grams of water at 22.0°C. What is the final temperature of the water? The specific heat of aluminum is 0.902 J/g°C and that of water is 4.184 J/g°C.
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A hot piece of aluminum weighing 50.0 grams at 350°C is dropped
into 500. grams of...
A piece of titanium at 100.0°C was dropped into 50.0 g of water at 20.0°C. The...
A piece of titanium at 100.0°C was dropped into 50.0 g of water at 20.0°C. The final temperature of the system was 22.6°C. What was the mass of the titanium? Specific heat (J/g°C) titanium 0.54 water 4.184
7. A piece of metal weighing 90.3 grams and at an initial temperature of 99.0°C was...
7. A piece of metal weighing 90.3 grams and at an initial temperature of 99.0°C was dropped into a beaker containing 78.2 g of water whose initial temperature is 21.0°C. The final temperature of the metal and water was 29.0°C. Calculate the specific heat of metal. (Specific heat of water = 4.184 J/g.K) A. 0.372 B. 0.123 C. 0.886 D. 0.534 E. 0.414
please help me. Thanks A piece of copper metal weighing 36.3 g is initially at 100.0...
please help me. Thanks
A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
A chunk of aluminum weighing 18.5 grams and originally at 98.80 °C is dropped into an...
A chunk of aluminum weighing 18.5 grams and originally at 98.80 °C is dropped into an insulated cup containing 75.7 grams of water at 23.67 °C. Assuming that all of the heat is transferred to the water, the final temperature of the water is ___ °C.
A chunk of aluminum weighing 19.1 grams and originally at 98.95°C is dropped into an insulated...
A chunk of aluminum weighing 19.1 grams and originally at 98.95°C is dropped into an insulated cup containing 80.7 grams of water at 20.69°C. Assuming that all of the heat is transferred to the water, the final temperature of the water is °C.
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264...
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264 °C. The initial temperature of aluminum is 98.4°C. Calculate the final temperature of both water and aluminurn? (Specific heat of water and aluminum is from #1) 7) Calculate Enthalpy of the following reaction (Hz) from standard enthalpies of formation (H) from the table below. (a) C2H5OH(L) + 3 029) - 2 CO2(g) + 3 H2O(1) (b) 3 N0369) + H20(1) - 2 HNO3(aq) +...
A 50.0 g piece of hot iron is placed in 165 g of water with an...
A 50.0 g piece of hot iron is placed in 165 g of water with an initial temperature of 22.8°C. The temperature of the combination rises to 25.7°C. What was the initial temperature of the iron? The specific heat of iron is 0.449 J/gK and the specific heat of water is 4.18 J/gK.
Determine the final temperature (in K) if a 10.0 g piece of hot iron, at 77⁰C,...
Determine the final temperature (in K) if a 10.0 g piece of hot iron, at 77⁰C, is placed in 50.0 g of cold water at 20⁰C. (Specific heat capacity of iron is 0.45Jg·K and that of water is 4.184 Jg·K )
A hot lump of 35.9 g of aluminum at an initial temperature of 63.3 °C is...
A hot lump of 35.9 g of aluminum at an initial temperature of 63.3 °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 aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 42.0 g of aluminum at an initial temperature of 90.5 °C is...
A hot lump of 42.0 g of aluminum at an initial temperature of 90.5 °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 aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
A piece of titanium at 100.0°C was dropped into 50.0 g of water at 20.0°C. The final temperature of the system was 22.6°C. What was the mass of the titanium? Specific heat (J/g°C) titanium 0.54 water 4.184
7. A piece of metal weighing 90.3 grams and at an initial temperature of 99.0°C was dropped into a beaker containing 78.2 g of water whose initial temperature is 21.0°C. The final temperature of the metal and water was 29.0°C. Calculate the specific heat of metal. (Specific heat of water = 4.184 J/g.K) A. 0.372 B. 0.123 C. 0.886 D. 0.534 E. 0.414
please help me. Thanks
A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264 °C. The initial temperature of aluminum is 98.4°C. Calculate the final temperature of both water and aluminurn? (Specific heat of water and aluminum is from #1) 7) Calculate Enthalpy of the following reaction (Hz) from standard enthalpies of formation (H) from the table below. (a) C2H5OH(L) + 3 029) - 2 CO2(g) + 3 H2O(1) (b) 3 N0369) + H20(1) - 2 HNO3(aq) +...
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