Answer:
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Explanation:
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277.79 atm is the calculated gas pressure.
The ideal gas is a fictitious concept used to study how real gases behave by comparing them to their deviations. The pressure-temperature rules are followed by an ideal gas.
177 atm is the initial pressure. The starting temperature is 298 K (25 °C = 25 + 273 °C).
195°C = 195+273
= 468K is the final temperature.
The pressure temperature relation illustrated below can be used to get the final pressure.
P1/T1 = P2/T1
= P1T2/T1
= 177 atm 468 K /298 K
= 277.97 atm
The final pressure is therefore 277.97 atm.
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Answer:
Explanation:
Step 1: Data given
The equilibrium constant, Kc, for the following reaction is 4.76 * 10^-4 at 431 K
The equilibrium concentration of Cl2(g) is 0.233 M
Step 2: The balanced equation
PCl5(g) ⇄ PCl3(g) + Cl2(g)
Step 3: The initial concentration
[PCl5]= Y M
[PCl] = 0M
[Cl2] = 0M
Step 4: Calculate the concentration at equilibrium
[PCl5] = Y + X M = Y - 0.233 M
[PCl]= XM = 0.233 M
[Cl2]= XM = 0.233 M
Step 5: Define Kc
Kc = [Cl2]* [PCl3] / [PCl5]
4.76 * 10^-4 = 0.233² / (Y -0.233)
0.000476 = 0.05429 / (Y - 0.233)
Y - 0.233 = 0.05429 / 0.000476
Y - 0.233 = 114.05 M
Y = 114.283 M = the initial concentration
The concentration of PCl5 at the equilibrium is 114.05 M
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