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Vilka [71]
3 years ago
8

When entering coefficients to balance equations, recall that just writing the symbol implies "1." Therefore, if a coefficient of

"1" is required, choose "blank" for that box. Balance the following reaction. MgCl2 + AgNO3 → AgCl + Mg(NO3)2
Chemistry
1 answer:
ANEK [815]3 years ago
6 0

The balanced equation is MgCl₂ +2AgNO₃ ⟶ 2AgCl + Mg(NO₃)₂

<em>Step 1</em>. Start with the most complicated-looking formula [Mg(NO₃)₂].

Put a 1 in front of it and balance its atoms.

MgCl₂ +AgNO₃ ⟶ AgCl + <u>1</u>Mg(NO₃)₂

<em>Step 2</em>. Balance Mg.

<u>1</u>MgCl₂ +AgNO₃ ⟶ AgCl + <u>1</u>Mg(NO₃)₂

Already balanced —1 atom each side.

<em>Step 3</em>. Balance N.

We have 2 N on the right-hand side and 1 N on the left. We need 2 N on the left. Put a 2 in front of AgNO₃.

<u>1</u>MgCl₂ +<u>2</u>AgNO₃ ⟶ AgCl + <u>1</u>Mg(NO₃)₂

<em>Step 4</em>: Balance O

Done. We have 6 O on the left and 6 O on the right.

<em>Step 5</em>. Balance Ag.

We have 2 Ag on the left, so we need 2 Ag on the right. Put a 2 in front of AgCl.

<u>1</u>MgCl₂ +<u>2</u>AgNO₃ ⟶ <u>2</u>AgCl + 1Mg(NO₃)₂

The balanced equation is

MgCl₂ +2AgNO₃ ⟶ 2AgCl + Mg(NO₃)₂

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First we have to calculate the standard electrode potential of the cell.

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Now we have to calculate the standard Gibbs free energy.

Formula used :

\Delta G^o=-nFE^o_{cell}

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Now put all the given values in this formula, we get the Gibbs free energy.

\Delta G^o=-(2\times 96500\times (-0.47))=+90710J/mole=+90.71kJ/mole\approx +91kJ/mole

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The given chemical equation is:

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The ions which are present on both the sides of the equation are are not involved in net ionic equation.

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