According to the text, fission occurs when the nucleus
two lighter nuclei.

Answer:

Solvent, less polar molecule, more polar molecule, silica gel

Explanation:

Solvent has lowest polarity but less polar molecule has more polarity than solvent. The more polar molecule has higher polarity value whereas silica gel has the highest polarity. The polarity of compounds is due to the difference of electronegativity values of the elements that bonded with each other. The difference of electronegativity value is high between silicon and oxygen is responsible for high polarity of silica gel.

Answer:

what are you confused on?

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Answer: 3.98 x 10^-7

Explanation:

I hope this helped!

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Answer: The formula of the hydrate is [tex]MnSO_4.2H_2O[/tex]

Explanation:

Decomposition of hydrated manganese sulphate is given by:

[tex]MnSO_4.xH_2O\rightarrow MnSO_4+xH_2O[/tex]

Molar mass of [tex]MnSO_4[/tex] = 151.0 g/mol

According to stoichiometry:

(151.0+18x) g of [tex]MnSO_4.xH_2O[/tex] decomposes to give 151.0 g of [tex]MnSO_4[/tex]

Thus 45.91 g of [tex]MnSO_4.xH_2O[/tex] decomposes to give= [tex]\frac{ 151.0}{151.0+18x}\times 45.91g[/tex]  of [tex]MnSO_4[/tex]

Also we are given : 37.07 g of  [tex]MnSO_4[/tex] is produced

Thus we can equate the two equations:

[tex]\frac{ 151.0}{151.0+18x}\times 45.91=37.07[/tex]

[tex]x=2[/tex]  

Thus the formula of the hydrate is [tex]MnSO_4.2H_2O[/tex]

Answer: True

Explanation:

Answer:

Heat is the process of something getting hot(temperatures going up). Cold is when something gets cold(temperature decreases).

Explanation:

Answer:

I think A is the correct answer

Answer: the answer is B 100%

A

because both have 2's in front of them

Answer:

0.612 J/g°C

Explanation:

Using the formula as follows:

Q = m × c × ∆T

Where;

Q = amount of heat (Joules)

m = mass of substance (g)

c = specific heat capacity (J/g°C)

∆T = change in temperature (°C) i.e. final - initial temperature

According to the information provided in this question;

Q = 577 J

m = 32.3 g

c = ?

Final temp = 46.6ºC, initial temp. = 17.4°C

∆T = (46.6 - 17.4) = 29.2°C

Using Q = m × c × ∆T

c = Q ÷ m.∆T

c = 577 ÷ (32.3 × 29.2)

c = 577 ÷ 943.16

c = 0.6117

c = 0.612 J/g°C

Answer:

1 mol Li₂O₂/mol CO₂ or 1 mol CO₂/mol Li₂O₂

2 mol Li₂CO₃/mol O₂ or 1 mol O₂/2 mol Li₂CO₃

1 mol Li₂O₂/mol Li₂CO₃ or 1 mol Li₂CO₃/mol Li₂O₂

2 mol Li₂O₂/mol O₂ or 1 mol O₂/2 mol Li₂O₂

1 mol CO₂/mol Li₂CO₃ or 1 mol Li₂CO₃/mol CO₂

2 mol CO₂/mol O₂ or 1 mol O₂/2 mol CO₂

Explanation:

The balanced chemical equation is:

2 Li₂O₂ + 2 CO₂ → 2 Li₂CO₃ + O₂

The mole-to-mole relationships are provided by the chemical stoichiometric coefficients (2 for Li₂O₂, 2 for CO₂, 2 for Li₂CO₃ and 1 for O₂).

We have to relate the moles of 1 compound to the moles of another compound in the equation. So, we can start writing the relationships between reactants (Li₂O₂ and CO₂)

2 moles of Li₂O₂ react with 2 moles of CO₂ → 2 mol Li₂O₂/2 mol CO₂= 1 mol Li₂O₂/mol CO₂ or 1 mol CO₂/mol Li₂O₂

Now, the relationships between products (Li₂CO₃ and O₂):

2 moles of Li₂CO₃ are produced when 1 mol of O₂ produced → 2 mol Li₂CO₃/1 mol O₂= 2 mol Li₂CO₃/mol O₂ or 1 mol O₂/2 mol Li₂CO₃

Finally, between reactants and products:

2 moles of Li₂O₂ produce 2 moles of Li₂CO₃ → 2 mol Li₂O₂/2 mol Li₂CO₃= 1 mol Li₂O₂/mol Li₂CO₃ or 1 mol Li₂CO₃/mol Li₂O₂

2 moles of Li₂O₂ produce 1 mol of O₂ → 2 mol Li₂O₂/1 mol O₂= 2 mol Li₂O₂/mol O₂ or 1 mol O₂/2 mol Li₂O₂

2 moles of CO₂ produce 2 moles of Li₂CO₃ → 2 mol CO₂/2 mol Li₂CO₃= 1 mol CO₂/mol Li₂CO₃ or 1 mol Li₂CO₃/mol CO₂

2 moles of CO₂ produce 1 mol of O₂ → 2 mol CO₂/1 mol O₂= 2 mol CO₂/mol O₂ or 1 mol O₂/2 mol CO₂

Answer:

6.3*10^-11

no reasoning i just know thats the answer you dont have to trust me.

