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2 years ago

Explain why nickel has a high density.

Chemistry

1 answer:

postnew [5]2 years ago

3 0

Density Of A Nickel:-

8.902 (25°C)

Explanation of why does nickel have a high density:-

Nickel is the only element named after the devil. The name comes from the German word Kupfernickel, meaning "Old Nick's copper," a term used by German miners. They tried to remove copper from an ore that looked like copper ore, but they were unsuccessful. ... Nickel is also used in the manufacture of many other alloys.

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3 years ago

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Question number 3..........

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3 years ago

Consider the following system at equilibrium where AH° = -10.4 kJ, and K. = 55.6, at 698 K. H2(E) +13(g) = 2HIE) If the VOLUME o

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For 1: The correct answer is Option C.

For 2: The correct answer is Option B.

For 3: The correct answer is Option C.

For 4: The correct answer is Option C.

Explanation:

We are given:

$K_e=55.6$

$\Delta H^o_{rxn}=-10.4kJ$

For the given chemical reaction:

$H_2(g)+I_2(g)\rightarrow 2HI(g)$

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle. This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Any change in volume during equilibrium is studied on the basis of change of moles of reactants and products.

When volume is decreased, the equilibrium will shift in the direction which produces fewer moles of gas and when volume is increased, the equilibrium will shift in the direction which produces more moles of gas.

Number of moles of gases on reactant side = [1 + 1] = 2

Number of moles of gases on product side = 2

Change in number of moles = 2 -2 = 0

As, number of moles on both the side of the reaction is same. This means there will be no effect on change in volume.

For 1:

As, there is no effect of volume on equilibrium. So, the equilibrium constant remains the same.

Hence, the correct answer is Option C.

For 2:

$K_c$ is the constant of a certain reaction at equilibrium while $Q_c$ is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.