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3 years ago

10 moles of hydrogen are allowded to react with 6 moles of oxygen .How much water molecules are obtained?

Chemistry

1 answer:

DiKsa [7]3 years ago

5 0

Answer:

Since 2H₂ + O₂ ---> 2H₂O

We need 2 moles of hydrogen for each mole of oxygen

So, we need 2(6) = 12 moles of H₂ but since we only have 10 moles,

H₂ is the limiting reagent

So since 2 moles of H₂ gives 2 moles of water,

10 moles of H₂ will give rise to 10 moles of Water with 1 mole of remaining oxygen

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A layer of sandstone is found on top of a layer of shale. What most likely happened in this area?

storchak [24]

Answer:

Mud was deposited first, then sand.

Explanation:

This could have been a tidal mud flat succeeded by a sandy beach, or along the bed and course of a river with either mountain building upstream causing faster flow and carrying of mud farther away or the sea level falling with mud deposits being found closer to the new coastline. Hope this helps!

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3 years ago

State whether the sign of the entropy change expected for each of the following processes will be positive or negative, and expl

Strike441 [17]

Answer:

a) ΔS is negative

b) ΔS is positive

c) ΔS is positive

d) ΔS is negative

Explanation:

Entropy (S) is a thermodynamic parameter which measures the randomness or the disorder in a system. Greater the disorder more positive will be the value of entropy.

The extent of disorder increases as substances transition from the solid to the gaseous state. i.e.

S(solid) < S(liquid) < S(gas)

The entropy change for a given reaction is:

$\Delta S = S(products)-S(reactants)----(1)$

a) $PCl3(l) + Cl2(g) \rightarrow PCl5(s)$

Here the reactants are in the liquid and gas phase which have higher entropy than the product which is in the solid phase i.e. lower entropy.

Since S(product) < S(reactant), based on equation 1, ΔS will be negative.

b) $2HgO(s) \rightarrow 2Hg(l) + O2(g)$

Here the products are in the liquid and gas phase which have higher entropy than the reactant which is in the solid phase i.e. lower entropy.

Since S(product) > S(reactant), based on equation 1, ΔS will be positive.

c) $H2(g) \rightarrow 2H(g)$

Here the products and reactants are in the gas phase. However the number of moles of products is greater than the reactants

Since S(product) > S(reactant), based on equation 1, ΔS will be positive.

d) $U(s) + 3F2(g) \rightarrow UF6(s)$

Here one of the reactants is in the gas phase which corresponds to a more positive entropy compared to the product which is in the solid phase i.e. lower entropy.

Since S(product) < S(reactant), based on equation 1, ΔS will be negative.

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3 years ago

Is each of these statements true? If not, explain why.(p) A bimolecular reaction is generally twice as fast as a unimolecular re

Ede4ka [16]

A bimolecular reaction typically takes twice as long as a unimolecular reaction. The answer is true

<h3>How is activation energy related to temperature?</h3>

Consider what must occur for ClNO2 to react with NO to understand why reactions have an activation energy.
First and foremost, these two molecules must clash in order to organise the system.
Not only must they be brought together, but they must also be kept in precisely the appropriate orientation relative to one other in order for the reaction to occur.
Some energy must also be used in order to break the Cl-NO2 bond and allow the Cl-NO bond to form.

learn more about bimolecular reaction refer

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2 years ago

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VMariaS [17]

A. I think I’m that’s what it is

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4 years ago

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UkoKoshka [18]

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+180kJ

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