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In: Chemistry

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   

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

B) How many moles of each reactant does the reaction start with?

C)At STP, how many L of the gas is produced? (Ignoring water vapor)

D) Assuming the volume given in the problem remains the same, what is the molarity of the ionic compound 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?

F) How many L of your gas would be produced if the reaction was done at 25C at 0.992atm?

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Expert Solution

queen_honey_blossom answered 2 years ago
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