CH₃CH₂CH₂OH + KMnO₄/H⁺ ------------------------>CH₃CH₂COOH  i.e. propanoic acid.

let A be area of vessel.

a be area of hole

at any time let H be level of water in the vessel.

Time taken for water level to get reduced from H to 0 is given by  

Time taken for water level to get reduced from H/2 to 0 is given by

therefore Time taken for water level to get reduced from H to H/2 is given by (T1)=

  ---      ---------------------1

and Time taken for water level to get reduced from H/2 to 0 is given by (T2) =    -------------2

on dividing eqn 1 by 2 we get. T1/T2 =

the dipolar moment of nitrocyclohexane  is larger than the dipolar moment of nitobenzene because in nitrocyclohexane dipole moment due to lone pair is outwards completely and in nitobenzene the lone pair is in conjugation with the multiple bond of the benzene ring, therefore dipole moment due to the lone pair gats reduced to a large extent.

For PH₃ Hybridization is not defined- refer to drago's rule for more explaination.

H₂S- its hybridization is SP₃

either you should mention a particular aldehyde or the question should be conversion of aldehydes into carboxylic acid and in that case answer would be as followed:-

Aldehyde can be converted into carboxylic acid by its oxidation with a strong oxidising agents like KMnO₄/H⁺ or K₂Cr₂O₇/H⁺ ,i.e. in presence of strong acid.

When 1- propanol is treated with SOCl_2, following reaction takes place

CH₃-CH₃-CHOH + SOCl₂ -----> CH₃CH₂CHCl+SO₂+HCl

Many chemical reactions release energy in the form of heat, light, or sound. These are exothermic reactions. Exothermic reactions may occur spontaneously and result in higher randomness or entropy (ΔS > 0) of the system. They are denoted by a negative heat flow (heat is lost to the surroundings) and decrease in enthalpy (ΔH < 0). In the lab, exothermic reactions produce heat or may even be explosive.

There are other chemical reactions that must absorb energy in order to proceed. These are endothermic reactions. Endothermic reactions cannot occur spontaneously. Work must be done in order to get these reactions to occur. When endothermic reactions absorb energy, a temperature drop is measured during the reaction. Endothermic reactions are characterized by positive heat flow (into the reaction) and an increase in enthalpy (+ΔH).

Examples of Endothermic and Exothermic Processes

Photosynthesis is an example of an endothermic chemical reaction. In this process, plants use the energy from the sun to convert carbon dioxide and water into glucose and oxygen. This reaction requires 15MJ of energy (sunlight) for every kilogram of glucose that is produced:

sunlight + 6CO₂(g) + H₂O(l) = C₆H₁₂O₆(aq) + 6O₂(g)

An example of an exothermic reaction is the mixture of sodium and chlorine to yield table salt. This reaction produces 411 kJ of energy for each mole of salt that is produced:

Na(s) + 0.5Cl₂(s) = NaCl(s)

Many chemical reactions release energy in the form of heat, light, or sound. These are exothermic reactions. Exothermic reactions may occur spontaneously and result in higher randomness or entropy (ΔS > 0) of the system. They are denoted by a negative heat flow (heat is lost to the surroundings) and decrease in enthalpy (ΔH < 0). In the lab, exothermic reactions produce heat or may even be explosive.

There are other chemical reactions that must absorb energy in order to proceed. These are endothermic reactions. Endothermic reactions cannot occur spontaneously. Work must be done in order to get these reactions to occur. When endothermic reactions absorb energy, a temperature drop is measured during the reaction. Endothermic reactions are characterized by positive heat flow (into the reaction) and an increase in enthalpy (+ΔH).

Examples of Endothermic and Exothermic Processes

Photosynthesis is an example of an endothermic chemical reaction. In this process, plants use the energy from the sun to convert carbon dioxide and water into glucose and oxygen. This reaction requires 15MJ of energy (sunlight) for every kilogram of glucose that is produced:

sunlight + 6CO₂(g) + H₂O(l) = C₆H₁₂O₆(aq) + 6O₂(g)

An example of an exothermic reaction is the mixture of sodium and chlorine to yield table salt. This reaction produces 411 kJ of energy for each mole of salt that is produced:

Na(s) + 0.5Cl₂(s) = NaCl(s)

we know that time period of the pendulum = 1s.

also time period of spring mass system =

therefore by equating time period by 1 we get

m = 4π²k

here k = 0.1

therefore m =3.947 kg.

vector V =6i+2j-2k

let any other vector U = i+j+k

component of V along U is given by [(V. )]

we know that modulus of U here is

V.U = (6*1)+(2*1)-(2*1)

   = 6

also

therefore required answer is = 

            =2i+2j+2k

The plasma state is the fourth  state of matter and the most diffused in the  Universe. It is characterized by the absence of  molecular bond for biatomic gases such as  Nitrogen and Hydrogen and atomic bond for  mono atomic gases such as Argon and Helium. By  supplying  HEAT ENERGY to a biatomic gas,  its molecule breaks into atoms and atoms by further energy, break  into one or more positive charges.
Hence the plasma state is an ionized gas, formed  by positive ions and negative electrons of the  gas initially in neutral condition and is a very  good conductor of electricity and is affected by  magnetic fields.

.

Plasma is so energetic or "hot" that in space it consists soley of ions and electrons. It is only when plasma is cooled that the atoms or molecules that are so predominant in forming gases, liquids, and solids that we are so accustomed to on Earth, is possible. So, in space, plasma remains electrically charged. Thus plasmas carry electric currents and are more influenced by electromagnetic forces than by gravitational forces. Outside the Earth's atmosphere, the dominant form of matter is plasma, and "empty" space has been found to be quite "alive" with a constant flow of plasma.

we know that sin(90-A) =cos A

therefore sin 72 = cos 18

we know that cos 18=

and sin60 =

therefore rquired value =    - 

solve it and get the answer