Given the reaction: h2o2(l) ⇌ h2(g) + o2(g) the forward reaction is endothermic. determine which of the following changes would result in equilibrium shifting towards the products. i. increase h2 ii. decrease o2 iii. add a catalyst iv. increase the temperature v. increase h2o2

Option(II) and option (IV) are correct.

Explanation:

Here products are and and reactant is

(I) According to Le-chatelier principle,increase in  will shift the equilibrium towards reactant side to keep the equilibrium constant unchanged.

(II) According to Le-chatelier principle,decrease in  will shift the equilibrium towards product side to keep the equilibrium constant unchanged.

(III) Adding a catalyst will not change position of equilibrium. Catalyst only helps to achieve equilibrium in a lesser time.

(IV) As this reaction is an endothermic reaction therefore heat is consumed in formation of product. Therefore increase in temperature will lead to formation of more product to consume excess heat added.

(V) Pure solids and liquids do not affect position of equilibrium as their concentrations remain unchanged.

answer

fusion: the energy source of stars. the energy released from the collapse of the gas into a protostar causes the center of the protostar to become extremely hot. when the core is hot enough, nuclear fusion commences. fusion is the process where two hydrogen atoms combine to form a helium atom, releasing energy.

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