How do we represent the oxidation of a $31.7 \cdot g$ $31.7*g$ mass of iron by chlorine gas? What mass of $F e C l_{3} (s)$ $FeCl_3(s)$ results?

Question

How do we represent the oxidation of a $31.7 \cdot g$ $31.7*g$ mass of iron by chlorine gas? What mass of $F e C l_{3} (s)$ $FeCl_3(s)$ results?

1 Answer

Impact of this question

1809 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2015-11-03T20:38:48

$F e (s) + \frac{3}{2} C l_{2} (g) \to F e C l_{3} (s)$ $Fe(s) + 3/2Cl_2(g) rarr FeCl_3(s)$

Explanation:

Moles of iron: $\frac{31.7 \cdot g}{55.85 \cdot g \cdot m o l^{- 1}}$ $(31.7*g)/(55.85* g* mol^-1)$ $=$ $=$ $? ? \cdot m o l$ $??*mol$

This molar quantity of iron requires $\frac{3}{2}$ $3/2$ molar equivalents of chlorine gas for complete reaction. What is oxidized, and what is reduced in the reaction? How do you know?

Science

Math

Humanities

... and beyond

How do we represent the oxidation of a $31.7 \cdot g$ $31.7*g$ mass of iron by chlorine gas? What mass of $F e C l_{3} (s)$ $FeCl_3(s)$ results?

1 Answer

Explanation:

Related questions

Impact of this question

Science

Math

Humanities

... and beyond

How do we represent the oxidation of a 31.7⋅g31.7*g mass of iron by chlorine gas? What mass of FeCl3(s)FeCl_3(s) results?

1 Answer

Explanation:

Related questions

Impact of this question

How do we represent the oxidation of a $31.7 \cdot g$ $31.7*g$ mass of iron by chlorine gas? What mass of $F e C l_{3} (s)$ $FeCl_3(s)$ results?