The equilibrium constant, Kp, for the following reaction is 3.11×10-³ at 350 K: 21Br(g) Br₂(g) + 12(g) Calculate the equilibrium partial pressures of all species when IBr(g) is introduced into an evacuatec flask at a pressure of 0.954 atm at 350 K. P IBr P Bra = atm atm

The equilibrium constant, Kp, for the following reaction is 3.11×10-³ at 350 K: 21Br(g) Br₂(g) + 12(g) Calculate the equilibrium partial pressures of all species when IBr(g) is introduced into an evacuatec flask at a pressure of 0.954 atm at 350 K. P IBr P Bra = atm atm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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IBr
The equilibrium constant, Kp, for the following reaction is 3.11×10-³ at 350 K:
21Br(g) Br2(g) + 1₂(g)
Calculate the equilibrium partial pressures of all species when IBr(g) is introduced into an evacuated
flask at a pressure of 0.954 atm at 350 K.
P
=
Br2
||
=
PI2
Submit Answer
References
Use the References to access important values if needed for this question.
atm
atm
atm

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The equivalence point is defined as moles acid = moles base. So first, let's calculate the initial moles of base we used. molpase Mpase = Volsoiution Molarity base = 0.100 (M) Volume of solution= _50.00 mL Moles of base = _5.00 mmol So, we need 5.00 mmol of acid (titrant) to be delivered to the analyte. Since we know the molarity of the acid and moles of acid, we just need to solve for the volume of acid (titrant) to be added. molacid Voladded Macid Molarity acid = . 0.200 (M) Moles of acid = _5.00 (mmol) Volume of acid needed to reach equivalence point (mL)
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