The vapor pressure of liquid antimony is 400 mm hg at 1.84×103 k. assuming that its molar heat of vaporization is constant at 115 kj/mol, the vapor pressure of liquid sb is 394.98 mm hg at a temperature of 1.81×103 k. find the vapor pressure of liquid sb?

Vapor pressure of liquid Sb = 8.19 x 10⁴ mm Hg

Explanation:

The vapor pressure can be calculated by using Clausius‐Clapeyron equation.

ln(p₁/p₂) = (-ΔHvap/R)(1/T₁ - 1/T₂)

Where

p₁ is the vapor pressure at T₁ (Initial Temperature)

p₂ is the vapor pressure at T₂ (final Temperature)

ΔHvap is molar heat of vaporization of the substance

R is the real gas constant = 8.314 x 10⁻³ kJ/mol.K

Data Given:

p₁ = ?

p₂ = 394.98 mm Hg

T₁ = 1.84×10³ K

T₂ = 1.81×10³ K

ΔHvap = 115 kJ/mol

Put the values in the Clausius‐Clapeyron equation

                             ln(p₁/p₂) = (-ΔHvap/R)(1/T₁ - 1/T₂)

ln(p₁/394.98 mm Hg) = (-115 kJ/mol / 8.314 x 10⁻³ kJ/mol.K)(1/1.84×10³ K- 1/1.81×10³ K)

ln(p₁ /394.98 mm Hg) = (- 13.8321 x 10³)(-0.5519)

ln(p₁ /394.98 mm Hg) = 7633.936

ln cancel out by E, e is raise to a power x

So,

p₁/394.98 mm Hg = e^7633.936

p₁/ 394.98 mm Hg =    20.75 x 10³

p₁ = 20.75 x 10³ x 394.98 mm Hg

p₁ = 8.19 x 10⁴ mm Hg

Vapor pressure of liquid Sb = 8.19 x 10⁴ mm Hg

338 mm Hg

Explanation:

)

ln(p2/400)=-0.16705

p2/400= e^-0.16705=0.84615

p2=0.84615*400=338

Note that T2 is lower than T1 and that the vapor pressure decreases as the temperature decreases.

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.

definition

                    entropy is a measure of the randomness or the extent of disorder of a chemical process.

                      enthalpy is a measure of the heat change of a reaction occurring at a constant pressure.

measurement units:

                        entropy is measured in joule per kelvin (jk⁻¹)   whereas enthalpy is measured in joule per mole (jmol⁻¹)

requirements:

                            entropy has no requirements or limits, and its change is measured by the division between the heat change of the chemical process and the temperature.

                              in contrast, enthalpy can only be related to the heat change of the reaction under standard conditions.