Answer:
A
Explanation:
Got a calculation of 8.05297
Answer:
84.4g of AgCl
Explanation:
Based on the reaction:
2AgNO₃ + CaCl₂ → 2AgCl + Ca(NO₃)₂
<em>2 moles of AgNO₃ and 1 mole of CaCl₂ priduce 2 moles of AgCl and 1 mole of Ca(NO₃)₂</em>
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100g of each reactant are:
AgNO₃: 100g × (1mol / 169.87g) = 0.589 moles
CaCl₂: 100g × (1mol / 110.98g) = 0.901 moles
For a complete reaction of 0.901 moles of CaCl₂ are necessaries 0.901×2 = <em>1.802 moles of AgNO₃. </em>As there are just 0.589moles, <em>AgNO₃ is limitng reactant</em>
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0.589 moles of AgNO₃ produce:
0.589 moles × ( 2 moles AgCl / 2 moles AgNO₃) =
<em>0.589 moles of AgC</em>l. In mass:
0.589 moles of AgCl × (143.32g / mol) =<em> 84.4g of AgCl</em>
Answer:
To determine a molecular formula from the empirical formula you need to know:
-the molecular mass
-calculate the empirical formula mass
-divide the molecular formular by the empirical formula mass
-multiply by this whole number the empirical formula
Explanation:
See the image below
