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3 years ago

In which of the three states of matter are the particles moving at the greatest speed?

Chemistry

1 answer:

tekilochka [14]3 years ago

4 0

Answer:

Gas(this is because we are only considering that there are 3 states of matter, while in reality there are 5.)

Explanation:

There are actually 4 states of matter excluding a 5th one that has just been discovered, but if we consider that there are only 3 states of matter then the particles move the fastest in gases. As the particles are the furthest apart.

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If you have a gold coin that contains 0.637 moles of gold, how many grams of gold does it contain?

mario62 [17]

The answer is 5 gold token from Chuck E. Cheese

8 0

3 years ago

A) Combustion analysis of toluene, a common organic solvent, gives 5.86 mg of CO2 and 1.37 mg of H2O. If the compound contains o

Mumz [18]

Answer:

For a: The empirical formula for the given compound is $CH$

For b: The empirical and molecular formula for the given organic compound are $C_{10}H_{20}O$

Explanation:

For a:

The chemical equation for the combustion of hydrocarbon follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

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

We are given:

Conversion factor used: 1 g = 1000 mg

Mass of $CO_2=5.86mg=5.86\times 10^{-3}g$

Mass of $H_2O=1.37mg=1.37\times 10^{-3}g$

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

So, in $5.86\times 10^{-3}g$ of carbon dioxide, $\frac{12}{44}\times 5.86\times 10^{-3}=1.60\times 10^{-3}g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in $1.37\times 10^{-3}g$ of water, $\frac{2}{18}\times 1.37\times 10^{-3}=0.152\times 10^{-3}g$ of hydrogen will be contained.

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

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.60\times 10^{-3}g}{12g/mole}=0.133\times 10^{-3}moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.152\times 10^{-3}g}{1g/mole}=0.152\times 10^{-3}moles$

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 $0.133\times 10^{-3}$ moles.

For Carbon = $\frac{0.133\times 10^{-3}}{0.133\times 10^{-3}}=1$

For Hydrogen = $\frac{0.152\times 10^{-3}}{0.133\times 10^{-3}}=1.14\approx 1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H = 1 : 1

Hence, the empirical formula for the given compound is $CH$

For b:

The chemical equation for the combustion of menthol 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 $CO_2$ = 0.2829 g

Mass of $H_2O$ = 0.1159 g

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

So, in 0.2829 g of carbon dioxide, $\frac{12}{44}\times 0.2829=0.077g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in 0.1159 g of water, $\frac{2}{18}\times 0.1159=0.013g$ of hydrogen will be contained.

Mass of oxygen in the compound = (0.1005) - (0.077 + 0.013) = 0.105 g

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

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.077g}{12g/mole}=0.0064moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.013g}{1g/mole}=0.013moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.0105g}{16g/mole}=0.00065moles$

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 0.00065 moles.

For Carbon = $\frac{0.0064}{0.00065}=9.84\approx 10$

For Hydrogen = $\frac{0.013}{0.00065}=20$

For Oxygen = $\frac{0.00065}{0.00065}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 10 : 20 : 1

The empirical formula for the given compound is $C_{10}H_{20}O$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 156 g/mol

Mass of empirical formula = 156 g/mol

Putting values in above equation, we get:

$n=\frac{156g/mol}{156g/mol}=1$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(1\times 10)}H_{(1\times 20)}O_{(1\times 1)}=C_{10}H_{20}O$

Hence, the empirical and molecular formula for the given organic compound are $C_{10}H_{20}O$

3 0

4 years ago

A certain kind of light has a wavelength of 4.6 micrometers what is the frequency of this light and gigahertz? Use c= 2.998 × 10

Leno4ka [110]

Answer:

6.52×10⁴ GHz

Explanation:

From the question given above, the following data were obtained:

Wavelength (λ) = 4.6 μm

Velocity of light (v) = 2.998×10⁸ m/s

Frequency (f) =?

Next we shall convert 4.6 μm to metre (m). This can be obtained as follow:

1 μm = 1×10¯⁶ m

Therefore,

4.6 μm = 4.6 μm × 1×10¯⁶ m / 1 μm

4.6 μm = 4.6×10¯⁶ m

Next, we shall determine frequency of the light. This can be obtained as follow:

Wavelength (λ) = 4.6×10¯⁶ m

Velocity of light (v) = 2.998×10⁸ m/s

Frequency (f) =?

v = λf

2.998×10⁸ = 4.6×10¯⁶ × f

Divide both side by 4.6×10¯⁶

f = 2.998×10⁸ / 4.6×10¯⁶

f = 6.52×10¹³ Hz

Finally, we shall convert 6.52×10¹³ Hz to gigahertz. This can be obtained as follow:

1 Hz = 1×10¯⁹ GHz

Therefore,

6.52×10¹³ Hz = 6.52×10¹³ Hz × 1×10¯⁹ GHz / 1Hz

6.52×10¹³ Hz = 6.52×10⁴ GHz

Thus, the frequency of the light is 6.52×10⁴ GHz

5 0

3 years ago

How many ozone particles are needed to form 24 particles of oxygen gas?

bearhunter [10]

First, you have to know the chemical formula of ozone and oxygen gas. Oxygen gas is O₂; it is one of the few gases that are diatomic in nature. The chemical formula of ozone is O₃. In oxygen gas, there are 2 particles of the oxygen element, while there are 3 particles for the ozone. There might be a slight difference but this induces a great difference in their properties. Oxygen is essential to living things because this is the gas that we breathe in. However, ozone is not safe to breathe in. It is a very strong oxidizing agent, almost 4 times as strong as the oxygen. Its main function is to block the UV rays from entering the Earth's atmosphere which can be harmful to our health.

Having known their chemical formula and properties, we know that an oxygen gas has 2 particles of oxygen element. So, if there are 24 particles of oxygen gas, that would mean 48 particles of the oxygen element. Since an ozone compound contains 3 particles of the oxygen element, then 48/3 = 16. It would take 16 particles of ozone to form 24 particles of the oxygen gas.

6 0

3 years ago

What is the total amount of work done when Danny lifted 25 pounds of weight over 5 meters and applying 30- Newtons of Force?

MariettaO [177]

Answer:

Definition and Mathematics of Work

Calculating the Amount of Work Done by Forces

Potential Energy

Kinetic Energy

Mechanical Energy

5 0

3 years ago