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earnstyle [38]
3 years ago
14

How many moles of ammonium carbonate are needed to decompose in order to produce 6.52g of carbon dioxide? Ammonium oxide is the

other product.
A.) 0.116 moles

B.) 0.251 moles

C.) 0.148 moles

D.) 286.88 moles


Help me solve please...
Chemistry
1 answer:
pychu [463]3 years ago
3 0

Answer:

Option (C) is correct.

Explanation:

Decomposition reaction: (NH_{4})_{2}CO_{3}\rightarrow 2NH_{3}+CO_{2}+H_{2}O

Molar mass of CO_{2} = 44.01 g/mol

No. of moles = (mass)/(molar mass)

So, 6.52 g of CO_{2} = \frac{6.52}{44.01} moles of CO_{2} = 0.148 moles of CO_{2}

According to balanced equation-

1 mol of CO_{2} is produced from decomposition of 1 mol of (NH_{4})_{2}CO_{3}

So, 0.148 mol of CO_{2} is produced from decomposition of 0.148 mol of (NH_{4})_{2}CO_{3}

Hence, option (C) is correct.

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2. Size of the X atom.

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4. Oxidation state of the central atom

5. Values of Ka and pKa.

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So, we will base the force of an acid by it's pKa value.

The pKa value which is calculated with the expression:

pKa = -logKa

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So calculating the pKa on every structure we have:

HF: pKa = -log(3.5x10^-4) = 3.46

HNO2: pKa = -log(4.6x10^-4) = 3.34

HCN: pKa = -log(4.9x10^-10) = 9.31

HCOOH: pKa = -log(1.8x10^-4) = 3.74

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Answer:

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mass[m]=3g

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