Use the balanced equation below to answer the question that follows

Consider the chemical equation in equilibrium.

djverab [1.8K]

Answer:

The forward reaction will be favored.

Explanation:

The reaction is:

$2H_{2}(g)+2O_{2}(g)--->2H_{2}O(g)$

As per equation (equilibrium equation), there are two moles of gaseous molecules on product side and three moles of reactant side.

a) If we increase pressure, the volume will decrease.

b) Due to decrease in volume, the moles per unit volume will increase.

c) In order to attain equilibrium again, the system will shift in the direction where it can nullify this effect [Le Chatelier's principle]

d) This can be done, if system moves in the direction where number of moles of gaseous molecules are less, which is product side.

e) Thus forward reaction will be favored.

4 0

3 years ago

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Solid substances are most likely to sublime if they have...?

tankabanditka [31]

Technically the are both right and wrong. Solid substances are most likely to sublime is they have... high vapor pressure and weak intermolecular forces.

5 0

3 years ago

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what are the reactants in the first word equation above. magnesium+hydrochloric acid ⇒ magnesium chloride + hydrogen

Alex

Answer:

magnesium+ hydrochloric acid is the reactants

Explanation:

the reactants are always in the left and the products are always in the right by

magnesium+hydrochloric acid ⇒ magnesium chloride + hydrogen

by combining magnesium and hydrochloric acid it produces magnesium chloride and hydrogen.

hope this helps..

6 0

3 years ago

Given the two half-reactions, what must be done in the next step before the reaction can be balanced? Au3+ --> Au I- --> I

Artyom0805 [142]

Answer:

The balance equation is

$2Au^{+3} + 6I^{-}$ → $2Au + 3I_{2}$

Explanation:

first, we have to make sure that the atoms are balanced

$Au^{+3}$ → $Au^{}$

$2I^{-}$ → $I_{2}$

then we proceed to balance charges of each half-reaction

$Au^{+3} + 3e^{-}$ → $Au^{}$

$2I^{-}$ → $I_{2}$ $+ 2e^{-}$

Now we multiply the half-reactions to match the number of electrons in each one

( $Au^{+3} + 3e^{-}$ → $Au^{}$ )x2

( $2I^{-}$ → $I_{2}$ $+ 2e^{-}$ )x3

and now we do the sum of the half-reactions

2 $Au^{+3} + 6e^{-}$ → 2 $Au^{}$

$6I^{-}$ → 3 $I_{2}$ $+ 6e^{-}$

$2Au^{+3} + 6I^{-}$ → $2Au + 3I_{2}$

note: the only atom that needed to be balanced was I

3 0

4 years ago

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Which phase change is an example of an exothermic process?

liberstina [14]

its solid to liquid

5 0

3 years ago