2. Why does the temperature of a mixture of ice and water remain constant during melting and freezing?

Why is water covalent if there is hydrogen bonding which is non-covalent?

how many joules of heat are required to heat 25.0 g of ethyl alcohol from the prevailing room temperature, 22.5 oC , to its boiling point, 78.5oC?

How much water at its boiling point can be vaporized by adding 1.50kJ of heat?

Why does water resist changes in temperature?

If it requires 70.4 kJ of heat to boil 1.60 moles of water, what is its enthalpy of vaporization?

Niobium is a transition metal used for making airplane propellers stronger as well as making eyeglasses thinner.  As a metal, it has a heat of fusion of 26.8 kJ/mol. Calculate the heat required to completely melt 25.4 g of niobium metal at its melting point.  Use 92.91 g/mol as the molar mass of niobium.

An ice cube at 0.00 °C with a mass of 8.64g is placed into 85.0g of water at 45°C. If no heat is lost to the surroundings, what is the final temperature of the water sample after all the ice is melted. (The specific heat of water is 4.184J/g°C, the ∆Hfus = 6.02kJ/mol)

2.The amount of energy involved in melting a substance without changing its temperature is called the A) heat of vaporization. B) calorie. C) joule. D) heat of fusion. E) heat of combustion.

Calculate the final temperature of a mixture of 130.0  g of ice initially at -15.50 °C and 337.0  g of water initially at 80.50 °C.