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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Formula: C3H6O
Melting Point: -94.0°C
Boiling Point: 56.0°C
Density of liquid: 0.791 g/mL
Heat of Fusion: 98.14 J/g
Heat of vaporization: 538.9 J/g
Specific heat capacity (solid): 1.653 J/g°C
Specific heat capacity (liquid): 2.161 J/g°C
Specific heat capacity (gas): 1.291 J/g°C
How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?
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- Entrhaipy of lusion: Afus H 334 J g • Enthalpy of vaporization: Avap H° = 2250Jg -1 Part A How much heat energy, in kilojoules, is required to convert 32.0 g of ice at -18.0 °C to water at 25.0 ° C? Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) HA 12.6 kJ Submit Previous Answers X Incorrect; Try Again; 2 attempts remaining Part B How long would it take for 1.50 mol of water at 100.0 ° C to be converted completely into steam if heat were added at a constant rate of 19.0 J s ? Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) ? min 50.62 Submit Previous Answers X Incorrect; Try Again; 4 attempts remainingarrow_forward1) 80°F What does not correspond to the molar heat of fusion? O AHfus Mostly sunny F1 AH cond O the heat absorbed by one mole of a substance in melting from a solid to a liquid at a constant temperature O the enthalpy change when 1 mol of a substance melts F2 2 W F3 2+ #M 3 E F4 $ 4 F5 R И ur jo % F6 T ☆ O Search F7 6 Y F8 & 7 + U F9 * 00 8 F10 28 GO F11 O F12 P Prt Sc Insert Del Backspacearrow_forwardHow much heat is released when 105 g of steam at 100.0 C is cooled to ice at -15.0 C? The enthalpyof vaporization of water is 40.67 kj/mol, the enthalpy of fusion for water is 6.01 kj/mol, the specific heatcapacity of liquid water is 4.18 J/g C and the specific heat capacity of ice is 2.02 J/g C.(q heating = m x C x ΔT, q phase change = ΔH vap x n)arrow_forward
- A 41.30 g piece of solid acetone has a temperature of -119.2°C. How much heat is involved in converting it to a liquid with a temperature of -94.0°C? Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°Carrow_forwardThe following information is given for n-pentane, C5H12, at 1atm: AHvap(36.2 °C) = 25.8 kJ/mol boiling point specific heat liquid = 36.2 °C = 2.28 J/g °C At a pressure of 1 atm, normal boiling point of 36.2 °C. kJ of heat are needed to vaporize a 25.5 g sample of liquid n-pentane at itsarrow_forwardHow much heat is required to warm 25.0 g of H2O from a solid at -12ºC to a liquid at 60ºC? ∆Hfus = 6.02 kJ/mol Csolid = 2.09 J/gºC Cliq = 4.18 J/gºC Tfreezing = 0ºCarrow_forward
- Determine the amount of heat, in kJ, required to heat 19 g of solid Ca at 125 C to 851C (still solid). Melting Point = 851C Boiling Point = 1487C Molar Heat Capacities: Csolid = 26.2 J/mol C C liquid = 31.0 J/molC AH_fusion = 9.33 kJ/mol AH_vaporization = 162 kJ/molarrow_forwardThe following information is given for benzene, C6H6, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point = 80.1 °C specific heat liquid = 1.74 J/g°C At a pressure of 1 atm, boiling point of 80.1 °C. kJ of heat are needed to vaporize a 40.2 g sample of liquid benzene at its normalarrow_forwardWhat quanity of energy does it take to convert 0.451 kg ice at -20.0 degrees celcius to steam at 250.0 degrees celcius? Specific heat capacities: Ice, 2.03J/g degrees celcius; liquid, 4.18 J/g degrees celcius; steam, 2.02 J/g degrees celcius. delta H vap = 40.7kJ/mol; deltaHfus = 6.02kJ/molarrow_forward
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