Determine the heat flow (in units of kJ) when 49.7 g water at 131.3°C is lowered to 82.6°C? molar mass of water = 18.0152 g/mol %3D enthalpy of fusion of water = 6.01 kJ/mol enthalpy of vaporization of water = 40.79 kJ/mol specific heat of solid water = 2.03 J/(g - °C) specific heat of liquid water = 4.184 J/(g °C) specific heat of vapor water = 1.99 J/(g- °C) Recall that q = mxsxAT

Determine the heat flow (in units of kJ) when 49.7 g water at 131.3°C is lowered to 82.6°C? molar mass of water = 18.0152 g/mol %3D enthalpy of fusion of water = 6.01 kJ/mol enthalpy of vaporization of water = 40.79 kJ/mol specific heat of solid water = 2.03 J/(g - °C) specific heat of liquid water = 4.184 J/(g °C) specific heat of vapor water = 1.99 J/(g- °C) Recall that q = mxsxAT

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.450 kg of water decreased from 103 °C to 42.0 °C. NOTE: MOLAR specfic heat capacities (Cp.n) are given here! Property Value Units °C Melting point Boiling point 100.0 °C AHfus 6.01 kJ/mol AHvap 40.67 kJ/mol p (s) 37.1 J/mol . °C 75.3 J/mol °C 33.6 J/mol · °C kJ
578,070 J of heat is required to raise the temperature of 15.0 moles of liquid methanol, CH3OH, from 25.0 °C to its boiling point (64.6 °C) and then to completely evaporate the methanol at that temperature. The specific heat of liquid methanol is 2.53 J g^-1 K ^-1 . Calculate the enthalpy of vaporisation of the compound.
Can you help with 1 and 2
2. Calculate the amount of energy (in kJ) needed to heat 100 g of H₂O(1) from 0°C to 210°C. The molar heat of vaporization of water at 100°C is 40.7 kJ/mol. [Specific heat: H₂O(1) = 4.184 J/g °C, H₂O(g) = 1.996 J/g °C)].
A 0.439 mol sample of liquid propanol (60.09 g/mol) is heated from 25.6°C to 328.3PC. The boiling point of propanol is 206.6°C. The specific heat of liquid propanol is 2.40 J/g°C. The specific heat of propanol vapor is 1.42 J/g°C. The enthalpy of vaporization for propanol is 47.5 kJ/mol. What is the energy change of this process, in kJ?
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.950 kg of water decreased from 111 °C to 25.0 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
Which is not true regarding the specific heat of water? The specific heat of water explains capillary action. The specific heat of water is 4.18 J/( C g). Water is useful as an engine coolant because of its high specific heat The specific heat of water is the reason islands have milder climates.
Please don't provide handwritten solution...
Energy Constants for H2O334 J/g = Heat of Fusion (Hf)2260 J/g = Heat of Vaporization (Hv)2.11 J/goC = Specific Heat Capacity of solid water4.18 J/goC = Specific Heat Capacity of liquid water2.00 =J/goC = Specific Heat Capacity of water vapor 2. How much energy is needed to completely boil away 250 g of 40oC water into 100oC water vapor?
If a particular liquid has a normal boiling point of 338.0 K and a vapor pressure of 75.0 mmHg at 285.0 K, determine AHvap for the liquid. wents.ics B CertainGovernm.pdf A CertainGovernm.pdf A 2020 W-2 and E.pdf MacBook Pro G Search or type URL 6
Based on the thermodynamic properties provided for water, determine the amount of energy released for 50.00 g of water to go from 62.0 °C to -17.0 °C. Property Melting point Boiling point 12.3 AHfus Hvap Cp (s) Cp (1) Cp (g) kJ Value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 Units. °C °C kJ/mol kJ/mol J/mol · °C J/mol · °C J/mol °C
Mening 10. suomming Condensation freezing boiling deposition Calculate the enthalpy change upon converting 1.50 g of water at -45.0 °C to steam at 115.0 °C under a constant pressure of 1 atm. The specific heats of ice, liquid water, and steam are 2.03 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, AHfus = 6.01 kJ/mol and AHvap = 40.67 kJ/mol.