Respuesta :
Answer:
the fraction of CO reacted is 0.76 or 76.0 %
Explanation:
Step 1: Data given
a new catalyst combines a 2.0 : 1.0 mole ratio mixture of carbon monoxide and oxygen gas
Volume = 2.45 L
Total pressure = 740 torr
Temperature = 552 °C = 825 K
Pressure decreases to 552 torr
Step 2: The balanced equation
2CO(g) + O2 (g) --> 2CO2(g)
Step 3: Calculate the percentage of the CO was converted to CO2
P1/n1 = P2/n2
⇒P1 = the initial pressure = 740 torr
⇒n1 = the initial number of moles = 2.0 moles CO and 1 mol of O2 = 3.0 moles
⇒P2 = the final pressure = 552 torr
⇒n2 = the final number of moles = TO BE DETERMINED
n2 = n1 * P2/P1
n2 =3.0 * 552 torr / 740 torr
n2 = 2.24 moles
Step 4: Calculate total moles of CO
Suppose X = the fraction of CO
final = 2*(x) + 3*(1-x)
2.24 = 2x + 3 - 3x
2.24 = -X + 3
-0.76 = -X
X = 0.76
This means the fraction of CO reacted is 0.76 or 76.0 %
The fraction or the percentage of the carbon monoxide converted to carbon dioxide is 76%.
Given:
Ratio of new catalyst to the mole ratio of carbon dioxide and oxygen = 2:1
Volume = 2.45 L
Temperature = 825 K
Pressure = 740 torr
The reaction is:
2CO(g) + O₂ (g) [tex]\rightarrow[/tex] 2CO₂
From the reaction, the amount of CO converted into carbon dioxide is:
[tex]\dfrac{\text{P}_1}{\text n _1}&=\dfrac{\text{P}_2}{\text n _2}[/tex]
Where,
P₁ = initial pressure
n₁ = number of moles (initial)
P₂ = final pressure
n₂ = final number of moles
Now, calculating the n₂:
[tex]\text n_2 &= \dfrac{\text n_1 \times \text P_2}{\text P_1}[/tex]
[tex]\text n_2 &= \dfrac{3 \times 552}{740}[/tex]
n₂ = 2.24 moles.
Now, the total moles of carbon monoxide is:
2.24 = 2 x Y + 3 x (1 - Y)
2.24 = 2Y + 3 - 3Y
Y = 0.76
Thus, the number of a fraction of CO is 0.76.
To know more about moles, refer to the following link:
https://brainly.com/question/20486415
