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3 years ago

What's the balanced chemical equation of magnesium reacting with silver nitrate to produce silver and magnesium nitrate?

Chemistry

1 answer:

Strike441 [17]3 years ago

4 0

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

Step 1. Write the unbalanced equation

Mg + AgNO₃ ⟶ Mg(NO₃)₂ + Ag

Step 2. Start with the most complicated-looking formula [Mg(NO₃)₂] and balance its atoms.

Mg: Already balanced —1 atom each side.

N: We need 2 N on the left. Put a 2 in front of AgNO₃.

1Mg + 2AgNO₃ ⟶ 1Mg(NO₃)₂ + Ag

O: Already balanced —6 atom6 each side.

Step 3: Balance Ag

We have 2Ag on the left. We need 2Ag on the right.

1Mg + 2AgNO₃ ⟶ 1Mg(NO₃)₂ + 2Ag

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Consider the following reaction. SO2Cl2 → SO2 + Cl2. After collecting experimental data you found that plotting ln[SO2Cl2] vs. t

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Answer:

$[SO_2Cl_2]_{600}= 0.0842 M$

Explanation:

Some theoretical knowledge is required here. We should understand that whenever we plot the natural logarithm, ln, of a concentration vs. time and obtain a straight line, this indicates a first-order reaction. That said, since this is the case here, we have a first-order reaction with respect to $SO_2Cl_2$ .

The linear equation has the following terms:

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It is a linear form of the integrated first-order law equation:

$ln[SO_2Cl_2]_t = -kt + ln[SO_2Cl_2]_o$

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Using the equation, we may substitute for t = 600 s and obtain the natural logarithm of the concentration at that time:

$ln[SO_2Cl_2]_{600} = -0.000290 s^{-1}\cdot 600 s - 2.30 = -2.474$

Take the antilog of both sides to find the actual molarity:

$[SO_2Cl_2]_{600}=e^{-2.474} = 0.0842 M$

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