For the reaction below; NH_3 (g) + BF_3 (g) rightarrow H_3NBF_3 (s) Which of the

Question

For the reaction below; NH_3 (g) + BF_3 (g) rightarrow H_3NBF_3 (s) Which of the three different definitions of acid-base given by various Scientists is applicable? The K_a of a weak acid is 1.8 times 10^-4. What is the K_b of its conjugate base? An aqueous buffer contains acetic acid (CH_3COOH) and sodium acetate (CH_3COONa). Write down a reaction equation by which the buffer minimizes the pH change when HCl is added. State the third law of thermodynamics in not more than two sentences. Which of the four compounds below has the highest standard molar entropy? CH_4 (g), CH_3 CH_2 CH_3 (g), CH_3 CH_2 CH_3 (l) CH_3 (CH_2)_2 CH_3 (g). To cause the largest increase in entropy for one mole of an ideal gas, what changes must be made in terms of temperature and volume? (Use the words: Increase/Decrease to appropriately describe them. Calculate the delta G value for the reaction 2C_2H_6 (g) + 7O_2 (g) rightarrow 4CO_2 (g) + 6H_2O (g) delta H degree _ r times n = -2855.1 kJ, delta s degree _ r times n = 92.6 J.K-1. And indicate if under standard conditions the reaction will be spontaneous or non- spontaneous, at high or low temperatures.

Explanation / Answer

Q4) Lewis acid base theory

NH3 is Base - give pair of electron

BF3 is Acid - accept pair of electron

Q5) Kb = Kw/Ka

Kw = ionic product of water = 1×10^-14

Kb = 1×10^-14/1.8×10^-4

=5.56× 10^-11

Q6) HCl react with CH3COO-

HCl(aq) + CH3COO-(aq) ------> CH3COOH(aq) + Cl-(aq)

Concentration of CH3COO- decreased

Concentration of CH3COOH increased

pH = pKa - log([CH3COO-]/[CH3COOH])

Q7) The entropy of a perfect crystal at absolute zero temperature is exactly equal to zero

Q8) CH3(CH2)2CH3

Q9) Temperature - Incease

   Volume - Increase

Q10) G° = H° - TS°

   = -2855.1KJ - (298K × 0.0926KJ/K)

   = -28551KJ - 27.6 KJ

   = -28578.6KJ

H is negative

   S is positive

So , the reaction is spontaneous at higher and lower temperatures

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