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3 years ago

Please help!!!

Chemistry

1 answer:

Anon25 [30]3 years ago

8 0

Answer:

Never destroyed or created.

Explanation:

Althought your text book may say it is the law of conservation of mass (which correct), it is also the Law of Conservation of matter (Both hold roughly the same meaning). Law of conservation of mass states the mass of the system must remain constant, as system mass cannot change quantity if it is not added or removed over time. Whereas, the law of conservation of energy states that energy cannot be created or destroyed.

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What is the most abundant chemical element in the universe?

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hydrogen is the most

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4 years ago

What role do catalysts play in chemical reactions?

Ludmilka [50]

Role of a catalysts in chemical reactions:
Catalyst is a substance, usually used in small amounts relative to the reactants, that modifies and increases the rate of a reaction without being consumed in the process.

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3 years ago

A 0.1014 g sample of a purified compound containing C, H, and, O was burned in a combustion apparatus and produced 0.1486 g CO2

Alina [70]

Answer: The empirical formula for the given compound is $CH_2O$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=0.1486g$

Mass of $H_2O=0.0609g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 0.1486 g of carbon dioxide, $\frac{12}{44}\times 0.1486=0.0405g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 0.0609 g of water, $\frac{2}{18}\times 0.0609=0.00677$ of hydrogen will be contained.

Mass of oxygen in the compound = (0.1014) - (0.0405 + 0.00677) = 0.054 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.0405g}{12g/mole}=0.003375moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.00677g}{1g/mole}=0.00677moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.054g}{16g/mole}=0.003375moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.485 moles.

For Carbon = $\frac{0.003375}{0.003375}=1$

For Hydrogen = $\frac{0.00677}{0.003375}=2.00\times 2$

For Oxygen = $\frac{0.003375}{0.003375}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1 : 2 : 1

The empirical formula for the given compound is $C_1H_2O_1=CH_2O$

Thus, the empirical formula for the given compound is $CH_2O$

8 0

3 years ago

Help me plz I don’t know what it’s mean

Pavlova-9 [17]

Answer:

1 has the highest density because it has the most amount of circles in the least amount of space- it is the most densely filled with circles; it is the most dense.

4 0

3 years ago

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Given the relative abundance of the following naturally occurring isotopes of oxygen, calculate the average atomic mass of oxyge

STatiana [176]

The average atomic mass of oxygen is 16 amu.

According to the formula of average atomic mass of oxygen

= $\frac{Sum of (Mass of each isotope)(relative abundance)}{100} \\\\= \frac{((16)(99.76)+(17)(0.037)+(18)(0.204)}{100} \\\\=16 amu$

6 0

4 years ago

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