Question

According to the Law of Definite Proportions, under which conditions will water be 11% hydrogen and 89% oxygen by mass?

a) When the water is under a lot of pressure
b) When it is liquid water
c) Any pure sample of water, regardless of phase or source, will be 11% hydrogen and 89% oxygen by mass
d) After it has been freshly reacted from hydrogen and oxygen gas

Answer 1

The correct answer to the question is: c) Any pure sample of water, regardless of phase or source, will be 11% hydrogen and 89% oxygen by mass, though the actual figures are slightly more precise: 11.2% hydrogen and 88.8% oxygen by mass.Water will always be 11.2% hydrogen and 88.8% oxygen by mass according to the Law of Definite Proportions, regardless of its phase, source, or how it was prepared.

Step-by-step explanation:

According to the Law of Definite Proportions, any pure sample of water, regardless of phase or source, will always consist of 88.8% oxygen by mass and 11.2% hydrogen by mass. This fundamental law of chemistry posits that a given chemical compound always contains exactly the same proportion of elements by mass. So in the case of water, this proportion does not change whether it is under high pressure, it's in a liquid state, just freshly reacted from hydrogen and oxygen gas, or found naturally. Different methods of preparation or different states, be it ice, liquid, or vapor, do not affect this composition.

The correct answer to the question is: c) Any pure sample of water, regardless of phase or source, will be 11% hydrogen and 89% oxygen by mass, though the actual figures are slightly more precise: 11.2% hydrogen and 88.8% oxygen by mass.