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3 years ago

In a closed system, how will a decrease in pressure affect the following reaction: 2A(g) +2B(g) ⇌ 2C(g) + 2D(g)?

Chemistry

2 answers:

LekaFEV [45]3 years ago

6 0

Answer:

B. No change will occur.

Explanation:

Notice that the two moles of gas on the side of the reactants also reflects on the side of the products (i.e. there are also two moles of gas on the side of the products).

This translates to there won't be any change in the equilibrium if the pressure is increased.

The only important factor to take note of is that altering the pressure can only result in a significant change for equilibrium reactions between gases, when the reaction features a change in the number of moles of gas.

DochEvi [55]3 years ago

3 0

As number of gaseous moles in reactant and prodict are same that is 4

So No change will occur

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Answer:

Bromine (Br) loses an electron, so it is the reducing agent.

Explanation:

A reducing agent also called a reducer, is known to be an electron donor. A reducing agent is oxidized, because it loses electrons in the redox reaction.

A oxidising agent also called a oxidant or oxidiser, is known to be an electron acceptor. A oxidising agent is reduced, because it gains electrons in the redox reaction.

Cl2(aq) + 2Br-(aq) --> 2Cl-(aq) + Br2(aq)

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Cl2(aq) + 2e- --> 2Cl-(aq)

2Br-(aq) --> Br2(aq) + 2e-

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Calculate the volume(in L), at STP, of carbon dioxide produced by the complete combustion of 6.75 lbs of charcoal.

gtnhenbr [62]

535.8 L volume(in L), at STP, of carbon dioxide produced by the complete combustion of 6.75 lbs of charcoal.

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The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Given:

$C(s) + O_2(g)$ ⇒ $CO_2(g)$

1 mole of $CO_2(g)$ is formed from 1 mole of charcoal, that means 1 mole of $CO_2(g)$ is formed from 12 g of charcoal.

1 lbs = 453.592 grams

6.75 lbs = 6.75 x 453.592 =3061.746g

So, $CO_2(g)$ formed from 3061.746g of charcoal is:

= $\frac{1}{12}$ x 3061.746g

=255.14 mol.

Now, at STP, the volume of 1 mol of gas =22.4 L

Volume of 255.14 mol of $CO_2(g)$ = 255.14 x 22.4 L

Volume of 255.14 mol of $CO_2(g)$ = 535.8 L

Hence, 535.8 L volume(in L), at STP, of carbon dioxide produced by the complete combustion of 6.75 lbs of charcoal.

Learn more about the ideal gas here:

brainly.com/question/27691721

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