Answer:
The correct answer is "0.0179".
Explanation:
The given reaction is:
⇒ [tex]CO_2(g) + C(s) \rightleftharpoons 2 \ CO(g)[/tex]
The given value is:
At 727°C temperature,
Kp = 1.47
As we know,
Gas constant,
R = 0.0821 L atm/mol.K
Temperature,
= [tex]727+273[/tex]
= [tex]1000 \ K[/tex]
Now,
The change in moles will be:
⇒ [tex]\Delta n=Products-reactants[/tex]
⇒ [tex]=2-1[/tex]
⇒ [tex]=1[/tex]
As we know,
⇒ [tex]K_p=K_c(RT)^{\Delta n}[/tex]
On substituting the given values, we get
⇒ [tex]1.47=K_c(0.0821\times 1000)^1[/tex]
⇒ [tex]K_c=\frac{1.47}{0.0821\times 1000}[/tex]
⇒ [tex]=\frac{1.47}{82.1}[/tex]
⇒ [tex]=0.0179[/tex]
The correct answer is "0.0179".
[tex]k_p=k_c(RT)^{n}[/tex]
At 727°C temperature,
Kp = 1.47
Gas constant,R = 0.0821 L atm/mol.K
Temperature=[tex]727+273=1000 K[/tex]
Now,
The change in moles will be:[tex]2-1=1[/tex]
On substituting the given values, we get
[tex]1.47=k_c\times(0.0821\times1000)^{1} \\\\k_c=0.0179[/tex]
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