ANSWERS Phase Diagram Questions.docx

12.) A 36.0 g sample of liquid water at 100.0oC is heated to 145.0 oC.   How much heat does the water absorb in this process?  What is its phase at the end?  You will need to use some of the information given below. Specific Heat Capacities: CS(H2O,s) = 2.09 J/g oC;  CS(H20, l) = 4.18 J/g oC;  CS(H2O,g) = 2.01 J/g oC ΔHofus =  6.02 kJ/mol;   ΔHovap =   40.7 kJ/mol.

Which equation calculates the temperature change of 100 g of water that absorbs the same amount of heat as it takes to boil 5 g of water?   Question 12 options:   (100 g / 18 g mol–1 × 40650 J mol–1)  / (5 g × 4.184 J g–1 °C–1)   (5 g / 18 g mol–1 × 40650 J mol–1)  / (100 g × 4.184 J g–1 °C–1)   (100 g × 4.184 J g–1 °C–1)  / (5 g / 18 g mol–1 × 40650 J mol–1)

(c) Is methane a solid, liquid, or gas at 1 atm and 0 °C? (d) If solid methane at 1 atm is heated while the pressure is held constant, will it melt or sublime? (e) If methane at 1 atm and 0 °C is compressed until a phase change occurs, in which state is the methane when the compression is complete?

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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.

What is the resulting temperature when 100 g of water at 75°C is mixed with 30 g of ice at 0 °C? Assume that all of the ice has melted. The specific heat of water is 4.184 J g-1 C°.-1 and the heat of fusion of ice is 335 J g-1.

Calculate total heat absorbed (kJ) for heating 36 g ice at – 10 °C into liquid water at 15 Oc. Cp,m (Ice) = 37.7 J/mol K, enthalpy of fusion of ice at 0.0 °C (AH°F) = 6025 J/mol and Cp.m (H20 ) = 75.3 J/mol K -

In the ICE table below, complete the "Change" values in terms of x for the reaction: 2S03(g) =2s02(g) + O2(g) Make sure to add the + or - sign where needed and formatted as +2x, +1x, 0, -1x, -2x, etc. 2S03(g) = 2S02(g) O2(g) %3D Change + X -3x Equilibrium 0.125 M ++ +2x +3x

Calculate the heat energy released when 19.5 g19.5 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point.

Use the following data to calculate AvapHo for water at 298 K. Avap Ho for water at 373 K is 40.7 kJ/mole. Cp is 75.2 J/Kmol for liquid and 33.6 J/Kmol for gaseous water. Is the value of Avap Ho higher or lower than at 373 K? Can you give a reason why?

Calculate the heat, in kJ, exchanged in the conversion of 20.0 g of steam at 104 °C to water at 10.5 °C. J Specific heat capacity, H20(s) = 2.087 g-ºC J Specific heat capacity, H20(1) = 4.184 g.ºC J Specific heat capacity, H20(g) = 2.042 g.°C %3D AH fus = 6.01 kJ/mol AH vap = 40.7 kJ/mol

How much heat does it take to raise 50.0 g of liquid water to 120 °C if its initial temperature is 50 °C? (Possibly useful values: Cwater = 4.184 J/g.°C, Csteam = 1.99 J/g.°C, Cice = 2.108 J/g.°C, AHfus 6.01 kJ/mol, AHvap = 40.79 kJ/mol) %3D %3D 142.3 kJ 14.6 kJ 312.6 kJ 125.6 kJ 284.3 kJ

Can you help with 1 and 2

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.450  kg of water decreased from 101  °C to 51.5  °C.  What is the kJ?  _____ kJ 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

A liquid has a ΔH°vapof 32.7 kJ/mol and a boiling point of 124°C at 1 atm. What is its vapor pressure at 101°C?

The heat of fusion of Hg at its normal melting point of -38.9°C is 2.82 calg^-1. The densities of solid and liquid mercury at 1 atm and at that temperature are 14.193 and 13.690 gcm^-3, respectively. Find its melting point at 200 atm.

Question 12 of 13 Given AH = -19.4 kJ/mol and AS = +92.3 J/mol-K, determine AG for the phase change CO:(g) → CO.(aq) at 25 °C. + 1 4 7 +/- 2 5 8 PE kJ/mol 3 6 9 0 Submit 冈 C x 100

H2O has a ΔHvap = 40.8 kJ/mol and a ΔHfus = 6.02 kJ/mol. The specific heat capacity of ice is 2.11 J/g•°C, of liquid water is 4.18 J/g•°C and of steam is 2.00 J/g•°C. Calculate the total heat transferred to elevate 250 g of pure water from –42 °C to 127 °C.

When 5.00 g of isopropyl alcohol ((CH3),CHOH; molar mass = point of 82.6°C, it absorbs 3.66 kJ of heat. What is the enthalpy of vaporization of isopropyl alcohol in kJ/mol? 60.09 g/mol) evaporates at its boiling

For water, specific heat values for the solid and liquid phase are 2.00 J/gC and 4.18 J/gC respectively andthe heat of vaporization and the heat of fusion are 2260 J/g and 334 J/g respectively   How doesthe slope of the ∆T line for a phase diagra from solid and liquid compare for water? Explain the comparison interms ofspecific heat capacities.▪ How does the horizontal length of the melting/boiling portions of the graph compare for water? Explain the comparison in terms of IMFs.

How much energy is needed to change the temperature of 39 g of water from 10.0 °C to 95.0 °C? Enthalpy values for H2O: Cp (g) = 1.89 J/g•°C Cp () = 4.18 J/g•°C Cp (s) = 2.11 J/g•°C ΔΗ AH us = 6.01 kJ/mol ΔΗ. vap = 40.7 kJ/mol

A liquid at 20.0 °C exhibits a vapor pressure of 0.555 atm. The liquid is heated to 60.0 °C. What is the new vapor pressure (in atm to three decimal places) if ΔHvap = 25.595 kJ mol–1?

How much heat is removed from the condensation of water at 25 °C? Given: S° H2O (1) = 69.9 J/mol·K and S° H2O (g) = 188.7 J/mol-K * %3D +35,420.2200 J/ mol O -35,420.2200 J/ mol O +34,520.2200 J/ mol O -34,520.2200 J/ mol

Ethanol 1C2H5OH2 melts at -114 °C and boils at 78 °C.The enthalpy of fusion of ethanol is 5.02 kJ>mol, and itsenthalpy of vaporization is 38.56 kJ>mol. The specific heatsof solid and liquid ethanol are 0.97 and 2.3 J>g@K, respectively.(a) How much heat is required to convert 42.0 g ofethanol at 35 °C to the vapor phase at 78 °C? (b) How muchheat is required to convert the same amount of ethanol at-155 °C to the vapor phase at 78 °C?

There are 270 Calories in a Hershey's® Milk Chocolate bar. The following data might be useful: AHvap = 43.9 kJ/mol, AHfusion = 6.02 kJ/mol, AHsublimation = 49.9 kJ/mol, specific heat of ice = 2.05 J g ¹°C 1, specific heat of water = 4.18 Jg ¹1°C-1, and specific heat of steam = 2.08 Jg ¹¹°C 1. Assume the specific heat of water does not change with temperature. (Density of ice = 0.920 g/mL). X Incorrect. How much energy is used up at each step of the heating, including heating the solid, melting, heating the liquid, and vaporization? If all of the energy in the bar were used to heat up 75.0 mL of ice at -25.0 °C, how hot would the water get? i 6406 ! °C

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