# Question b960d

Jun 17, 2017

You must use 8.28 g of water.

#### Explanation:

M_text(r):color(white)(mmmmll)18.02color(white)(mml)"63.01#
$\textcolor{w h i t e}{m m m} \text{3NO"_2 + "H"_2"O" → "2HNO"_3 + "NO}$

Calculate the moles of ${\text{HNO}}_{3}$

${\text{Moles of HNO"_3 = 57.9 color(red)(cancel(color(black)("g HNO"_3))) × ("1 mol HNO"_3)/(63.01 color(red)(cancel(color(black)("g HNO"_3)))) = "0.9189 mol HNO}}_{3}$

Calculate the moles of $\text{H"_2"O}$

$\text{Moles of H"_2"O" = 0.9189 color(red)(cancel(color(black)("mol HNO"_3))) × ("1 mol H"_2"O")/(2 color(red)(cancel(color(black)("mol HNO"_3)))) = "0.4595 mol H"_2"O}$

Calculate the mass of $\text{H"_2"O}$

$\text{Mass of H"_2"O" = 0.4595 color(red)(cancel(color(black)("mol H"_2"O"))) × ("18.02 g H"_2"O")/(1 color(red)(cancel(color(black)("mol H"_2"O")))) = "8.28 g H"_2"O}$