Question

Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

heat capacity of H_{2}O(s) |
37.7 J/(mol*k) |

heat capacity of H_{2}O(l) |
75.3 J/(mol*k) |

enthalpy of fusion of H_{2}O |
6.01 kJ/mol |

Answer #1

Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water
after all the ice melts.
Heat capactiy of H2o (s) = 37.7 J/(mol x K)
Heat capactiy of H2o (l) = 75.3
enthapy infusion of H20= 6.01 kj/mol

Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water
after all the ice melts. heat capacity of H2O(s) is 37.7 J/mol*K
heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20
is 6.01 kJ/mol

Two 20.0-g ice cubes at –18.0 °C are placed into 245 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts. Please show work.
Heat capacity of H20(s): 37.7 J/(mol x K)
Heat capacity of H20(l): 75.3 J/(mol x K)
Enthalpy of fusion of H20: 6.01 kJ/mol

Two 20.0-g ice cubes at –20.0 °C are placed into 275 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –19.0 °C are placed into 275 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –20.0 °C are placed into 255 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –20.0 °C are placed into 265 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –16.0 °C are placed into 295 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –15.0 °C are placed into 225 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –15.0 °C are placed into 285 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 6 minutes ago

asked 12 minutes ago

asked 19 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 3 hours ago

asked 3 hours ago