. In the decomposition of liquid water (D=0.997 g/mL), what volume of water is needed to produce 3.25 moles of hydrogen gas?

58.7 mL of liquid water are needed

Explanation:

We begin from the decomposition of water's equation:

2H₂O (l) → 2H₂(g) + O₂(g)

Ratio is 2:2. Therefore, 2 moles of hydrogen are produced in the decomposition of 2 moles of water. If we have produced 3.25 moles of H₂ it means that we used the same amount of water → 3.25 moles

We convert the moles to mass, to find the volume with density:

3.25 mol . 18 g / 1mol = 58.5 g

Density = mass / volume → Water density = Water mass / Water volume

Water volume = Water mass / Water density → 58.5 g / 0.997 g/mL =

58.7 mL

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer