Question

S + 6 HNO3 → H2SO4 + 6 NO2 + 2 H2O

In the above equation, how many grams of water can be made when 5.6 moles of HNO3 are consumed?

Answer 1

When 5.6 moles of HNO3 react, approximately 33.7 grams of water can be produced.

Step-by-step explanation:

To find the amount of water produced when 5.6 moles of HNO3 react, we can use the mole ratio from the balanced equation.

In the balanced equation, the mole ratio between HNO3 and H2O is 6:2. This means that for every 6 moles of HNO3, 2 moles of H2O are produced.

So, to find the moles of water produced, we can set up a proportion:

6 moles HNO3 / 2 moles H2O = 5.6 moles HNO3 / x moles H2O

Solving for x, the moles of H2O, we get:

x = (2 moles H2O * 5.6 moles HNO3) / 6 moles HNO3 = 1.87 moles H2O

Finally, to find the grams of water produced, we can use the molar mass of water which is approximately 18.015 g/mol:

Mass of water = 1.87 moles H2O * 18.015 g/mol = 33.65955 g = 33.7 grams of water

Answer 2

33.63 g H₂O

Step-by-step explanation:

The mole ratio of HNO₃ and H₂O is 6 : 2

Hence, 16.9 moles of HNO₃ will produce = 2/6×5.6 = 1.86 moles of H₂O

Also,

Mass = Moles × M.Mass

Mass = 1.86 mol × 18.02 g/mol

Mass = 33.63 g H₂O