How many grams of nitric acid are needed to produce 30.0 g of water?

4Zn+10HNO3=4Zn (NO3) 2+NH4NO3+3H2O

Mass = 32.13 g

Explanation:

Given dа ta:

Mass of water produced = 30 g

Mass of nitric acid needed = ?

Solution:

Chemical equation:

4Zn + 10HNO₃ → 4Zn (NO₃) ₂ + NH₄NO₃ + 3H₂O

Number of moles of water:

Number of moles = mass/molar mass

Number of moles = 30 g / 18 g/mol

Number of moles = 1.7 mol

Now we will compare the moles of water with nitric acid.

HNO₃ : H₂O

10 : 3

1.7 : 3/10*1.7 = 0.51 mol

Mass of nitric acid:

Mass = number of moles * molar mass

Mass = 0.51 mol * 63.01 g/mol

Mass = 32.13 g