Looking at the following image of a curve of partial pressures vs mole fractions of the two components A and B of an ideal mixture of liquids that obeys Raoult's Law where pa and Pa are the partial pressures of the two liquids A and B respectively and xa and xg are the mole fractions of A and B respectively, which of the following statements is true? R A. The intercepts R and S are representative of the equilibrium vapour pressures of the components A and B respectively B. The intercepts R and S are representative of the equilibrium vapour pressures of the components B and A respectively C. The slopes of the two curves, red and blue, are representative of the equilibrium vapour pressures of the components A and B respectively O D. Both (B) and (C) E. The slopes of the two curves, red and blue, are representative of the mole fractions of the components A and B respectively

Acetone has a vapour pressure of 53.3 kPa at 39.5 °C and 202.6 kPa at 78.6 °C. From the above data, obtain an equation to correlate the vapour pressure of acetone. (The equation should be in the form In(P)= -A/T + Co where P, is in kPa units. Find numerical values for A and Co) A= 5756 K, Co = 17.989 A= 4756 K, Co = 16.989 A= 3756 K, Co = 15.989 A= 2756 K, Co = 14.989

If there is a negativeor positive deviation in an ideal solution (Raoult's Law) what does that mean in terms of the intermolecular forces in the mixture and the value of enthalpy of solution?

4. The vapor pressures of pure C5H12 and C6H14 at 298.15K are 511 torr and 150 torr, respectively. Determine the partial pressures of the components, and the composition (mole fractions) of the vapor above an equimolar mixture of these two liquids at 298.15K

both pls

Assume seawater as a 3.7% NaCl (M(NaCl) = 58 g mol-1) solution by mass fraction. Which freezing point depression is to be expected with a melting enthalpy ∆H of 6.008 kJ mol-1?