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

Question

Two 2.00 L flasks at 25°C are connected by a stopcock. One flask contains 5.00 g of NH3(g), and the other contains 5.00 g of HCl(g). When the stopcock is opened, the gases react until one of them is completely consumed. Which gas will remain in the system after the reaction is complete? Additionally, what will be the final pressure of the system after the reaction is complete, assuming we neglect the volume of the ammonium chloride formed? Thank you!

Anonymous · Accepted Answer

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)

Anonymous · Answer

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…

Anonymous

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

2 Answers

AI-Powered Insights

Want to answer this question?

Categories

Tags

Related Questions