What is the mass of 1.20 x 1024 atoms of potassium?

Answer:

complimentary

Explanation:

Answer:

Proximal

Explanation:

Answer:

the answer is 11.111 and when you round it to the nearest one it’s 11, but to the nearest tenth it’s 10

Explanation:

Answer:

1. Mass percent of ethanol = 28.02 %.

2. Mole fraction of ethanol = 0.13.

Explanation:

1. To find the mass percent we need to use the following equation:

[tex]\%_{m/m} = \frac{m_{e}}{m_{s}} \times 100[/tex]

Where:

[tex]m_{e}[/tex] is the mass of ethanol

[tex]m_{s}[/tex] is the mass of the solution

We need to calculate the mass of ethanol and the mass of the solution:

[tex] d = \frac{m_{s}}{V} [/tex]

Where:

d: is the density of the solution = 0.957 g/mL

V: is the volume = 1 L

[tex] m_{s} = d*V = 0.957 \frac{g}{mL}*\frac{1000 mL}{1 L}*1 L = 957 g [/tex]

Now, from the concentration we can find the mass of ethanol:

[tex] C = \frac{n_{e}}{V} = \frac{m_{e}}{M_{e}*V} [/tex]                      

Where:

[tex]M_{e}[/tex]: is the molar mass of ethanol = 46.07 g/mol

[tex]n_{e}[/tex]: is the number of moles of ethanol = m/M

[tex] m_{e} = C*M*V = 5.82 \frac{mol}{L}*46.07 \frac{g}{mol}*1 L = 268.13 g [/tex]

Finally, the mass percent of ethanol is:

[tex]\%_{m/m} = \frac{268.13 g}{957 g} \times 100 = 28.02 \%[/tex]

2. The mole fraction of ethanol is given by:

[tex] \chi_{e} = \frac{n_{e}}{n_{s}} [/tex]

The number of moles of ethanol is:

[tex]n_{e} = \frac{m_{e}}{M_{e}} = \frac{268.13 g}{46.07 g/mol} = 5.82 moles[/tex]

And the moles of the solution is:    

[tex] n_{s} = n_{e} + n_{w} [/tex]

Where w is for water

[tex] n_{s} = n_{e} + \frac{m_{w}}{M_{w}} [/tex]

[tex] n_{s} = n_{e} + \frac{m_{s} - m_{e}}{M_{w}} [/tex]

[tex]n_{s} = 5.82 moles + \frac{957 g - 268.13 g}{18 g/mol} = 44.09 moles[/tex]

Hence, the mole fraction of ethanol is:

[tex]\chi_{e} =\frac{5.82 moles}{44.09 moles}=0.13[/tex]

I hope it helps you!                                                          

Answer: gas molecules will hit the container walls more frequently and with greater force

Explanation:

According to the postulates of  kinetic molecular theory:

1. The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls.

2. The average kinetic energy of the gas molecules is proportional to the kelvin temperature of the gas.

When the temperature is increased, so the average kinetic energy and the rms speed also increase. This means that the gas molecules will hit the container walls more frequently and with greater force because they are all moving faster. This increase the pressure.

Answer:

Number of moles of Al₂O₃ = 0.45 mol

Explanation:

Given data:

Number of moles of Fe produced = 1.35 mol

Number of moles of Al₂O₃ = ?

Solution:

2Al + 3FeO   →    3Fe + Al₂O₃

now we will compare the moles of iron and  Al₂O₃

              Fe         :           Al₂O₃

               3          :             1

              1.35      :            1/3×1.35 = 0.45 mol

126 g Fe

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

2.25 mol Fe

Step 2: Identify Conversions

Molar Mass of Fe - 55.85 g/mol

Step 3: Convert

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

125.663 g Fe ≈ 126 g Fe

Answer:

Explanation:

C

[tex]4.9 \times 10^{23}[/tex]  are present in 18.4L of argon (Ar).

To calculate the amount of particles present in a given amount of volume, it is necessary to have knowledge of the molar volume:

                                          [tex]1 mol = 22.4L[/tex]

Thus, in 22.4L there is 1 mol of an element, remembering that:

                                   [tex]1 mol = 6\times10^{23}[/tex] particles

In this way, it is enough to relate the value of the molar volume given with the value requested by the question:

                                     [tex]\frac{6\times10^{23}particles}{xparticles} = \frac{22.4L}{18.4L}[/tex]

                                    [tex]x = 4.9 \times 10^{23}[/tex] particles

 So, [tex]4.9 \times 10^{23}[/tex] are present in 18.4L of argon (Ar).

