Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl (s)….?

Two 2.00 L flasks at 25°C are connected by a stopc̫o̫ςκ. One flasks contains 5.00 g of NH3(g) and the other contains 5.00 g of HCl(g). When the stopc̫o̫ςκ is oƿє-ṅєd, the gases react until one is completely consumed.

Which gas will remain in the system after the reaction is complete?

What will be the final pressure of the system after the reaction is complete? (neglect the volume of the ammonium chloride formed)


3 Answers

  • Find the moles of each gas present. Use: g/MM = moles

    NH3 = 5.00g/(17.0304g/mole) = 0.294moles

    HCl = 5.00g/(36.461g/mole) = 0.137moles

    Since the gases react in a 1:1 ratio, there will be NH3 remaining (0.157 moles to be exact).

    The final volume is 4.00L, since the flasks are now open to each other. Assuming no temperature change due to the reaction, we can calculate as follows:

    P = nRT/V = (0.157moles)(0.0821Latm/Kmol)(298K)/4L = 0.960atm (730torr)

  • NH4Cl (aq) + NaOH (aq) ——-> NH4OH (aq) + NaCl (aq) OR NH4Cl (aq) + NaOH (aq) ———> NaCl (aq) + H2O (l)+ NH3 (g) it somewhat is a self balanced equation. A Bronsted-Lowry (BL) acid is defined as any substance that should donate a hydrogen ion (proton) and a Bronsted-Lowry base is any substance that should settle for a hydrogen ion (proton). consequently, in accordance to the BL definition, acids and bases might desire to are obtainable what’s called conjugate pairs. NH4Cl donates one H+, so because it somewhat is a lowry bronsted acid. NH3 is its conjugate base. NaOH is the backside…

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