Question

Ethanol (C2H5OH) boils at 78∘C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g−K.

1. How much heat is required to convert 25.0 g of ethanol at 30 ∘C to the vapor phase at 78 ∘C?

2. Place the following substances in order of decreasing volatility: CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2. Rank from most volatile to least volatile. To rank items as equivalent, overlap them.

3. How do the boiling points vary through this series? Rank from highest to lowest boiling point. To rank items as equivalent, overlap them. CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2.

Answer #1

**Q1) heat of enthalpy vaporization = 38.56 KJ/mol = 38560
Joules/mol**

**Molar mass of Ethanol (C2H5OH) = 12 * 2 + 1 * 6 + 16 =
46 gm/mol**

**Heat of enthalpy vaporization per gm = 38560/46 = 838.26
J/gm**

**Heat Required = 25 * 2.3 * (78-30) + 838.26 *
25**

**=> 25 * 2.3 * 48 + 25 * 838.26**

**=> 23716.6**

**= 23.716 KJ**

**Q2) The order of decreasing voltality will
be**

**assuming that voltality is same per gm of compound, the
least weighted compound will be the most volatile and heavier
compounds will be less volatile, so the final order will
be**

**CH4 > CH3Cl > CH2Cl2 > CH2Br2 > CHBr3 >
CBr4**

**Q3) Lower the voltality, higher will be the boiling
point, hence in Q3, the reverse answer of Q2 will be
used**

**So the final order is**

**CH4 < CH3Cl < CH2Cl2 < CH2Br2 < CHBr3 <
CBr4**

Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The
enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of
vaporization is 38.56 kJ/mol. The specific heat of solid and liquid
ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively.
A. How much heat is required to convert 40.5
g of ethanol at 36 ∘C to the vapor phase at 78 ∘C?
B. How much heat is required to convert 40.5
g of ethanol at -161 ∘C to...

Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The
enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of
vaporization is 38.56 kJ/mol. The specific heat of solid and liquid
ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. Q: A) How much
heat is required to convert 36.5 g of ethanol at 35 ∘C to the vapor
phase at 78 ∘C? B) How much heat is required to convert 36.5 g of
ethanol at -167...

Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is
5.02 kJ/mol. The specific heats of solid and liquid ethanol are
0.97 J/g•K and 2.3 J/g•K, respectively. How much heat (kJ) is
needed to convert 25.0 g of solid ethanol at -125 °C to liquid
ethanol at -40 °C

Ethanol (C2H5OH) melts at -114°C. The
enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and
liquid ethanol are 0.97 J/gK and 2.3 J/gK, respectively. How much
heat (kJ) is needed to convert 25.0 g of solid ethanol at -135°C to
liquid ethanol at -50°C?

Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is
5.02 kJ/mol. The specific heats of solid and liquid ethanol are
0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is
needed to convert 25.0 g of solid ethanol at -135 °C to liquid
ethanol at -60 °C?
A. 207.3
B. -13.3
C. 6.34
D. 3617
E. 8.63

Ethanol (C2H5OH) melts at -114°C. The enthalpy of fusion is 5.02
kJ/mol. The specific heats of solid and liquid ethanol are 0.97
J/gK and 2.3 J/gK, respectively. How much heat (kJ) is needed to
convert 25.0 g of solid ethanol at -135°C to liquid ethanol at
-50°C?
A) 207.3 kJ
B) -12.7 kJ
C) 6.91 kJ
D) 4192 kJ
E) 9.21 kJ
Show all your calculations.

Ethanol, C2H5OH, (MW 46.06 g/mol) melts at
-114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats
of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K,
respectively. How much heat (kJ) is needed to convert 20.0 g of
solid ethanol at -135 °C to liquid ethanol at -50 °C?
please show work

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