The vapor pressure of substance x is measured at several temperatures: temperature (c) vapor pressure (atm)34 0.23644 0.29254 0.355use this information to calculate the enthalpy of vaporization of x. round your answer to 2 significant digits. be sure your answer contains a correct unit symbol. clears your work. undoes your last action. provides information about entering answers.

ΔHv = 17.04 KJ/mol

Explanation:

T(°C)   T(K)      Pv(atm)         1/T(K)                LnPv

34      307      0.236       0.00325733      - 1.4439

44      317       0.292       0.0031545         - 1.2310

54      327      0.355       0.003058          - 1.0356

Clausius-Clapeyron:

⇒ δLnP = ΔH/R (δT/T²)

∴ δT/T² = δ/δT(- 1/T )

⇒ δLnP/δT = - ΔH/R

Graphing: LnP vs 1/T

we get an ecuation that corresponds to a straight line:

y = - 2049.6x + 5.2331 R² = 1

where the slope of this line is:

y = mx + b

⇒ m = - 2049.6 = - ΔH/RClausius-Clapeyron

⇒ ΔH = (2049.6)(R)

∴ R = 8.314 E-3 KJ/mol.K

⇒ ΔHv = 17.04 KJ/mol

c is the answer because when something is left after something evaporates that shows the chemical change.

i have no clue hope you find the answer