8) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C?A) 0.56 calB) 80. calC) 3.6 calD) 1.8 cal81Insimalolgmootesd irmoils ononimuisE) 3.6 x 103 calos6.0 (8

The heat of fusion for water is 80 cal/g. It is required to calculate the calories needed to melt 45…

Answered: 8) If the heat of fusion for water is…

Living By Chemistry: First Edition Textbook

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ChapterU5: Fire: Energy , Thermodynamics, And Oxidation-reduction

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A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).
A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.
he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?
Will a closed container of water at 70 C or an open container of water at the same temperature cool faster on a cold winter day? Explain why.
Calculate the quantity of heating required to convert the water in four ice cubes (60.1 g each) from H2O(s) at 0 °C to H2O(g) at 100. °C. The enthalpy of fusion of ice is 333 J/g and the enthalpy of vaporization of liquid water is 2260 J/g.
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
Carbon disulfide, CS2 is a volatile, flammable liquid. It has a vapor pressure of 400.0 mmHg at 28.0C and 760.0 mmHg at 46.5C. What is the heat of vaporization of this substance?
Consider a substance X with a Hvap = 20.3 kJ/mol and Hfus = 9.0 kJ/mol. The melting point, freezing point, and heat capacities of both the solid and liquid X are identical to those of water. a If you place one beaker containing 50 g of X at 10C and another beaker with 50 g of H2O at 10C on a hot plate and start heating them, which material will reach the boiling point first? b Which of the materials from part a, X or H2O, would completely boil away first? c On a piece of graph paper, draw the heating curve for H2O and X. How do the heating curves reflect your answers from parts a and b?
Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
Explain why 15 g of steam at 100C melts more ice than 15 g of liquid water at 100C.

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8) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C? A) 0.56 cal B) 80. cal C) 3.6 cal D) 1.8 cal 81 Insimal olgmootesd ir moils ono nimuis E) 3.6 x 103 cal os6.0 (8