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Consider the following hypothetical dissociation:
(a) addition of A(NO3)3
(b) increase in temperature
(c) adding Na+, forming NaB
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Chapter 15 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardAt a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the equilibrium constant KP for the transformation at 60 C? H2O(l)H2O(g)arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
- For the reaction 4 PH; (g) = 6 H,(g) + P¿(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] = 0.370 M, and [P] = 0.750 M. What is the equilibrium constant for this reaction? K.arrow_forwardThe dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.arrow_forward2. Calculate Q and compare it to K for the following conditions to indicate if the reaction proceeds forward or in reverse. CH;COOH (ag) + NO2"(aa) CH3CO0' (ag) + HNO2 (a9) K=0.045 a. [CH;COOH] = 0.010 M, [NO2] = 0.10 M, [CH;COO']= 1.0 M, [HNO2] = 0.50 M b. [CH;COOH] = 0.102 M, [NO2"] = 0.10 M, [CH;COO']= 0.021 M, [HNO2] = 0.019 Marrow_forward
- Assume that the change in concentration of N2O4 is small enough to be neglected in the following problem.(a) Calculate the equilibrium concentration of both species in 1.00 L of a solution prepared from 0.129 mol of N2O4 with chloroform as the solvent.N2 O4(g) ⇌ 2NO2(g) Kc = 1.07 × 10−5 in chloroform(b) Show that the change is small enough to be neglected.arrow_forwardQuestion 7 of 25 Write the equilibrium constant expressions for the following. Fill the missing powers in the expressions. (a) 2NAHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) Keq = (Pco, ) i (PH;0) i (b) 2N2(g) + 6H20(1) 24NH3(g) + 302(g) Keq = (PNH, ) (Ро.) (PN, ) (c) 2C2H4(g) + O2g) 2CH3CHO(g) Keq = (PCH,CHO ) i (Pc,H, ) (Po.) (d) Ag2SO4(s) 2 2Ag*(aq) + SO42-(aq) Keq = [Ag*] i [So;-] i (e) NH4HS(s) 2H2S(g) + NH3(g) Keq = (PH,s) i (PNH, ) iarrow_forwardWrite the concentration equilibrium constant expression for this reaction. 3+ Cr,0; (aq)+61 (aq)+ 14 H*(aq)→ 3 I,(s)+2 Cr³"(aq)+ 7 H,0(1) ?arrow_forward
- Vinegar (chemical name : acetic acid, CH3COOH) is a weak acid. Consider the ionization of acetic acid in water. CH3COOH(aq) = H*(aq) + CH3COO (aq) Kc=6.80 ×10-4 If the initial concentration of acetic acid is 0.150 M. What is the concentration of hydrogen ions (H*) at equilibrium? O 0.0100 M O 0.0500 M O 0.100 M O 0.500 Marrow_forwardConsider the following equilibrium: BaSO4 ⇌ Ba2+ (aq) + SO42- (aq) In which direction (if any) will the equilibrium shift if: MgSO4 is added? Ba(NO3)2 is added? NaOH is added?arrow_forwardConsider the synthesis of ammonia: N2 (g) +3H2(g) 2NH3 (g)arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
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