Methanol ( C H 3 O H ) is manufactured by the reaction of carbon monoxide with hydrogen in the presence of a C u / Z n O / A l 2 O 3 catalyst: C O ( g ) + 2 H 2 ( g ) ⇌ C a t a l y s t C u / Z n O / A l 2 O 3 C H 3 O H ( g ) Δ H ° = − 91 k j Does the amount of methanol increase, decrease, or remain the same when an equilibrium mixture of reactants and products is subjected to the following changes? The temperature is increased. The volume is decreased. Helium is added. CO is added. The catalyst is removed.
Methanol ( C H 3 O H ) is manufactured by the reaction of carbon monoxide with hydrogen in the presence of a C u / Z n O / A l 2 O 3 catalyst: C O ( g ) + 2 H 2 ( g ) ⇌ C a t a l y s t C u / Z n O / A l 2 O 3 C H 3 O H ( g ) Δ H ° = − 91 k j Does the amount of methanol increase, decrease, or remain the same when an equilibrium mixture of reactants and products is subjected to the following changes? The temperature is increased. The volume is decreased. Helium is added. CO is added. The catalyst is removed.
Solution Summary: The author explains that a chemical reaction is in equilibrium if there is no further change in its concentration takes place with time.
Methanol (
C
H
3
O
H
) is manufactured by the reaction of carbon monoxide with hydrogen in the presence of a
C
u
/
Z
n
O
/
A
l
2
O
3
catalyst:
C
O
(
g
)
+
2
H
2
(
g
)
⇌
C
a
t
a
l
y
s
t
C
u
/
Z
n
O
/
A
l
2
O
3
C
H
3
O
H
(
g
)
Δ
H
°
=
−
91
k
j
Does the amount of methanol increase, decrease, or remain the same when an equilibrium mixture of reactants and products is subjected to the following changes?
The oxidation of glucose (C6H12O6) in body tissue producesCO2 and H2O. In contrast, anaerobic decomposition,which occurs during fermentation, produces ethanol(C2H5OH) and CO2. (a) Compare the equilibrium constants for the following reactions:
C6H12O6(s) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(l)
C6H12O6(s) ⇌ 2 C2H5OH(l) + 2 CO2(g)
(b) Compare the maximum work that can be obtained fromthese processes under standard conditions.
Consider the following general reaction:2A(g) + 2B(g) ⇌ 3C(g)
The reaction was measured to have an equilibrium reaction constant (K) of 0.0100 at 100 K. If the reaction has a standard enthalpy change (ΔHrxn) of 500.3 J/mol, what should the equilibrium reaction constant be when the temperature is 800 K? (Please provide your answer to 3 significant figures.)
For the following reaction:
2 A(aq) + 2 B(aq) ⇌ 3 C(aq)
Calculate the magnitude of Kc (don't report the units) assuming the following composition at equilibrium:
[A] = 0.297 mol L-1
[B] = 0.5 mol L-1
[C] = 0.14 mol L-1
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