For the following system,
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Introductory Chemistry: An Active Learning Approach
- 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 certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forwardShow that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forward
- Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.arrow_forwardWrite the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 HF (aq) + H20(1) H30+(aq) + F (aq) K =arrow_forwardWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution.arrow_forward
- Write the expression for the equilibrium constant K, for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PH )° as (P NH;°. If either the numerator or denominator is 1, please enter 1 NH,CI(s) + NH;(g) + HCl(g) K =arrow_forwardWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. (CH3),NH (aq) + H2O(1) (CH)2NH2* (аq)+ оH(аq) K =arrow_forwardwrite the chemical reaction for the following equilibrium constantarrow_forward
- isnt it Kp?arrow_forwardConsider the following balanced chemical equation CH3COOH (aq) + NO2 (aq) = CH3COO-(aq) + HNO2 (aq) a. Predict whether this reaction will favor the products or reactants at equilibrium b. Given the following information, calculate the equilibrium constant for the reaction above, does your prediction make sense?arrow_forwardThe equilibrium constant, Keq, for the reaction: 2 NOCl(g) -> 2NO(g) + Cl2(g) is 2.4 x 10-7 (no units). What is the Keq for the reaction 1/3 Cl2(g) + 2/3 NO (g) -> 2/3 NOCl(g)arrow_forward
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