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2 years ago

Write a net ionic equation for the reaction that occurs when excess hydroiodic acid and chromium(II) carbonate (s) are combined.

Chemistry

1 answer:

babymother [125]2 years ago

8 0

Step 1: Write the balanced "molecular equation:

$2HI(aq) + CrCO₃ (s) → CrI₂ (s) + H₂O(l) + CO₂(g)$

Step 2: Carbon dioxide and water are written in molecular form. Consult the solubility and net ionic equation rules on the information page to determine which of the other substances will dissociate:

$2HI(aq) + CrCo₃ (s) → Crl₂ (s) +H₂O(l)+CO₂(g)$

yes no yes

Step 3: Dissociate all soluble salts, strong acids, and strong bases (except calcium hydroxide), Leave together all "not soluble" salts and weak acids or bases:

${2H₂O}^{ + } (aq) + {2I}^{ - } (aq) + CrCO₃ (s)→ {Cr}^{2 + } (aq) + {2I}^{ - }(aq) + 3H₂O(l) + CO₂(g)$

Step 4: Cross out "spectator lons that appear on both sides of the reaction (these lons do not participate in the chemistry) and rewrite the "net" reaction using the smallest possible coefficients:

${2H₂O}^{ + } (aq) + CrCO₃ (s) →3H₂O + CO₂ + {Cr}^{2 + }$

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3 years ago

Fe(s) + 2HCl(aq) --> FeCl2(aq) + H2(g)

soldier1979 [14.2K]

Answer:

In the option(A) moles of HCl left are 0.100 moles which is wrong, making the option incorrect.

Explanation:

$Fe(s) + 2HCl(aq)\rightarrow FeCl_2(aq) + H_2(g)
$

Moles of HCl = n

Molarity of HCl = 1.0M

Volume of HCl solution = 30.0 mL = 0.030 L (1 mL = 0.001L)

$Moles=Molarity\times Volume (L)$

$n=1.0M\times 0.030 L=0.030 mol$

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According to recation , 1mol of Fe reacts with 2 mol HCl. Then 0.01 mole of Fe will recat with :

$\frac{2}{1}\times 0.01 mol= 0.02 mol$ of HCl

This means that HCl uis in excess , hence excessive reagent.

Moles of HCl left unreacted :

= 0.030 mol - 0.020 mol = 0.010 mol

But in the option moles of HCl left are 0.100 moles which is wrong, making the option incorrect.

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3 years ago

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Answer:

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2 years ago

Read 2 more answers