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?}

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

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