The normal boiling point of benzene is 80 °C. At 100 °C and 1 atm, which term isgreater in magnitude for the vaporization of benzene, ΔH or -TΔS?

3- Diethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6°C, diethyl ether has a vapor pressure of 760. torr, and at 17.9°C, it has a vapor pressure of 400 torr. What is the ΔH of vaporization for diethyl ether?

For a certain reaction, ΔHº = −1.8 x 102 kJ mol−1 and the equilibrium constant at 800. K is 9.1 × 102 . Estimate the temperature at which the equilibrium constant is 1.0 × 106 .

For an exothermic reaction     ΔH < 0     ΔH > 0     ΔH = 0     H = 0

Consider the synthesis of urea according to the equationCO2(g) + 2 NH3(g) −−→ (NH2)2CO(s) + H2O(l)Calculate the ∆rxnG−⊖−for the reaction at 25 ◦C for 3.25 mol of NH3 and an abundance of CO2. Assuming ∆rxnG−⊖− to be independent of temperature, what is the ∆Grxn for the reaction at a pressure of 10.0 atm? ∆rxnG−⊖−(CO2) = -394.36 kJ/mol ∆rxnG−⊖−(NH3)= -16.45 kJ/mol ∆rxnG−⊖−( (NH2)2CO)= -197.33 kJ/mol ∆rxnG−⊖−(H2O)= -273.13 kJ/mol

Oxygen (O₂) is necessary for cellular respiration; it must be transported from the lungs to tissues through the bloodstream. However, O₂ is not very soluble in water. The Keq of oxygen dissolving at 300.0 K is 7.64 x 10⁻⁴ and the Keq at 320.0 K is 5.23 x 10⁻⁴. Calculate the ∆H(dissolve) for oxygen solubility in water, in kJ/mol.

Calculate ΔGo for a reaction for which ΔHo = 24.6 kJ and ΔSo= 132 J/K at 298 K.

For a certain chemical reaction, the standard Gibbs free energy of reaction is  129.   kJ . Calculate the temperature at which the equilibrium constant K   =   ×6.010−25 .Round your answer to the nearest degree.

Suppose we redefine the standard state as P=4bar. Find the new standard ΔfG∘ values of the following substances.     Part A HCl (g)(ΔfG∘at1bar=−95.3kJmol−1)