Answer:
The total pressure is 0.8 atm
Explanation:
Step 1: The balanced equation
2 A(g) + 3 B(g) → A2B3 (g)
This means that for 2 moles of A consumed, we need 3 moles of B to produce 1 mole of A2B3
Initial pressure of A = 1.20 atm
Initial pressure of B = 1.20 atm
Step 2: Calculate limiting reactant and reactant in excesss
If 3 moles of B need 2 moles of A to be consumed; then 1.2 mole of B needs 0.8 moles of A.
0.8 moles of A will be consumed, this means 0.4 moles will remain.
⇒ A is in excess
B will completely react, so B is the limiting reactant
If 3 moles of B need 2 moles of A to be consumed; then 0.4 moles of A2B3 will be produced.
Step 3: Calculate the total pressure
Final pressure of A = 0 atm
Final pressure of B = (1.20 - 0.80) atm = 0.40 atm
Final pressure of A₂B₃ = 0.40 atm
Total pressure = pressure A + pressure B + pressure A2B3 = 0 atm + 0.4 atm + 0.4 atm = 0.8 atm
The total pressure at the end of the reaction is 0.8 atm.
The sum of the pressures of each individual gas can be used to calculate the overall pressure of a mixture of gases.
Calculation:
Given, equation is:
2 A(g) + 3 B(g) → A2B3 (g)
Initial pressure of A = 1.20 atm.
Initial pressure of B = 1.20 atm.
Now, If 3 moles of B need 2 moles of A, then 1.2 moles of B needs 0.8 moles of A.
There will be 0.4 moles of A left after 0.8 moles of A have been consumed.
Final pressures:
A = 0
B = (1.20 - 0.80) = 0.40
A₂B₃ = 0.40 atm.
Calculating the total pressure:
The total pressure = pressure A + pressure B + Pressure A2b3
0 atm. + 0.4 atm. + 0.4 atm. = 0.8 atm.
Thus, the total pressure will be 0.8 atm.
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