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3 years ago

6

What is the average atomic mass of a sample of naturally occurring x, if it is comprised of the following isotopes 47% ^51X, 17%

^52X and 36% ^56X

1 answer:

iogann1982 [59]3 years ago

8 0

What your going to do is take away the lowest number form the highest and subtract. Thats your answer...

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Why does 5060 have three significant figures?

Morgarella [4.7K]

<h2>5060 have three significant figures : Explanation given below </h2>

Explanation:

Significant figures

The significant figures (also known as the significant digits and decimal places) of a number are digits that possess certain meaning .

It includes all digits except: zeros

Rules to find significant figures

1.All non-zero digits are considered significant. For example, 23 has two significant figures.

2.Zeros in between two non-zero digits are significant: like in 202.1201 has seven significant figures.

3.Zeros to the left of the significant figures are not significant. For example, .000021 has two significant figures, zeros have no value .

4.Zeros to the right of the significant figures are significant.

That is the reason in number 5060 , it has 3 significant figures .

3 0

2 years ago

How many oxygen atoms are in<br> Ba(MnO4)2?

vlabodo [156]

Answer:

4

Explanation:

5 0

1 year ago

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Write the balanced reaction using the fewest whole number coefficients to describe the reaction between gaseous hydrogen and gas

Anastasy [175]

<u>Answer:</u> The percentage yield of water is 9.5 %

<u>Explanation:</u>

We are given:

Moles of hydrogen = 14 moles

Moles of oxygen = 10 moles

The chemical equation for the formation of water from hydrogen and oxygen follows:

$2H_2+O_2\rightarrow 2H_2O$

By Stoichiometry of the reaction:

2 moles of hydrogen gas reacts with 1 mole of oxygen gas

So, 14 moles of hydrogen gas will react with = $\frac{1}{2}\times 14=7mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent

Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of hydrogen gas produces 2 moles of water

So, 14 moles of hydrogen gas will produce = $\frac{1}{2}\times 14=7mol$ of water

To calculate the percentage yield of water, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of water = 1.33 moles

Theoretical yield of water = 14 moles

Putting values in above equation, we get:

$\%\text{ yield of water}=\frac{1.33mol}{14mol}\times 100\\\\\% \text{yield of water}=9.5\%$

Hence, the percent yield of the water is 9.5 %.

7 0

2 years ago

For the reaction KClO2⟶KCl+O2 KClO2⟶KCl+O2 assign oxidation numbers to each element on each side of the equation. K in KClO2:K i

frosja888 [35]

Answer:

Explanation:

The formula of the reaction:

KClO₂ → KCl + O₂

To assign oxidation numbers, we have to obey some rules:

Elements in an uncombined state or one whose atoms combine with one another to form molecules have an oxidation number of zero.
The charge on simple ions signifies their oxidation number.
The algebraic sum of all the oxidation number of all atoms in a neutral compound is zero. For radicals with charges, their oxidation number is the charge.

The oxidation number of K in KClO₂:

K + (-1) + 2(-2) = 0

K-5 = 0

K = +5

The oxidation number of K in KCl:

K + (-1) = 0

K = +1

The oxidation number Cl in KClO₂ is -1

For Cl in KCl, the oxidation number is -1

For O in KClO₂, the oxidation number is (2 x -2) = -4

For O in O₂, the oxidation number is 0

K moves from an oxidation state of +5 to +1. This is a gain of electrons and K has undergone reduction. We then say K is reduced.

O moves from an oxidation state of -4 to 0. This is a loss of electrons and O has undergone oxidation. We say O is oxidized.

7 0

2 years ago

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Luciana explains to Eric how electricity flows in a circuit. Which sentences are a part of her explanation? Select all that appl

Flauer [41]

I’m pretty sure it c hope that helped

8 0

3 years ago

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