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1. Consider the following specific heats
SHH2O(s) = 2.09 J/g ·
◦ C,
SHH2O(ℓ) = 4.18 J/g ·
◦ C, and
SHH2O(g) = 2.03 J/g ·
◦ C.
The heat of fusion for water is 334 J/g and
the heat of vaporization for water is 2260 J/g.
Calculate the amount of heat required to
convert 65 g of ice at −35◦C completely to
steam at 131◦C. Answer in units of kJ.
2. The specific heat of solid silver is 0.237 J/g·
◦C
and the heat of fusion of silver at its melting
point of 961 ◦C is 11 J/g. Find the final
temperature if 1020 J is used to heat 27 g of
silver initially at 20◦C. Answer in units of◦C.
SHH2O(s) = 2.09 J/g ·
◦ C,
SHH2O(ℓ) = 4.18 J/g ·
◦ C, and
SHH2O(g) = 2.03 J/g ·
◦ C.
The heat of fusion for water is 334 J/g and
the heat of vaporization for water is 2260 J/g.
Calculate the amount of heat required to
convert 65 g of ice at −35◦C completely to
steam at 131◦C. Answer in units of kJ.
2. The specific heat of solid silver is 0.237 J/g·
◦C
and the heat of fusion of silver at its melting
point of 961 ◦C is 11 J/g. Find the final
temperature if 1020 J is used to heat 27 g of
silver initially at 20◦C. Answer in units of◦C.