How many moles of calcium chloride (cacl2) are needed to react completely with 6.2 moles of silver nitrate (agno3)? 2agno3 + cacl2 → 2agcl + ca(no3)2 a. 2.2 mol cacl2 b. 3.1 mol cacl2 c. 6.2 mol cacl2 d. 12.4 mol cacl2

Here we have to choose the right option which tells the moles of CaCl₂ will react with 6.2 moles of AgNO₃ in the reaction

2AgNO₃ + CaCl₂→ 2AgCl + Ca(NO₃)₂

6.2 moles of silver nitrate (AgNO₃) will react with B. 3.1 moles of calcium chloride (CaCl₂).

From the reaction: 2AgNO₃ + CaCl₂→ 2AgCl + Ca(NO₃)₂

Thus 2 moles of AgNO₃ reacts with 1 mole of CaCl₂

Henceforth, 6.2 moles of AgNO₃ reacts with = 3.1 moles of CaCl₂.

1 mole of CaCl₂ reacts with 2 moles of AgNO₃. Thus-

A. 2.2 moles of CaCl₂ will react with 2.2×2 = 4.4 moles of AgNO₃.

C. 6.2 moles of CaCl₂ will reacts with 6.2×2 = 12.4 moles of AgNO₃.

D. 12.4 moles of CaCl₂ will reacts with 12.4 × 2 = 24.8 moles of AgNO₃

Thus the right answer is 6.2 moles of AgNO₃ will react with 3.1 moles of CaCl₂.

For the complete reaction of 6.2 moles of Silver nitrate, 3.1 moles of Calcium chloride has been needed.

The balanced chemical reaction can be as follows:

From the reaction, it is clear that 2 moles of silver nitrate require 1 mole of calcium chloride, for complete utilization.

If 2 moles of silver nitrate has been utilized by 1 mole of calcium chloride, then 6.2 moles of silver nitrate requires:

2 moles Silver nitrate = 1 mole Calcium chloride

6.2 moles Silver nitrate = moles Calcium chloride

6.2 moles Silver nitrate = 3.1 moles of Calcium chloride

For the complete reaction of 6.2 moles of Silver nitrate, 3.1 moles of Calcium chloride has been needed.

For more information about the Moles of a compound, refer to the link:

link