Answer:

The total pressure of the gas mixture = 2.76 atm

Note: The question is not complete. The complete question is as follow:

If 43.1 g of O2 and 6.8 g of CO2 are placed in a 13.7 L container at 34 degree Celsius , what is the pressure of the mixture of gases?

Explanation:

Mass of O₂ gas = 43.1 g, molar mass of O₂ gas = 32.0 g/mol

Number of moles of O₂ gas = 43.1/32.0 = 1.347 moles

Mass of CO₂ gas = 6.8 g, molar mass of CO₂ gas = 44.0 g

Number of moles of CO₂ gas = 6.8/44 = 0.155 moles

Total number of moles of gas mixture, n = (1.347 + 0.155) = 1.502 moles

Volume of gas mixture, V = 13.7 L

Temperature of gas mixture, T = 34 °C = (273.15 + 34) K = 307.15 K

Pressure of gas mixture = ?

Molar gas constant, R = 0.0821 liter·atm/mol·K.

Using the ideal gas equation: PV =nRT

P = nRT/V

P = (1.502 × 0.0821 × 307.15) / 13.7

P = 2.76 atm

Therefore, the total pressure of the gas mixture = 2.76 atm

Answer:

B

Explanation:

The solubility depends on the ksp. As the value of ksp increases the compound becomes more and more soluble.

In the options, the highest ksp value is 10^-10, thus that one is the most soluble.

Answer:

the answer is B if one mol contains of NH4NO3 contains 6.02X 10^23

Answer:

pollution causes smog

Smoke fog, or smog for short, is a type of intense air pollution.

it makes GHG wich is greenhouse gas and it makes the smog to stay inside the earth wich heats the Earth and it causes flood, storm, tornadoes, ect.

Answer:

Borax is a natural mineral with a chemical formula Na2B4O7 • 10H2O. Borax also is known as sodium borate, sodium tetraborate, or disodium tetraborate. It is one of the most important boron compounds. The International Union of Pure and Applied Chemistry (IUPAC) name for borax is sodium tetraborate decahydrate.

Answer:

Gill Slits

Explanation:

For the one who asked what hind limbs are they are back legs :)

Answer:

ik this isnt the answer but mathwa will solve all yours problems

Explanation:

I think it would be d bc water is everywhere

Answer:

You can tell them on April Fools and if they reject you just say April Fools.

Answer: if u do it on text just say oh wrong person or something I’m not sure

Explanation:

Answer:

hi

Explanation:

i am smart but i need this app cuz some are realy hard

Answer:

6.761 × 10⁴ g

Explanation:

Step 1: Write the balanced combustion reaction

2 C₂H₂ + 5 O₂ ⇒ 4 CO₂ + 2 H₂O

Step 2: Calculate the moles corresponding to 20000 g of C₂H₂

The molar mass of C₂H₂ is 26.038 g/mol.

20000 g × 1 mol/26.038 g = 768.11 mol

Step 3: Calculate the moles of CO₂ produced from 768.11 moles of C₂H₂

The molar ratio of C₂H₂ to CO₂ is 2:4.

768.11 mol C₂H₂ ×  4 mol CO₂/2 mol C₂H₂ = 1536.2 mol CO₂

Step 4: Calculate the mass corresponding to 1536.2 moles of CO₂

The molar mass of CO₂ is 44.01 g/mol.

1536.2 mol × 44.01 g/mol = 6.761 × 10⁴ g

Answer:  60.7 g of [tex]PH_3[/tex] will be formed.

Explanation:

To calculate the moles :

[tex]\text{Moles of solute}=\frac{\text{given volume}}{\text{Molar volume}}[/tex]    

[tex]\text{Moles of} H_2=\frac{60L}{22.4L}=2.68moles[/tex]

The balanced chemical reaction is

[tex]P_4(s)+6H_2(g)\rightarrow 4PH_3(g)[/tex]

[tex]H_2[/tex] is the limiting reagent as it limits the formation of product and [tex]P_4[/tex] is the excess reagent.

According to stoichiometry :

6 moles of [tex]H_2[/tex] produce = 4 moles of [tex]PH_3[/tex]

Thus 2.68 moles of [tex]H_2[/tex] will produce=[tex]\frac{4}{6}\times 2.68=1.79moles[/tex]  of [tex]PH_3[/tex]

Mass of [tex]PH_3=moles\times {\text {Molar mass}}=1.79moles\times 33.9g/mol=60.7g[/tex]

Thus 60.7 g of [tex]PH_3[/tex] will be formed by reactiong 60 L of hydrogen gas with an excess of [tex]P_4[/tex]