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 data:

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

false

because it does not have the potential to be entirely used up

idk what the question is about