ΔH of vapor cooler to 155 oC to 100 oC = 1.84 J/g oC x 5g x(100 -155) = -506 J
ΔH of Condensation = -2260 J/g x 5g = -11300 J
ΔH of water cooled 100 oC to oC = 4.18 J/g oC x 5g x (0-100) = -2090 J
ΔH of fusion = -336 J/g x 5g = -1680J
ΔH of ice cooled 0 oC to -55 oC = 2.09 J/g oC x 5g x (-55 -0) = -574.75J
Sum of ΔH = (-506 J) + (-11300 J) + (-2090 J) + (-1680 J) + (-574.75 J) = -16150.75 J = -16.1 kJ
155 gas a5 points) A 5.00 g sample of water Vapor, initially at 155°C is cooled...
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
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What is the final temperature when a 10.0 g sample of water is heated with an input of 20.0 kJ starting at 10.0°C? You might need the following information for water: specific heat H2O(s): 2.09 J/g°C specific heat H2O(l): 4.18 J/g°C specific heat H2O(g): 1.84 J/g°C heat of fusion: 6.09 kJ/mole heat of vaporization: 40.7 kJ/mole Answer choices are: 488°C 273°C 89.0°C 100.°C It said 488 was wrong.
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Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
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