Question

S + 6 HNO3 H₂SO4 +6 NO₂ + 2 H₂O

In the above equation, how many grams of water can be made when 2.5 moles of HNO3 are consumed?
Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer
as 4.0
Use the following molar masses. If you do not use these masses, the computer will mark your
answer incorrect.:
Element
Molar
Mass
Hydrogen 1
Nitrogen 14
Sulfur
32
Oxygen 16

Answer 1

15.0 grams of water are produced.

Step-by-step explanation:

The balanced chemical equation is:

S + 6 HNO3 → H2SO4 + 6 NO2 + 2 H2O

According to the equation, for every 6 moles of HNO3 consumed, 2 moles of water are produced. Therefore, we can set up a proportion to find the number of moles of water produced when 2.5 moles of HNO3 are consumed:

6 mol HNO3 : 2 mol H2O = 2.5 mol HNO3 : x mol H2O

where x is the number of moles of water produced.

Solving for x, we get:

x = (2.5 mol HNO3 × 2 mol H2O) / 6 mol HNO3

x = 0.8333 mol H2O

To convert moles of water to grams, we can use the molar mass of water, which is 18.015 g/mol:

0.8333 mol H2O × 18.015 g/mol = 15.01 g H2O

Rounding to the nearest tenth, we get:

15.0 g H2O

Therefore, when 2.5 moles of HNO3 are consumed, 15.0 grams of water are produced.