So let’s say you have a beaker that contains 6.02g ammonium chloride and to this you...

So let’s say you have a beaker that contains 6.02g ammonium chloride and to this you add 300.0mL of 0.450 M calcium hydroxide according to the following chemical equation: Ca(OH)2(aq) + 2NH4Cl(s)  CaCl2(aq) + 2H2O(l) + 2NH3(g) H = +90.66 kJ

A) draw the beaker at the end of the reaction- what would be in the beaker and or around it. what would the products look like on a molecular/atom/ion level?

B) at STP, how many L of your gas was produced? ignoring water vapor

C) why would water vapor be involved in this reaction?

D) assuming the aqueous volume given in the problem remains the same, what is the molarity of the two ions in the reaction at the end of the reaction? E) how many moles of excess reactant are left over at the end of the reaction?

Expert Solution

queen_honey_blossom answered 2 years ago

Expert Solution

queen_honey_blossom answered 2 years ago

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So let’s say you have a beaker that contains 6.02g ammonium chloride and to this you...

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