The optimum drinking temperature for a Shiraz is 15.0 ∘C . A certain bottle of Shiraz...
The optimum drinking temperature for a Shiraz is 15.0 ∘C . A certain bottle of Shiraz having a heat capacity of 3.40 kJ∘C−1 is 23.1 ∘C at room temperature. The heat of fusion of ice is 6.02 kJmol−1 and the heat capacity of ice is 2.108 Jg−1∘C−1. Assume that no heat is lost to the rest of the surroundings.What minimum mass of ice, originally at -3.0 ∘C , is required to bring the final temperature to 15.0 ∘C? Express your answer with the appropriate units.
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The optimum drinking temperature for a Shiraz is 15.0 ∘C . A
certain bottle of Shiraz...
The optimum drinking temperature for a Shiraz is 15.0 ∘C . A certain bottle of Shiraz...
The optimum drinking temperature for a Shiraz is 15.0 ∘C . A certain bottle of Shiraz having a heat capacity of 3.40 kJ∘C−1 is 23.1 ∘C at room temperature. The heat of fusion of ice is 6.02 kJmol−1 and the heat capacity of ice is 2.108 Jg−1∘C−1. Assume that no heat is lost to the rest of the surroundings. What minimum mass of ice, originally at -4.0 ∘C , is required to bring the final temperature to 15.0 ∘C?
What volume of methane at STP would be required to convert a 2.5 kg block of...
What volume of methane at STP would be required to convert a 2.5 kg block of ice at −13 ∘C to water at 13 ∘C, assuming that no heat is lost? The heat of fusion for ice is 6.01 kJmol−1 . The heat capacity of ice is 2.108 Jg−1∘C−1, the specific heat capacity of water is 4.184 Jg−1∘C−1 and the heat of combustion for methane is 891 kJmol−1.
What is the final temperature when 8 kg of ice at -5° C is mixed with...
What is the final temperature when 8 kg of ice at -5° C is mixed with 2 kg of steam at 126.8° C. The heat capacity of the steam is 1.901 kJ/Kg C and the heat capacity of ice is 2.108 kJ/kgC
How much heat energy is required to convert 15.0 g of solid ethanol at -114.5 °C...
How much heat energy is required to convert 15.0 g of solid
ethanol at -114.5 °C to gasesous ethanol at 143.1 °C? The molar
heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of
vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of
-114.5 °C and a normal boiling point of 78.4 °C. The specific heat
capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous
ethanol is 1.43 J/g·°C.
How much heat energy...
9. Four ice cubes exactly at-50 °C with a total mass of 53.5 g are combined with 1 15 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final tempe...
9. Four ice cubes exactly at-50 °C with a total mass of 53.5 g are combined with 1 15 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture? The heat capacity of ice is 2.03 JIg C and that of water is 4.18 JIg C. The heat of fusion of water is +6.01 kJ/mol. (1.5 pts)
9. Four ice cubes exactly at-50 °C...
What is the mass of ice (in g) at 0 °C that can be completely melted...
What is the mass of ice (in g) at 0 °C that can be completely melted into liquid water at 0°C by a 119 g aluminum block at temperature 112 °C? Assume the aluminum block can melt the ice until its temperature drops to 0 °C. The heat capacity of aluminum is 0.903 J g-1 °C-1 and the heat of fusion of water is 6.02 kJ mol-1. Express your answer to 3 significant figures.
A 18.7-g sample of ice at -13.1°C is mixed with 118.5 g of water at 80.0°C. Calculate the final temperature of the mixtu...
A 18.7-g sample of ice at -13.1°C is mixed with 118.5 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.03 and 4.18 J/g∙°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.
An ice cube of mass 8.5 g at temperature 0∘C is added to a cup of...
An ice cube of mass 8.5 g at temperature 0∘C is added to a cup of coffee, whose temperature is 90 ∘C and which contains 130 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0 kJ/mol. Find the temperature of the coffee after the ice melts.(in C)
An ice cube of mass 9.0g is added to a cup of coffee, whose temperature is 90.0 °C and which contains 120.0 g of li...
An ice cube of mass 9.0g is added to a cup of coffee, whose temperature is 90.0 °C and which contains 120.0 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0kJ/mol. Find the temperature of the coffee after the ice melts. Use the equation given in the lab manual on page 86. Ignore the + (CC) (AT)...
The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at...
The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at 0 °C is added to it. The desired final temperature of the water is 11 °C. The latent heat of fusion for water is 33.5 × 104 J/kg, and the specific heat capacity of water is 4186 J/(kg·C°). Ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added.
How much heat energy is required to convert 15.0 g of solid
ethanol at -114.5 °C to gasesous ethanol at 143.1 °C? The molar
heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of
vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of
-114.5 °C and a normal boiling point of 78.4 °C. The specific heat
capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous
ethanol is 1.43 J/g·°C.
How much heat energy...
9. Four ice cubes exactly at-50 °C with a total mass of 53.5 g are combined with 1 15 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture? The heat capacity of ice is 2.03 JIg C and that of water is 4.18 JIg C. The heat of fusion of water is +6.01 kJ/mol. (1.5 pts)
9. Four ice cubes exactly at-50 °C...
An ice cube of mass 9.0g is added to a cup of coffee, whose temperature is 90.0 °C and which contains 120.0 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0kJ/mol. Find the temperature of the coffee after the ice melts. Use the equation given in the lab manual on page 86. Ignore the + (CC) (AT)...
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