Answered

Westonci.ca connects you with experts who provide insightful answers to your questions. Join us today and start learning! Join our Q&A platform to get precise answers from experts in diverse fields and enhance your understanding. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.

Interpret the equation for the formation of water from its elements in terms of the numbers of molecules, moles, and volumes of gases at STP.

[tex]
2 H_2(g) + O_2(g) \rightarrow 2 H_2O(g)
[/tex]

Sagot :

GinnyAnswer
Absolutely, let's delve into the given balanced chemical equation for the formation of water from hydrogen and oxygen:

[tex]\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \][/tex]

We'll interpret this equation in terms of numbers of molecules, moles, and volumes of gases at Standard Temperature and Pressure (STP).

### Numbers of Molecules

First, consider the number of individual molecules:

1. Reactants:
- [tex]\(2\)[/tex] molecules of [tex]\(H_2\)[/tex]
- [tex]\(1\)[/tex] molecule of [tex]\(O_2\)[/tex]

2. Products:
- [tex]\(2\)[/tex] molecules of [tex]\(H_2O\)[/tex]

So, the reaction indicates that 2 molecules of hydrogen gas ([tex]\(H_2\)[/tex]) react with 1 molecule of oxygen gas ([tex]\(O_2\)[/tex]) to form 2 molecules of water ([tex]\(H_2O\)[/tex]).

### Moles

Next, let's talk about moles. The coefficients in a balanced chemical equation also represent the ratios of the substances in moles:

1. Reactants:
- [tex]\(2\)[/tex] moles of [tex]\(H_2\)[/tex]
- [tex]\(1\)[/tex] mole of [tex]\(O_2\)[/tex]

2. Products:
- [tex]\(2\)[/tex] moles of [tex]\(H_2O\)[/tex]

Thus, in this reaction, 2 moles of hydrogen gas ([tex]\(H_2\)[/tex]) react with 1 mole of oxygen gas ([tex]\(O_2\)[/tex]) to produce 2 moles of water ([tex]\(H_2O\)[/tex]).

### Volumes of Gases at STP

At STP (Standard Temperature and Pressure), 1 mole of any gas occupies [tex]\(22.4\)[/tex] liters. Thus, we can calculate the volume of each gas involved in the reaction:

1. Reactants:
- Volume of [tex]\(H_2\)[/tex]: [tex]\(2 \text{ moles} \times 22.4 \text{ liters/mole} = 44.8\)[/tex] liters
- Volume of [tex]\(O_2\)[/tex]: [tex]\(1 \text{ mole} \times 22.4 \text{ liters/mole} = 22.4\)[/tex] liters

2. Products:
- Volume of [tex]\(H_2O\)[/tex]: [tex]\(2 \text{ moles} \times 22.4 \text{ liters/mole} = 44.8\)[/tex] liters

Therefore, according to the equation, 44.8 liters of hydrogen gas ([tex]\(H_2\)[/tex]) react with 22.4 liters of oxygen gas ([tex]\(O_2\)[/tex]) to produce 44.8 liters of water vapor ([tex]\(H_2O\)[/tex]) at STP.

This interpretation comprehensively covers the molecule counts, moles, and gas volumes at standard conditions, aligning with the balanced chemical equation provided.
Thanks for using our service. We're always here to provide accurate and up-to-date answers to all your queries. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Westonci.ca is your go-to source for reliable answers. Return soon for more expert insights.