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2 years ago

1. What is the oxidation number of sulphur in Na2S2O8 A-9 B. -7 C. +7 D. +14

Chemistry

1 answer:

butalik [34]2 years ago

6 0

Answer:

<h2>Hereis the correct answer </h2>

(A.-9)

Explanation:

<h3>STUDY CORRECTION. </h3>

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If star a appears to move back and forth by a greater amount than star b, which star is closer to you?

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If Star A appears to move back and forth by a greater amount than Star B, which star do you think is actually closer to you? Star A. If the parallax angle for a star is 1 arcsecond, what is the distance from the Sun to that star

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2 years ago

Define the term. Theory

Sonja [21]

Answer:

a supposition or a system of ideas intended to explain something, especially one based on general principles independent of the thing to be explained.

(from goo gle)

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3 years ago

Is iced tea with no ice a homogenuous or a heterogenuous mixture? ...?

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It is a homogeneous mixture because you cannot see the individual components that make up the iced tea (such as the water, the molecules found in the tea leaves, etc.). Iced tea with ice in it is considered a heterogeneous mixture because you can distinguish the tea from the ice.

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2 years ago

Which of the following statements is true?

AlekseyPX

Answer:

Explanation:

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2 years ago

4. Magnesium and oxygen undergo a chemical reaction to

erastovalidia [21]

Answer:

About 16.1 grams of oxygen gas.

Explanation:

The reaction between magnesium and oxygen can be described by the equation:
$\displaystyle 2\text{Mg} + \text{O$_2$} \longrightarrow 2\text{MgO}$

24.4 grams of Mg reacted with O₂ to produce 40.5 grams of MgO. We want to determine the mass of O₂ in the chemical change.

Compute using stoichiometry. From the equation, we know that two moles of MgO is produced from every one mole of O₂. Therefore, we can:

Convert grams of MgO to moles of MgO.
Moles of MgO to moles of O₂
And moles of O₂ to grams of O₂.

The molecular weights of MgO and O₂ are 40.31 g/mol and 32.00 g/mol, respectively.

Dimensional analysis:

$\displaystyle 40.5\text{ g MgO} \cdot \frac{1\text{ mol MgO}}{40.31\text{ g MgO}} \cdot \frac{1\text{ mol O$_2$}}{2\text{ mol MgO}} \cdot \frac{32.00\text{ g O$_2$}}{1\text{ mol O$_2$}} = 16.1\text{ g O$_2$}$

In conclusion, about 16.1 grams of oxygen gas was reacted.

You will obtain the same result if you compute with the 24.4 grams of Mg instead:

$\displaystyle 24.4\text{ g Mg}\cdot \frac{1\text{ mol Mg}}{24.31\text{ g Mg}} \cdot \frac{1\text{ mol O$_2$}}{1\text{ mol Mg}} \cdot \frac{32.00\text{ g O$_2$}}{1\text{ mol O$_2$}} = 16.1\text{ g O$_2$}$

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2 years ago