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3 years ago

Seans formula did not have any atmos of oxygen

Chemistry

1 answer:

Dafna1 [17]3 years ago

8 0

What are you asking???? If the formula had no atoms of oxygen then......

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3 years ago

What is the smallest particle of an element?

RideAnS [48]

The smallest is an atom

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3 years ago

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Zina [86]

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3 years ago

How many moles of O2 will be formed from 1.65 moles of KCIO3? (2KClO3–>2KCl + 3O2)

Oduvanchick [21]

Answer:

2.475 mol of O2 formed.

Explanation:

Given 1.65 moles of KClO3 as the target amount in the reactant, used the coefficient of the balanced chemical reaction involved to determine the number of moles of O2 molecules formed.

x mole of O2 = 1.65 mol KClO3 x [(3 mol O2)/ (2 mol KClO3)] = 2.475 mol of O2

x mole of O2 formed = 2.475 mol of O2

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4 years ago

Suppose that two hydroxides, MOH and

kvasek [131]

This problem is providing us with the solubility product of two hydroxides, which can be used to calculate the pH at which they will precipitate. At the end, the answer turns out to be 9.67.

<h3>Solubility product:</h3>

In chemistry, we use solubility products in order to quantify the amount of precipitate a solid will be leftover after dissolving it. Thus, we can just write the equilibrium expressions and solve for x, molar solubility, for each hydroxide as follows:

$Ksp=[M^+][OH ^-]\\\\2.15x10^{-12}=(0.001+x)(x)\\\\x=2.15x10 ^{-9}M\\\\Ksp=[M^2^+][OH ^-]^2\\\\2.15x10^{-12}=(0.001+x)(x)^2\\\\x=4.535x10 ^{-5}M\\\\$

Then, since both x's contribute to the concentration of hydroxide ions, but just the second one is predominant, we add them together to get the total:

$[OH^-]=4.535x10^{-5}M+2.15x10^{-9}M=4.535x10^{-5}M$

Finally, we calculate the pOH and pH with:

$pOH=-log(4.535x10^{-5})=4.343\\\\pH=14-pOH=9.67$

Learn more about solubility product: brainly.com/question/1163248

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3 years ago