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0.125 mol Ca

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

5.00 g Ca

Step 2: Identify Conversions

Molar mass of Ca - 40.08 g/mol

Step 3: Convert

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

0.12475 mol Ca ≈ 0.125 mol Ca

The molecular formula =C₆H₁₂O₆

Given

6.00 g of a certain compound X

The molecular molar mass of 180. g/mol

CO₂=8.8 g

H₂O=3.6 g

Required

The molecular formula

Solution

mass C in CO₂ :

= 1.12/44 x 8.8

= 2.4 g

mass H in H₂O :

= 2.1/18 x 3.6

= 0.4 g

Mass O in compound :

= 6-(2.4+0.4)

= 3.2 g

Mol ratio C : H : O

= 2.4/12 : 0.4/1 : 3.2/16

= 0.2 : 0.4 : 0.2

= 1 : 2 : 1

The empirical formula : CH₂O

(CH₂O)n=180 g/mol

(12+2+16)n=180

(30)n=180

n=6

(CH₂O)₆=C₆H₁₂O₆

Answer:Prokaryotic cells carry out cellular respiration within the cytoplasm and eukaryotic cells carry out respiration in the mitochondria

Explanation:

Answer:

Invertebrates than eventually everything would die

Answer:

CH4

Explanation:

The ideal gas behavior of individual gases often depend on the magnitude of intermolecular interaction between the molecules of the gas as well as the presence or absence of polar bonds.

In CCl4, there are polar bonds and the presence of the more electronegative chlorine atom in the molecule and consequently a greater degree of intermolecular interaction at 400K compared to CH4 which contains only non polar bonds.

Therefore, CH4 displays greater ideal gas behavior at 400K than CCl4.

Answer:

50.8 g

Explanation:

Equation of reaction.

[tex]CH_4 + 2O_2 \to CO_2 + 2H_2O[/tex]

From the given information, the number of moles of methane = mass/ molar mass

= 15.4 g /  16.04 g/mol

= 0.960 mol

number of moles of oxygen gas = 90.3 g / 32 g/ mol

= 2.82 mol

Since 1 mol of methane requires 2 moles of oxygen

Then 0.960 mol of methane will require = 0.960 mol × 2 = 1.92 mol of oxygen gas

Thus, methane serves as a limiting reagent.

2.82 mol oxygen gas will result in 2.82 moles of water

So, the theoretical yield of water = moles × molar mass

= 2.82 mol × 18.01528 g/mol

= 50.8 g

Answer:

NARUTOOOO

Explanation:

Answer:

C = 107.97 mol/L

Explanation:

Given data:

Volume of solution = 1.38 mL (1.38 mL× 1 L /1000 mL = 0.00138 L)

Mass of ammonium sulfite = 17.36 g

Concentration of solution =?

Solution:

We will calculate the number of moles of ammonium sulfite.

Number of moles = mass/molar mass

Number of moles = 17.36 g / 116.15 g/mol

Number of moles = 0.149 mol

Concentration:

C = n/V

C = concentration

n = number of moles of solute

v = volume in L

C = 0.149 mol / 0.00138 L

C = 107.97 mol/L

Answer:

[tex]V_{HCl}=48.0 mL[/tex]

Explanation:

Hello!

In this case, since the reaction between calcium hydroxide and hydrochloric acid shows a 2:1 mole ratio between them:

[tex]2HCl+Ca(OH)_2\rightarrow CaCl_2+2H_2O[/tex]

We need to use the following mole ratio:

[tex]2n_{Ca(OH)_2}=n_{HCl}[/tex]

That can be written in volumes and concentrations:

[tex]2M_{Ca(OH)_2}V_{Ca(OH)_2}=M_{HCl}V_{HCl}[/tex]

Thus, we solve for the volume of HCl as it is the unknown:

[tex]V_{HCl}=\frac{2M_{Ca(OH)_2}V_{Ca(OH)_2}}{M_{HCl}}[/tex]

Therefore, we plug in to obtain:

[tex]V_{HCl}=\frac{2*0.120M*25.0mL}{0.150M} \\\\V_{HCl}=48.0 mL[/tex]

Best regards!

Answer:

0.0195 g

Explanation:

Ag^+(aq) + e -------> Ag(s)

Since 1 electron was transferred, that means 96500C of electricity was required

108 g is deposited 96500 C

xg is deposited 220 × 10^-3 × 79.0

x = 108 × 220 × 10^-3 × 79.0/96500

x= 19.5 × 10^-3 g

x= 0.0195 g

The air barrier system

Answer:

Density of the oil is lesser than that of the water

Explanation:

The density of water is given as 1.0g/cm³.

