arrange the following in order of increasing mass . a. 16 water molecules b. 2 atoms of lead 3. 5.1*10^-23

What type of energy has caused the fewest deaths per unit of energy produced?

mash [69]

Answer: Nuclear energy is by far the safest energy source in this comparison – it results in more than 442 times fewer deaths than the 'dirtiest' forms of coal; 330 times fewer than coal; 250 times less than oil; and 38 times fewer than gas.

4 0

3 years ago

What is most likely oxidation state of aluminum (AI)?

blagie [28]

Aluminum has three oxidation states. The most common one is +3. The other two are +1 and +2. One +3 oxidation state for Aluminum can be found in the compound aluminum oxide, Al2O3.

7 0

3 years ago

Nicotine is 74.1% carbon, 8.6% hydrogen, and 17.3% nitrogen by mass. What is its molecular formula if its molar mass is 162.26 g

WINSTONCH [101]

first we need to find the empirical formula of nicotine

empirical formula is the simplest ratio of whole numbers of elements making up a compound

the percentage compositions for each element has been given. So we can calculate for 100 g of the compound.

masses of elements and the number of moles

C - 74.1 g - 74.1 g/12 g/mol = 6.17 mol

H - 8.6 g - 8.6 g / 1 g/mol = 8.6 mol

N - 17.3 g - 17.3 g / 14 g/mol = 1.23

divide all by the least number of moles

C - 6.17 / 1.23 = 5.01

H - 8.6 / 1.23 = 6.99

N - 1.23 / 1.23 = 1.00

when the atoms are rounded off to the nearest whole numbers

C - 5

H - 7

N - 1

empirical formula is C₅H₇N

we have to find what the mass of 1 empirical unit is

mass - 5 x 12 g/mol + 7 x 1 g/mol + 14 g/mol = 81 g

molecular mass is 162.26 g/mol

we have to find how many empirical units make up 1 molecule

number of empirical units = molecular mass / mass of 1 empirical unit

= 162.26 g/mol / 81 g = 2.00

there are 2 empirical units

molecular formula is - 2 (C₅H₇N)

molecular formula - C₁₀H₁₄N₂

4 0

3 years ago

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PLEASE ANSWER CORRECTLY !!!!!!!!!!!!!! WILL MARK BRAINLIEST !!!!!!!!!!!!!!

geniusboy [140]

Answer:

the ice has reached its melting point

the water has reached its freezing point

the whatever that is has reached its cooling point I guess

8 0

3 years ago

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A 14.60g sample of an unknown compound, composed only of carbon, hydrogen, and oxygen, produced 28.6g of CO2 and 14.6g of H2O in

o-na [289]

Answer: The empirical formula for the given compound is $C_{2}H_{5}O$

Explanation:

The chemical equation for the combustion of compound 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 $CO_2=28.6g$

Mass of $H_2O=14.6g$

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 28.6 g of carbon dioxide, $\frac{12}{44}\times 28.6=7.8g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in 14.6 g of water, $\frac{2}{18}\times 14.6=1.6$ of hydrogen will be contained.

For calculating the mass of oxygen:

Mass of oxygen in the compound = (14.60) - (7.8 + 1.6) = 5.2 g

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

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{7.8g}{12g/mole}=0.65moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.6g}{1g/mole}=1.6moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{5.2g}{16g/mole}=0.32moles$

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 0.32 moles.

For Carbon = $\frac{0.65}{0.32}=2.03\approx 2$

For Hydrogen = $\frac{1.6}{0.32}=5$

For Oxygen = $\frac{0.32}{0.32}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 2 : 5 : 1

Hence, the empirical formula for the given compound is $C_{2}H_{5}O_{1}=C_{2}H_{5}O$

8 0

3 years ago

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arrange the following in order of increasing mass . a. 16 water molecules b. 2 atoms of lead 3. 5.1*10^-23​

arrange the following in order of increasing mass . a. 16 water molecules b. 2 atoms of lead 3. 5.1*10^-23