How many moles of C2H2 are needed to react completely with 84.0 mol O2?
2 answers:
Answer: 33.6 moles
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
Combustion of ethylene is represented by following balanced equation:
According to stoichiometry:
5 moles of react completely with = 2 moles of
Thus 84.0 moles of react completely with =
moles of
Thus 33.6 moles of are needed to react completely with 84.0 mol
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Answer:
Explanation:
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In this case, since the average rate of reaction is computed as a change given by:
In such a way, given the concentrations at the specified times, we plug them in to obtain:
Whose negative sign means the concentration decreased due to the decomposition.
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Answer:
A. O=C=O and O≡C−O
Explanation:
Resonance:
When the electron distribution on the molecule become uneven like one molecule have more electron compare to other.Resonance occurs due to overlap of the orbitals.When electron flow through pi system then resonance occurs.
So the option A is correct.
A. O=C=O and O≡C−O
setup 1 : to the right
setup 2 : equilibrium
setup 3 : to the left
<h3>Further explanation</h3>The reaction quotient (Q) : determine a reaction has reached equilibrium
For reaction :
aA+bB⇔cC+dD
Comparing Q with K( the equilibrium constant) :
K is the product of ions in an equilibrium saturated state
Q is the product of the ion ions from the reacting substance
Q <K = solution has not occurred precipitation, the ratio of the products to reactants is less than the ratio at equilibrium. The reaction moved to the right (products)
Q = Ksp = saturated solution, exactly the precipitate will occur, the system at equilibrium
Q> K = sediment solution, the ratio of the products to reactants is greater than the ratio at equilibrium. The reaction moved to the left (reactants)
Keq = 6.16 x 10⁻³
Q for reaction N₂O₄(0) ⇒ 2NO₂(g)
Setup 1 :
Q<K⇒The reaction moved to the right (products)
Setup 2 :
Q=K⇒the system at equilibrium
Setup 3 :
Q>K⇒The reaction moved to the left (reactants)