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9966 [12]
3 years ago
13

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is exce

ss NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
Chemistry
1 answer:
adoni [48]3 years ago
8 0

Answer:

The answer is "10.84 g".

Explanation:

The formula for calculating the number for moles:

\text{Number of moles }= \frac{\ Mass}{ \ molar \ mass }

In the given acid nitric:

Owing to the nitric acid mass = 75.9 g

Nitric acid molar weight= 63\  \frac{g}{mol}

If they put values above the formula, they receive:

\text{moles in nitric acid} = \frac{75.9}{63}

                               =1.204 \ mol

In the given chemical equation:

3 NO_2 \ (g) + H_2O \ (l) \longroghtarrow 2 HNO_3 \ (aq) + NO\ (g)

In this reaction, 2 mols of nitric acid are produced by 1 mole of water.

So, 1.204 moles of nitric acid will be produced:

= \frac{1}{2} \times 1.204

=0.602\ \ \text{mol of water}.

We are now using Equation 1 in determining the quantity of water:

Water moles = 0.602\  mol

Water weight molar = 18.02 \ \frac{g}{mol}

\to 0.602 = \frac{\text{mass of mols}}{ 18.02}\\\\\to \text{mass of mols} = 0.602 \times 18.02\\\\

                         =10.84 \ g

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