How do you Calculate how much sodium nitrate is needed to give 126g of nitric acid by reaction?

Answer 1

The reaction would be NaNO3 (s) + H2SO4 (l) -> HNO3 (l) + NaHSO4 (s)

Moles ratio 1 : 1 : 1 : 1

Moles of nitric acid:

= Mass / Mr

= 126g / HNO3

= 126g / (1) + (14) + (16 x 3)

= 126g / (1) + (14) + (48)

= 126g / 63

= 2 mol

sodium nitrate:nitric acid

Moles ratio 1 : 1

Actual moles in reaction 2 : 2

Mass of sodium nitrate:

= Moles x Mr

= 2 x NaNO3

= 2 x (23) + (14) + (16 x 3)

= 2 x (23) + (14) + (48)

= 2 x 85

= 170g

Mass of sodium nitrate needed = 170g

Answer 2

To calculate the amount of sodium nitrate needed to produce 126g of nitric acid, you first need to balance the chemical equation for the reaction between sodium nitrate and sulfuric acid to form nitric acid. Then, use stoichiometry to determine the molar ratio between sodium nitrate and nitric acid, and convert the given mass of nitric acid to moles. Finally, use the molar ratio to calculate the amount of sodium nitrate needed.