  Salad oil is found to float on water, this implies that the density of this salad oil is lesser than that of the water.

Density is the mass per unit volume of a substance.

Answer:

two components of the same thing

Explanation:

The percentage of water in the compound CaSO₄.6H₂O = 44.26%

Given

Compound CaSO₄. 6H₂O

Required

The percentage of water

Solution

MW CaSO₄. 6H₂O :

= 40 + 32 + 4.16 + 12.1 + 6.16

= 244

MW 6H2O :

= 12.1 + 6.16

= 108

%water = (108 : 244) x 100%

%water = 44.26

The percentage of water in the compound CaSO₄.6H₂O is 44.26%

Since MW CaSO₄. 6H₂O :

= 40 + 32 + 4.16 + 12.1 + 6.16

= 244

Now

MW 6H2O :

= 12.1 + 6.16

= 108

So, percentage of water = (108 : 244) x 100%

= 44.26

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Answer:

[tex]C^{2+}[/tex]

Explanation:

When a proton is removed, it changes the whole element. However, when electrons are removed, it becomes an ion. Since we are removing two electrons, we are subtracting a negative number, giving us positive two as our net ionic charge. Therefore, the answer is [tex]C^{2+}[/tex]

Answer: 5.47x10^24 molecules

Explanation:

6.02214076x10^23 molecules CO2 = 44g

400g = (400/44)*6.02214076*10^23 = 5.47x10^24

According to the concept of Avogadro's number, there are 54.75 ×10²³ molecules of carbon dioxide are 400 grams of the substance.

Avogadro's number is defined as a proportionality factor which relates number of constituent particles with the amount of substance which is present in the sample.

It has a SI unit of reciprocal mole whose numeric value is expressed in reciprocal mole which is a dimensionless number and is called as Avogadro's constant.It relates the volume of a substance with it's average volume occupied by one of it's particles .

According to the definitions, Avogadro's number depend on determined value of mass of one atom of those elements.It bridges the gap between macroscopic and microscopic world by relating amount of substance with number of particles.

Number of atoms can be calculated using Avogadro's number as follows: mass/molar mass×Avogadro's number .Number of moles= 400/44=9.09 moles which is number of molecules =9.09×6.023×10²³= 54.75 ×10²³ .

Learn more about Avogadro's number,here:

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147.05 g/mol

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

CuClO₃

Step 2: Find MM

Molar Mass of Cu - 63.55 g/mol

Molar Mass of Cl - 35.45 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of CuClO₃ - 63.55 + 35.45 + 3(16.00) = 147.05 g/mol

Answer:

b.oil

Explanation:

oil is a nonrewnewable resource

Answer:

С3Н6.

Explanation:

Hello!

In this case, since addition reactions imply that a radical or some radicals are added to the parent chain, we notice that only unsaturated hydrocarbons are able to undergo addition whereas saturated ones undergo substitution reactions as they already have all the carbon bonds bonded to leaving groups.

In such a way, we can rule out C2H6, C3H8 and CH4 as they are all alkanes; therefore, only С3Н6 is able to undergo an addition reaction due to the C=C which is able to lose one of those bonds and allow an incoming radical to get included into the parent chain.

Best regards!

Answer: Hydrogen molecules will have greatest average speed.

Explanation:

The formula for average speed is  :

[tex]\mu_{av}={\sqrt{\frac{8RT}{\pi\times M}}}[/tex]

R = gas constant  

T = temperature  

M = Molecular Mass

Now putting all the values:

[tex]\frac{\nu_{H_2}}{\nu_{O_2}}=\sqrt{\frac{8RT}{\pi\times M_{H_2}}}/{\sqrt{\frac{8RT}{\pi\times M_{O_2}}}[/tex]

[tex]\frac{\nu_{H_2}}{\nu_{O_2}}=\sqrt{\frac{16}{2}}[/tex]

[tex]\frac{\nu_{av}_{H_2}}{\nu_{av}_{O_2}}=8[/tex]

Thus average speed of hydrogen is 8 times the average speed of oxygen. Thus hydrogen molecules will have greatest average speed

Answer:

No. of moles, n = 7.52 moles

Explanation:

Given that,

Mass, m = 563.9 grams

Molar mass of arsenic = 74.92 g/mol

We need to find the number of moles in 563.9 grams of arsenic. Let it is denoted by n. It is equal to given mass divided by total molar mass.

[tex]n=\dfrac{563.9 }{74.92}\\\\=7.52\ \text{moles}[/tex]

So, there are 7.52 moles in 563.9 grams of arsenic.