Question

1) For the reaction below, which change would cause the equilibrium to shift to the right? CH4(g) + 2H2S(g) ? CS2(g) + 4H2(g) (a) Decrease the concentration of dihydrogen sulfide. (b) Increase the pressure on the system. (c) Increase the temperature of the system. (d) Increase the concentration of carbon disulfide. (e) Decrease the concentration of methane. 2) What would happen to the position of the equilibrium when the following changes are made to the equilibrium system below? 2SO3(g) ? 2SO2(g) + O2(g) (a) Sulfur dioxide is added to the system. (b) Sulfur trioxide is removed from the system. (c) Oxygen is added to the system. 3) What would happen to the position of the equilibrium when the following changes are made to the reaction below? 2HgO(s) ? Hg(l) + O2(g) (a) HgO is added to the system. (b) The pressure on the system increases.

          1) For the reaction below, which change would cause the equilibrium to shift to the right?
CH4(g) + 2H2S(g) ? CS2(g) + 4H2(g)
(a) Decrease the concentration of dihydrogen sulfide.
(b) Increase the pressure on the system.
(c) Increase the temperature of the system.
(d) Increase the concentration of carbon disulfide.
(e) Decrease the concentration of methane.
2) What would happen to the position of the equilibrium when the following changes are
made to the equilibrium system below?
2SO3(g) ? 2SO2(g) + O2(g)
(a) Sulfur dioxide is added to the system.
(b) Sulfur trioxide is removed from the system.
(c) Oxygen is added to the system.
3) What would happen to the position of the equilibrium when the following changes are
made to the reaction below?
2HgO(s) ? Hg(l) + O2(g)
(a) HgO is added to the system.
(b) The pressure on the system increases.

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1) For the reaction below, which change would cause the equilibrium to shift to the right?
CH4(g) + 2H2S(g) ? CS2(g) + 4H2(g)
(a) Decrease the concentration of dihydrogen sulfide.
(b) Increase the pressure on the system.
(c) Increase the temperature of the system.
(d) Increase the concentration of carbon disulfide.
(e) Decrease the concentration of methane.
2) What would happen to the position of the equilibrium when the following changes are
made to the equilibrium system below?
2SO3(g) ? 2SO2(g) + O2(g)
(a) Sulfur dioxide is added to the system.
(b) Sulfur trioxide is removed from the system.
(c) Oxygen is added to the system.
3) What would happen to the position of the equilibrium when the following changes are
made to the reaction below?
2HgO(s) ? Hg(l) + O2(g)
(a) HgO is added to the system.
(b) The pressure on the system increases.

Added by Guillermo D.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Jital V

02/26/2022

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For the reaction below, which change would cause the equilibrium to shift to the right? CH4 + 2H2S ↔ CS2 + 4H2 (a) Decrease the concentration of dihydrogen sulfide. (b) Increase the pressure on the system. (c) Increase the temperature of the system. (d) Increase the concentration of carbon disulfide. (e) Decrease the concentration of methane.

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Transcript

00:01 Welcome here in this question we have a reaction.

00:03 So ch4 gas reacting with 2h2s gas, gistras 2, it is at equilibrium with cs2 gas plus 4h2 gas.

00:18 Okay, so they are asking which conditions are which change would cause the equilibrium to shift right, right? means towards product side.

00:32 So which change will produce this change? so the shift.

00:39 So the first option is change in decrease in concentration of dihydrozen sulfide.

00:47 So decrease in concentration of h2s.

00:52 So decrease in concentration means it is happens because it shifts towards right side, left side because the decrease in concentrations of reactants and increase in concentrations of concentrations of products.

01:21 So then equilibrium shifts towards left.

01:34 Left means reactant side.

01:42 We want to shift the equilibrium to right side, not left side.

01:48 So that's why it is wrong statement.

01:51 And if we increase the, so what is the correct statement? if we increase the concentration of reactants and decrease in concentration of products, then equilibrium shifts towards right means.

02:15 So then forward reaction will take place.

02:18 Okay.

02:18 So the first one is wrong.

02:21 And the second one, they are given here.

02:26 The decrease in the pressure on the system.

02:31 Decrease the pressure on the system.

02:43 So change in pressure means if we have the positive.

02:49 So if delta n.

02:52 Of gas is negative then due to pressure or change in volume so there is a left shift shift of equilibrium is towards left and delta n of gas is to then it goes to right side right side shift will be happened and delta n is equal to zero there is no change in equilibrium so there is no new equilibrium so there is no new equilibrium will produce...

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