Q2: The management of a medium-sized manufacturing firm has invited you the HR Manager of the firm to act as an Internal Organization Theory (OT) Specialist to initiate a study of the problems and issues faced by the firm. For this purpose a preliminary meeting is scheduled and you have planned to deliver a presentation on a framework of OT. Elaborate the subject matter will you cover in the presentation? – 2.5 marks (Word limit 150 to 200 words).

Answer:

nth term of A.P 9,7,5....=a+(n−1)d

⇒9+(n−1)−2

⇒9−2n+2⇒11−2n

nth term of A.P 15,12,9,....=a+(n−1)d

⇒15+(n−1)−3

⇒15−3n+3⇒18−3n

∴11−2n=18−3n

⇒3n−2n=18−11

⇒n=7

Step-by-step explanation:

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Answer:

there are some species it doesn't exist like the Dodo,Banded allotoca,Yellow fatu,Zanzibar Leopard,Quagga.ect

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Answer:

Dodo,

Tasmanian tiger,

passenger pigeon,

Great auk,

Quagga,

Wooly mammoth,

Wooly rhinoceros,

Western Black rhinoceros are some i know dude

Answer:

-7

Step-by-step explanation:

-t - 3 - 2t=10

-3t - 3=10

t= -10/3

[tex] \frac{1}{2} (t + 3) - 2t = 5 \\ = > \frac{1}{2} t + \frac{3}{2} - 2t = 5 \\ = > \frac{t - 4t}{2} = \frac{10 - 3}{2} \\ = > - 3t = - 7 \\ = > t = \frac{7}{3} \: (ans.)[/tex]

Answer:

Explanation:

Hint: We know that benzene (C6H6(l)) contains three double bonds. To break these three bonds and convert benzene (C6H6(l)) to cyclohexane (C6H12(l)) three molecules of hydrogen (H2) will be required. To calculate the enthalpy of hydrogenation of the given compound we must add resonance energy to the total enthalpy of the reaction.

Complete step by step solution:

We are given that the enthalpy of hydrogenation of benzene (C6H6(l)) is −205 kJ and the resonance energy of benzene as −152 kJ/mol.

To calculate the actual enthalpy of hydrogenation of benzene if there is no resonance we add the enthalpy of hydrogenation and the resonance energy. Thus,

ΔHcyclohexene=ΔHbenzene+Resonance energy

Where ΔHcyclohexene is the enthalpy of hydrogenation of cyclohexene,

            ΔHbenzene is the enthalpy of hydrogenation of benzene.

Substitute −205 kJ for the enthalpy of hydrogenation of benzene, −152 kJ/mol for the resonance energy of benzene and solve for the enthalpy of hydrogenation of cyclohexene. Thus,

ΔHcyclohexene=(−205 kJ/mol)+(−152 kJ/mol)

ΔHcyclohexene=−357 kJ/mol

Thus, the actual enthalpy of hydrogenation of benzene is −357 kJ/mol

.

The hydrogenation reaction of benzene is as follows:

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In this reaction, three bonds break and three hydrogen molecules are required.

In the given figure i.e. cyclohexene there is only one double bond. Thus, only one molecule of hydrogen will be required for the breaking of the bond.

Thus, enthalpy of hydrogenation of cyclohexene will be,

ΔHcyclohexene=ΔHbenzene3

Where ΔHcyclohexene is the enthalpy of hydrogenation of cyclohexene,

            ΔHbenzene is the enthalpy of hydrogenation of benzene.

Substitute −357 kJ/mol

for the enthalpy of hydrogenation of benzene. Thus,

ΔHcyclohexene=−357 kJ/mol3

ΔHcyclohexene=−119 kJ/mol

Thus, the enthalpy of hydrogenation of the given figure is −119 kJ/mol.

Thus, the correct option is (D) −119 kJ/mol.

Note:

Do not forget to consider the signs of enthalpy of hydrogenation and the resonance energy in the calculation. To break one pi-bond one molecule of hydrogen is required.