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4 years ago

Water (h20) is composed of the same element as hydrogen peroxide (h202) how do their properties compare?

Chemistry

2 answers:

kenny6666 [7]4 years ago

8 0

Your answer is: <span>They have different properties because the arrangement of atoms is different.</span>

RSB [31]4 years ago

5 0

The formation of compound takes place by the combination of two or more different atoms. The combination of atoms takes place in a definite proportions. Compounds with different proportions of atoms have different properties.

Water ( $H_2O$ ) is composed of the same element as hydrogen peroxide ( $H_2O_2$ ) that is hydrogen ( $H$ ) and oxygen ( $O$ ). The combination of hydrogen and oxygen atoms in water is in $1:2$ ratio whereas the combination of hydrogen and oxygen atoms in hydrogen peroxide is in $2:2$ ratio. So, the properties of water and hydrogen peroxide are different as the arrangement of atoms is different in the compound.

Hence, the correct option is they have different properties because the arrangement of atoms is different.

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3 years ago

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3 years ago

2. How do chemical reactions involve energy?

Vesnalui [34]

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3 years ago

Question 5 of 10

djyliett [7]

A. A diagram showing the effects of temperature and pressure on phase

Explanation:

A phase diagram is a diagram that shows the effects of temperature and pressure on phase.

A phase diagram shows how different substances are transformed from one form to another.
The transformation is an interplay between pressure and temperature.
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Phase change brainly.com/question/1875234

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3 years ago

When 7.085 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.71 grams of CO2 and 10.37 grams of H

Taya2010 [7]

Answer:

- Empirical:

$C_3H_7$

- Molecular:

$C_6H_{14}$

Explanation:

Hello,

In this case, based on the information regarding the combustion, the moles of carbon turn out:

$n_C=21.71gCO_2*\frac{1molCO_2}{44gCO_2}*\frac{1molC}{1molCO_2}=0.493molC$

Moreover, the moles of hydrogen:

$n_H=10.37gH_2O*\frac{1molH_2O}{18gH_2O}*\frac{2molH}{1molH_2O}=1.152molH$

Thus, the subscripts of carbon and hydrogen in the hydrocarbon turn out:

$C=\frac{0.4934}{0.4934}=1\\H=\frac{1.15222}{0.4934}=2.335\\CH_{2.335}$

Now, looking for a suitable whole number we obtain the following empirical formula as 2.335 times 3 is 7 for hydrogen:

$C_3H_7$

In such a way, that compound has a molar mass of 43 g/mol, thus, the whole compound's molar mass is 86.18 g/mol for which the molecular formula is twice the empirical one, therefore:

$C_6H_{14}$

Which is hexane.

Best regards.

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4 years ago