Ammonium hydrogen sulfide, NH4HS, is unstable at room temperature and decomposes: NH4HS(s) ↔ NH3(g) + H2S(g) If you place some solid Ammonium hydrogen sulfide in the closed flask, in which of the following case it will produce less hydrogen sulfide gas- a) Removing some ammonia b) Adding some ammonia c) Removing some Ammonium hydrogen sulfide d) Increasing the pressure in the flask..
Ammonium hydrogen sulfide, NH4HS, is unstable at room temperature and decomposes:
NH4HS(s) ↔ NH3(g) + H2S(g)
If you place some solid Ammonium hydrogen sulfide in the closed flask, in which of the
following case it will produce less hydrogen sulfide gas-
a) Removing some ammonia
b) Adding some ammonia
c) Removing some Ammonium hydrogen sulfide
d) Increasing the pressure in the flask..
Equal numbers of moles of two soluble substances; A & B, are dissolved into 1 L of water
separately. Explain the following:
a) The Water samples are cooled down. Solution A freezes at -0.5°C and B at -1°C. How
these solutions can have different freezing points?
b) Compare the freezing point of 500 mL of solution B with the 1 L of solution A.
c) Calculate the molality of the solution A & B assuming i=1 for substance A.
d) Describe the change of freezing point if you add 1 Kg of water into solution B.
e) What would be the concentrations of A & B if they have the freezing point of -0.05°C?
f) Compare the all-other colligative properties of the original solutions of A & B.
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