An aqueous solution is 22.0% by mass ethanol. CH3CH2OH, and has a density of 0.9

Question

An aqueous solution is 22.0% by mass ethanol. CH3CH2OH, and has a density of 0.966 g/mL. The molality of ethanol in the solution is [ ]m. An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of 102 gmL. The mole fraction of hydrochloric acid in the solution is [ ] . The equilibrium constant, Kc, for the following reaction is 1.80E-2 at 698 K. Calculate Kp for this reaction at this temperature. 2HI(g) H2(g) + I2(g) The equilibrium constant, Kc, for the following reaction is 1.80E-2 at 698 K. NH4HS NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.87L container at 298K contains 1.30 mol of NH4HS(s) and 0.344 mol of NH3, the number of moles of H2S present is [ ]moles.

Explanation / Answer

1. 6.26

2. 0.178

3. 6.06*10^5

4. 0.018

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