Find the % composition for each element in Zinc Chlorate

PLEASE SOMEONE HELP ME WITH THIIS QUESTION

sdas [7]

Answer:

The correct answer is - 5 carbon compounds due to low to high intermolecular forces between their molecules.

Explanation:

Bottle C has gas in it and we know that alkane has carbon and hydrogen only which means they have a single sigma bond between them and very low intermolecular forces in between molecules and are present mostly at gaseous state. Thus, bottle C has alkane.

Alcohols have -OH group that can form rarely two pi bonds which means they have intermediate intermolecular force whereas acids have -cooH group with a high molecular force so bottle B with liquid is alcohol and A has acid.

3 0

3 years ago

a sample of gas initially occupies 5.50 liter at a pressure of 0.750 atm at 13.0 C. what will the temperture change to 22.5 C an

sergey [27]

Answer:

The pressure will be 2.84 atm

Explanation:

The gas laws are a set of chemical and physical laws that allow us to determine the behavior of gases in a closed system. The parameters evaluated in these laws are pressure, volume, temperature and moles.

Boyle's law indicates that the volume is inversely proportional to the pressure: if the pressure increases, the volume decreases and if the pressure decreases, the volume increases. Boyle's law is expressed mathematically as:

P * V = k

On the other hand, Charles's law indicates that with increasing temperature, the volume of the gas increases and with decreasing temperature, the volume of the gas decreases. That is, they are directly proportional. This is expressed mathematically as:

$\frac{V}{T} =k$

Finally, the Gay-Lussac law says that at constant volume, the pressure of the gas is directly proportional to its temperature. Mathematically, it is expressed as:

$\frac{P}{T} =k$

Combined law equation is the combination of three gas laws called Boyle's, Charlie's and Gay-Lusac's law:

$\frac{P*V}{T}=k$

When you want to study two different states, an initial and a final one of a gas, you can use the following expression:

$\frac{P1*V1}{T1}=\frac{P2*V2}{T2}$

In this case:

P1= 0.750 atm
V1= 5.50 L
T1= 13 C= 286 K (being 0 C=273 K)
P2=?
V2= 1.50 L
T2= 22.5 C=295.5 K

Replacing:

$\frac{0.750 atm*5.50 L}{286 K}= \frac{P2*1.50 L}{295.5 K}$

Solving:

$P2=\frac{295.5K}{1.50L} *\frac{0.750 atm*5.50 L}{286 K}$

P2= 2.84 atm

<u><em>The pressure will be 2.84 atm</em></u>

8 0

4 years ago

The photo shows an animal called a water flea. Which level of organization is it an example of?

Citrus2011 [14]

Answer:

A. organism i think

8 0

3 years ago

Read 2 more answers

How many grams of copper would have the same number of atoms as 139.82 grams of argon

lianna [129]

Answer:

Lesson 3 Quiz ReturntoAssessmentList Part 1 of 4 - 4.0/ 8.0 Points Question 1 of ... in the balloon containing regular air D.Each balloon has an equal number of atoms. ... The purity of those pre-1982 pennies are really about 95% copper (5% zinc ... that had a mass of 3.11 grams, how many atoms of copper would you have?

Explanation:

7 0

3 years ago

How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The

WARRIOR [948]

Answer:

The answer to the question above is

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C = 29.36 kJ

Explanation:

The given variables are

ΔHfus = 7.27 kJ/mol

Cliq = 2.16 J/g°C

Cgas = 1.29 J/g°C

Csol = 1.65 J/g°C

Tmelting = -95.0°C.

Initial temperature = -154.0°C

Final temperature = -42.0°C?

Mass of acetone = 87.1 g

Molar mass of acetone = 58.08 g/mol

Solution

Heat required to raise the temperature of solid acetone from -154 °C to -95 °C or 59 °C is given by

H = mCsolT = 87.1 g* 1.65 J/g°C* 59 °C = 8479.185 J

Heat required to melt the acetone at -95 °C = ΔHfus*number of moles =

But number of moles = mass÷(molar mass) = 87.1÷58.08 = 1.5

Heat required to melt the acetone at -95 °C =1.5 moles*7.27 kJ/mol = 10.905 kJ

The heat required to raise the temperature to -42 degrees is

H = m*Cliq*T = 87.1 g* 2.16 J/g°C * 53 °C = 9971.21 J

Total heat = 9971.21 J + 10.905 kJ + 8479.185 J = 29355.393 J = 29.36 kJ

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C is 29.36 kJ

4 0

3 years ago