Consider the following reaction. how many grams of water are required to form 75.9 g of hno3? assume that there is excess no2 present. the molar masses are as follows: h2o = 18.02 g/mol, hno3 = 63.02 g/mol. no2(g) + h2o(l) → hno3(aq) + no(g)

The mass of water required will be 10.848 g.

Explanation:

To calculate the number of moles, we use the equation:

   ......(1)

Given mass of nitric acid = 75.9 g

Molar mass of nitric acid = 63 g/mol

Putting values in above equation, we get:

For the given chemical equation:

By Stoichiometry of the reaction:

2 moles of nitric acid is produced by 1 mole of water.

So, 1.204 moles of nitric acid will be produced by = of water.

Now, calculating the amount of water, we use equation 1:

Moles of water = 0.602 mol

Molar mass of water = 18.02 g/mol

Putting values in equation 1, we get:

Hence, the mass of water required will be 10.848 g.

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one negative thing it that it can kill water animals. another negative thing is it can cause the destruction of ecosystem. one way water pollution can be reduced is to conserve energy.