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How many grams of H2O are formed from the reaction of 34.7 g of NH3?

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Answer:

Step-by-step explanation:

NH3 + 3O2 -> NO + 2H2O

The balanced equation for the reaction of NH3 and O2 to form NO and H2O is:

4 NH3 + 5 O2 -> 4 NO + 6 H2O

From the balanced equation, we can see that for every 4 moles of NH3 that react, 6 moles of H2O are formed.

To find out how many grams of H2O are formed from 34.7 g of NH3, we can first convert the mass of NH3 to moles using the formula:

moles = mass/molar mass

The molar mass of NH3 is 17.03 g/mol.

So, 34.7 g of NH3 is equal to 34.7 g/17.03 g/mol = 2.04 moles of NH3

If 4 moles of NH3 react, 6 moles of H2O are formed.

So, if 2.04 moles of NH3 react, 2.04 moles/4 moles * 6 moles = 2.04 moles/4 * 6 moles = 3.06 moles of H2O are formed.

To find out the mass of 3.06 moles of H2O, we use the formula:

mass = moles * molar mass

The molar mass of H2O is 18.02 g/mol.

so, 3.06 moles of H2O weighs 3.06 moles * 18.02 g/mol = 55.18 g

In conclusion, 55.18 g of H2O are formed from the reaction of 34.7 g of NH3

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