Question

agno₃ + hcl → agcl + hno₃
50.0 ml of 0.20 m agno₃ is added to
50.0 ml of 0.20 m hcl. the resulting
temperature change is an increase of
1.60 °c.
\\(c_{sol} = 4.20\space j/g\space °c\\) \\(d_{sol} = 1.02\space g/ml\\) \\(c_{cal} = 5.60\space j/°c\\)
\\(mass_{sol} = 102\space g\\) \\(q_{rxn} = -694\space j\\)
how many moles reacted?
moles reacted = ? mol

Explanation:

Step1: Determine moles of \(AgNO_3\)

Volume of \(AgNO_3\) is \(50.0\space mL = 0.0500\space L\), molarity \(M = 0.20\space M\). Using \(n = M\times V\), \(n_{AgNO_3}=0.20\space mol/L\times0.0500\space L = 0.010\space mol\).

Step2: Determine moles of \(HCl\)

Volume of \(HCl\) is \(50.0\space mL = 0.0500\space L\), molarity \(M = 0.20\space M\). Using \(n = M\times V\), \(n_{HCl}=0.20\space mol/L\times0.0500\space L = 0.010\space mol\).

Step3: Check stoichiometry

The reaction \(AgNO_3 + HCl
ightarrow AgCl + HNO_3\) has a 1:1 stoichiometry. Both reactants have 0.010 mol, so the limiting reactant is either (both same moles). Thus, moles reacted is 0.010 mol.

Answer:

\(0.010\)