According to the following reaction, how many moles of sodium chloride will be formed upon the complete reaction of 0.470 moles chlorine gas with excess sodium iodide? chlorine (g) + sodium iodide (s) > sodium chloride (s) + iodine (s) moles sodium chloride

There will be formed 0.940 moles of sodium chloride

Explanation:

Step 1: The balanced equation

2NaI + Cl2 → 2NaCl + I2

We see that for 2 moles of NaI consumed, there is needed 1 mole of Cl2 to produce 2 moles of NaCl and 1 mole of I2

Step 2: Given data

0.470 moles of chlorine gas will completely react with sodium iodide, in excess.

Step 3: Calculate moles

If chloring gas will completely react that means there will be consumed 0.470 moles of chlorine gas.

We know that for 1 mole of Cl2 there is consumed 2 moles of NaI

For 0.470 moles of Cl2, there is 2*0.470= 0.940 moles of NaI consumed

to form 0.940 moles of NaCl and 0.470 moles of I2.

There will be formed 0.940 moles of sodium chloride

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

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