suppose that 0.95g of water condenses on a 75.0g block of iron that is initially at...
suppose that 0.95g of water condenses on a 75.0g block of iron that is initially at 22 degree Celsius.if the heat released goes in to only warming the iron block.what is the final temperature of the iron block in degree Celsius.(assume the heat of enthalpy of vaporization for water of 44.0 kj/mol.
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suppose that 0.95g of water condenses on a 75.0g block of iron
that is initially at...
Suppose that 0.94 g of water condenses on a 85.0 g block of iron that is...
Suppose that 0.94 g of water condenses on a 85.0 g block of iron that is initially at 21 degrees Celsius. If the heat released during condensation goes only to warming the iron block, what is the final temperature,(in Celsius) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)
Suppose that 0.92 g of water condenses on a 85.0 g block of iron that is...
Suppose that 0.92 g of water condenses on a 85.0 g block of iron that is initially at 24 ∘C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in ∘C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)
Suppose that 0.95 gg of water condenses on a 85.0 gg block of iron that is...
Suppose that 0.95 gg of water condenses on a 85.0 gg block of iron that is initially at 21 ∘C∘C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in ∘C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol and a heat capacity for iron of 0.449 J⋅g−1⋅∘C−1.)
Part B Suppose that 0.48 g of water at 25° C condenses on the surface of...
Part B Suppose that 0.48 g of water at 25° C condenses on the surface of a 55-g block of aluminum that is initially at 25°C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in degrees Celsius) of the metal block? (The specific heat capacity of aluminum, Cs,A1, is 0.903 J/(g. °C).) Express your answer in degrees Celsius to two significant figures. IVO ΑΣφ ? T = 22 C Submit Previous...
Calculate the amount of heat (in kilojoules) required to vaporize 2.58 kg of water at its...
Calculate the amount of heat (in kilojoules) required to vaporize 2.58 kg of water at its boiling point. Express the heat in kilojoules to three sianificant fiaures. Suppose that 0.48 g of water at 25°C condenses on the surface of a 55-g block of aluminum that is initially at 25 °C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in degrees Celsius) of the metal block? (The specific heat capacity aluminum,...
Suppose that 1.13 g of rubbing alcohol (C3H8O) evaporates from a 66.0 g aluminum block.
Suppose that 1.13 g of rubbing alcohol (C3H8O) evaporates from a 66.0 g aluminum block.Part AIf the aluminum block is initially at 25℃, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization of the alcohol comes only from the aluminum block and that the alcohol vaporizes at 25℃. The heat of vaporization of the alcohol at 25℃ is 45.4 kJ / mol, the specific heat of aluminum...
Suppose that 1.02 g of rubbing alcohol (C3H8O) evaporates from a 55.0-g aluminum block. If the...
Suppose that 1.02 g of rubbing alcohol (C3H8O) evaporates from a 55.0-g aluminum block. If the aluminum block is initially at 25 degree C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization ofthe alcohol K comes only from the aluminum block and that the alcohol vaporizes at 25 degree C.
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped...
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped into a large lake at 15°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and the lake water. Determine the total entropy change for this process. The specific heat of Iron at room temperature is cp0.45 kJ/kg.K. The specific heat of copper at 27°C is ep 0,386 kJ/kg.K. Iron Lake 15°C Copper The total entropy change...
A coffee cup calorimeter initially contains 135g of water at 22.0oC. Calcium chloride (21.0g) at the...
A coffee cup calorimeter initially contains 135g of water at 22.0oC. Calcium chloride (21.0g) at the same temperature is added to the water and after the CaCl2 dissolves the final temperature 46.0 degrees C. Calculate the molar enthalpy change for dissolving the salt in KJ/mol. Assume the solution has a heat capacity of 4.184 J/C g and assume no heat is lost to the surrounding or the calorimeter.
An aluminum block weighing 32 kg initially at 140°C is brought into contact with a block...
An aluminum block weighing 32 kg initially at 140°C is brought into contact with a block of iron weighing 44 kg at 60°C in an insulated enclosure. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of aluminum at 400 K is Cp0.949 kJ/kg.K. The specific heat of iron at room temperature is Cp=0.45 kJ/kg.K. The final equilibrium temperature is 108,35 K. The total entropy change for this process is 397 kJ/K
Part B Suppose that 0.48 g of water at 25° C condenses on the surface of a 55-g block of aluminum that is initially at 25°C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in degrees Celsius) of the metal block? (The specific heat capacity of aluminum, Cs,A1, is 0.903 J/(g. °C).) Express your answer in degrees Celsius to two significant figures. IVO ΑΣφ ? T = 22 C Submit Previous...
Calculate the amount of heat (in kilojoules) required to vaporize 2.58 kg of water at its boiling point. Express the heat in kilojoules to three sianificant fiaures. Suppose that 0.48 g of water at 25°C condenses on the surface of a 55-g block of aluminum that is initially at 25 °C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in degrees Celsius) of the metal block? (The specific heat capacity aluminum,...
Suppose that 1.02 g of rubbing alcohol (C3H8O) evaporates from a 55.0-g aluminum block. If the aluminum block is initially at 25 degree C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization ofthe alcohol K comes only from the aluminum block and that the alcohol vaporizes at 25 degree C.
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped into a large lake at 15°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and the lake water. Determine the total entropy change for this process. The specific heat of Iron at room temperature is cp0.45 kJ/kg.K. The specific heat of copper at 27°C is ep 0,386 kJ/kg.K. Iron Lake 15°C Copper The total entropy change...
An aluminum block weighing 32 kg initially at 140°C is brought into contact with a block of iron weighing 44 kg at 60°C in an insulated enclosure. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of aluminum at 400 K is Cp0.949 kJ/kg.K. The specific heat of iron at room temperature is Cp=0.45 kJ/kg.K. The final equilibrium temperature is 108,35 K. The total entropy change for this process is 397 kJ/K
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