The standard enthalpy of certain reaction is approximately constant at +125kjmol-1 from 800k to 1500k. the standard gibbs energy is +25kjmol-1 at 1150k. estimate the temperature at witch the equilibrium constant becomes greater than 1.

T = 3006.976 K

Explanation:

∴ ΔH° = 125 KJ/mol ( 800K - 1500K)

∴ ΔG° = 25 KJ/mol (1150 K)

⇒ T = ? ∴ K > 1

In the equilibrium:

∴ K > 1

If ΔG°/RT = 1

⇒ e∧(1) = 2.72 > 1

∴ ΔG°/RT = 1

⇒ T = ΔG°/R = (25 KJ/mol)/(8.314 E-3 KJ/mol.K)

⇒ T = 3006.976 K

verifying:

⇒ K = e∧(25/((8.314 E-3)(3006.976)))

⇒ K = 1.000000061 > 1

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

2b2t

explanation:

2b2t