Question

Cr-->Cr2O3-->CrCl3-->Cr(OH)3-->Cr2O3-->Cr

Answer 1

1.  4Cr+3o2=2cr2o3
2   Cr2O3+ 6hcl=2CrCl3+3H2o
3    CrCl3+3naoh=Cr(oh)3+3naCl
4    2Cr(oh)3= Cr2o3+3h2o

 5   Cr2o3+2Al=2Cr+al2o3 

Answer 2

The series you provided represents a set of chemical reactions involving chromium (Cr) in different oxidation states and various compounds. Let's go through each reaction step by step:

1. Cr → Cr2O3: This reaction represents the oxidation of chromium (Cr) to chromium(III) oxide (Cr2O3) through the addition of oxygen. The balanced equation for this reaction is:

4 Cr + 3 O2 → 2 Cr2O3

2. Cr2O3 → CrCl3: In this step, chromium(III) oxide (Cr2O3) reacts with hydrochloric acid (HCl) to form chromium(III) chloride (CrCl3) and water (H2O). The balanced equation for this reaction is:

Cr2O3 + 6 HCl → 2 CrCl3 + 3 H2O

3. CrCl3 → Cr(OH)3: Chromium(III) chloride (CrCl3) reacts with sodium hydroxide (NaOH) to yield chromium(III) hydroxide (Cr(OH)3) and sodium chloride (NaCl). The balanced equation for this reaction is:

CrCl3 + 3 NaOH → Cr(OH)3 + 3 NaCl

4. Cr(OH)3 → Cr2O3: Chromium(III) hydroxide (Cr(OH)3) can undergo dehydration to form chromium(III) oxide (Cr2O3). The balanced equation for this reaction is:

2 Cr(OH)3 → Cr2O3 + 3 H2O

5. Cr2O3 → Cr: Finally, chromium(III) oxide (Cr2O3) can be reduced to chromium metal (Cr) by the addition of carbon (C) and heating. The balanced equation for this reaction is:

2 Cr2O3 + 3 C → 4 Cr + 3 CO2

In summary, the series of reactions you provided describes the transformation of chromium from its elemental form (Cr) to chromium(III) oxide (Cr2O3), then to chromium(III) chloride (CrCl3), followed by the formation of chromium(III) hydroxide (Cr(OH)3). The chromium(III) hydroxide can be dehydrated back to chromium(III) oxide, and finally, the chromium(III) oxide can be reduced to elemental chromium (Cr) by the addition of carbon and heating.