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3 years ago

For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts.

Chemistry

1 answer:

Nesterboy [21]3 years ago

7 0

Answer:

0.712 mol of NO₂ are formed .

Explanation:

For the reaction , given in the question ,

2 N₂O₅ ( g ) → 4 NO₂ ( g ) + O₂ ( g )

From the above balanced reaction ,

2 mol of N₂O₅ reacts to give 4 mol of NO₂

Applying unitary method ,

1 mol of N₂O₅ reacts to give 4 / 2 mol of NO₂

From the question , 0.356 mol of N₂O₅ are reacted ,

<u>now, using the above equation , to calculate the moles of the NO₂ , as follow -</u>

Since ,

1 mol of N₂O₅ reacts to give 4 / 2 mol of NO₂

0.356 mol of N₂O₅ reacts to give 4 / 2 * 0.356 mol of NO₂

Calculating ,

0.712 mol of NO₂ are formed .

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3 years ago

Read 2 more answers

A chemist titrates 160.0mL of a 0.3403M aniline C6H5NH2 solution with 0.0501M HNO3 solution at 25°C . Calculate the pH at equiva

maxonik [38]

Answer : The pH of the solution is, 5.24

Explanation :

First we have to calculate the volume of $HNO_3$

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$M_1V_1=M_2V_2$

where,

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Putting values in above equation, we get:

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Now we have to calculate the total volume of solution.

Total volume of solution = Volume of $C_6H_5NH_2$ + Volume of $HNO_3$

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Now we have to calculate the pH of the solution.

At equivalence point,

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$pOH=\frac{1}{2}[14+4.87+\log (0.0437)]$

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3 years ago

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2 years ago

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The diagram illustrating this is shown on the second uploaded image

Explanation:

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