Which aqueous solution is colored?1.
CuSO4(aq)
2.
BaCl2(aq)
3.
KCl(aq)
4.
MgSO4(aq)

Answer:

C

Explanation:

polar has unequal sharing of electrons that has the lone pairs which has the electronegativity difference. can be mixed with water.

Final answer:

The combination of polar bleach and polar water would likely be most miscible with each other as substances with similar molecular structures and polarities tend to mix. This is based on the rule of 'like dissolves like' in chemistry.

Explanation:

The question is asking which combination of substances would be most likely to mix, or be miscible, in one another. Miscibility is a property in chemistry relating to whether different substances can combine into a homogeneous mixture without separating.

The rule of thumb in chemistry is 'like dissolves like' which means that substances with similar molecular structures and polarities tend to be miscible with each other. Therefore, among the provided options, the combination of polar bleach and polar water (Option C) would be the most likely to mix with each other as they are both polar substances.

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In the periodic table,the The +3 oxidation state is characteristic of the actinides. All actinides are radioactive.The actinides are silvery and chemically reactive.

What is periodic table?

Periodic table is a tabular arrangement of elements in the form of a table. In the periodic table, elements are arranged according to the modern periodic law which states that the properties of elements are a periodic function of their atomic numbers.

It is called as periodic because properties repeat after regular intervals of atomic numbers . It is a tabular arrangement consisting of seven horizontal rows called periods and eighteen vertical columns called groups.

Elements present in the same group have same number of valence electrons and hence have similar properties while elements present in the same period show gradual variation in properties due to addition of one electron for each successive element in a period.

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Answer:

The +3 oxidation state is characteristic of the actinides.

All actinides are radioactive.

Cerium (Ce) rnakes 100th in abundance (by mass %).

The actinides are silvery and chemically reactive.

If there is direct variation and y=75 when x=25,when y=48 X = 16. Therefore, option A is correct.

What is direct variation ?

link between two variables that can be described mathematically by an equation where one variable equals a constant multiplied by the other. For instance, the constant of variation is k = = 3 if y varies straight as x and y = 6 when x = 2. Consequently, y = 3x is the equation that describes this directvariation.

When x is not equal to zero, an equation of the form y = kx describes the linear function known as direct variation. When x is not equal to zero and k is a nonzero real number constant, the equation of the form xy = k describes the nonlinear function known as inverse variation.

x = ky

where k is constant

25 = k × 75

25 / 75 = k

k = 1 / 3

now when y = 48 then substitute the values

x = ky

x = 1 ÷ 3 × 48

x = 16

Thus, option A is correct.

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The mass of carbon in is 12.007 amu, is 12.007, is 144.084 amu, and is 60.035 amu.

What is the mass of one Carbon atom?

The mass has been given as the sum of the atomic mass unit in the compound. The mass of 1 atom of carbon is 12.007 amu.

The mass of carbon in the following compounds is given as:

The number of Carbon units = 1

The mass of carbon in compound = 12.007 amu

The number of Carbon units = 1

The mass of carbon in the compound = 12.007 amu

The number of carbon units =12

The mass of carbon in the compound:  

The number of carbon units = 5

The mass of carbon in the compound:

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Answer:

The atomic mass of carbon (C) is 12.0107 amu, so if you want to calculate the total mass in each molecule, you just need to multiply the number of carbon atoms in the substance by 12.017. In (a) there is one atom of C, (b) have also one atom of C, (c) have 12 atoms of C, and (d) have five atoms of C. Thus, the total mass (amu) of carbon is:

(a) 12.017 amu

(b) 12.017 amu

(c) 144.204 amu

(d) 60.085 amu

Answer:

Explanation:

When an electron moves from a lower energy level to a higher energy level, energy is absorbed by the atom. When an electron moves from a higher to a lower energy level, energy is released and photon is emitted.

this emitted photon is depicted as a small wave-packet being expelled by the atom in a well-defined direction.

Answer:

226.2 kJ/mol

Explanation:

Let's consider the following thermochemical equation for the combustion of acetylene.

C₂H₂(g) + (5/2) O₂(g) → 2 CO₂(g) + H₂O(l), ΔH°rxn = –1299 kJ/mol.

We can also calculate the enthalpy of the reaction per mole of acetylene from the enthalpies of formation.

ΔH°rxn = 2 mol × ΔH°f(CO₂(g)) + 1 mol × ΔH°f(H₂O(l)) - 1 mol × ΔH°f(C₂H₂(g)) - 1 mol × ΔH°f(O₂(g))

1 mol × ΔH°f(C₂H₂(g)) = 2 mol × ΔH°f(CO₂(g)) + 1 mol × ΔH°f(H₂O(l)) - ΔH°rxn - 1 mol × ΔH°f(O₂(g))

1 mol × ΔH°f(C₂H₂(g)) = 2 mol × (-393.5 kJ/mol) + 1 mol × (-285.8 kJ/mol) - (-1299 kJ) - 1 mol × (0 kJ/mol)

ΔH°f(C₂H₂(g)) = 226.2 kJ/mol

Answer:

The enthalpy of formation of acetylene is 226.2 kJ/mol

Explanation:

Step 1: Data given

C2H2 (g) + (5/2)O2 (g)  → 2CO2 (g) + H2O (l)  Heat of Reaction (Rxn) = -1299kJ/mol

Standard formation [CO2 (g)]= -393.5 kJ/mol

Standard formation [H2O (l)] = -285.8 kj/mol

Step 2: The balanced equation

The formation of acetylene is:

2C(s) + H2(g)   → C2H2(g)

Step 3: Calculate the enthalpy of formation of acetylene

It doesn't matter if the process will happen in 1 step or in more steps. What matters is the final result. This is Hess' law of heat summation.

To have the reaction of the formation of acetylene we have to take:

⇒ the reverse equation of the combustion of acetylene

   2CO2 (g) + H2O (l) → C2H2 (g) + (5/2)O2 (g)

⇒  The equation of formation of CO2 (multiplied by 2)

2C(s) + 2O2(g) → 2CO2(g)

⇒ the equation of formation of H2O

H2(g) + 1/2 O2(g) → H2O(l)

2CO2 (g) + H2O (l) + 2C(s) + 2O2(g) + H2(g) + 1/2 O2(g  → C2H2 (g) + (5/2)O2 (g) + 2CO2(g) + H2O(l)

Final reaction = 2C(s) + H2(g)   → C2H2(g)

Calculate the enthalpy of formation of acetylene =

ΔHf = 1299 kJ/mol + (2*-393.5) kJ/mol + (-285.8) kJ/mol

ΔHf = 226.2 kJ/mol

The enthalpy of formation of acetylene is 226.2 kJ/mol