Silver nitrate solution reacts with calcium chloride solution according to the equation 2AgNO_3...
Question:
Silver nitrate solution reacts with calcium chloride solution according to the equation
2AgNO_3 (aq) + CaCI_2 (aq) --> Ca(NO_3)_2 (aq) + 2AgCI (s)
If a solution containing 6.30 g of AgNO_3 is mixed with a solution containing 4.20 g of CaCI_2/what mass of excess reagent remains?
a.3.04 g
b.5.32 g
c.6.21 g
d.1.87 g
e.2.14 g
Balanced Chemical Reaction:
The balanced chemical reaction tells us that 2 moles of silver nitrate react with 1 mole of calcium chloride. We can determine how many moles of silver nitrate and calcium chloride we have using their molar masses. One species will be reacted entirely and the other will be in excess.
Answer and Explanation: 1
We will first determine how many moles of each of the reactants we have. The molar mass of silver nitrate is 169.87 g/mol. The molar mass of calcium chloride is 110.98 g/mol.
{eq}6.30g \cdot \frac{1mol}{169.87}=0.0371mol\:AgNO_3\\ 4.20g \cdot\frac{1mol}{110.98g}=0.0378mol\:CaCl_2 {/eq}
Because it takes 2 moles of silver nitrate to react with 1 mole of calcium chloride, in order to react all of the calcium chloride, we would need 0.0756 moles of silver nitrate. We do not have this much silver nitrate.
We need 0.0186moles of calcium chloride to react with all of the moles of silver nitrate. We have this and more. After the 0.01855 moles of calcium chloride react there are 0.0378-0.0186=0.0192moles of calcium chloride remaining. This amount is in excess. The mass of this excess is:
{eq}0.0192moles \cdot \frac{110.98g}{1mol}=2.13g {/eq}
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Limiting Reactants & Calculating Excess Reactants
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