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- -cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F91. Which of the following correctly describes the equilibrium constant for the gas-phase reaction between Hland Ozlto form gaseous Ke a) [H2O] [H2](O2) Ke b) [H2O]2 [H2](O2) K. = c) [H2O]2 [H2]2(O2) Ke d) [H2[02] [H2O]2 e) K.OWLV2 | Online teaching and I X + ow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take K [Review Topica] [References] ts (M) Use the References to access important values if needed for this question. M) The equilibrium constant, K„, for the following reaction is 2.74 at 1.15×10³K. M) 2SO3(g) 2SO2(g) + O2(g) M If an equilibrium mixture of the three gases in a 13.7 L container at 1.15×10°K contains S0z at a pressure of 1.17 atm and atm. SO2 at a pressure of 1.47 atm, the equilibrium partial pressure of O2 is
- Hame Tools Document Sign in 1L ontainec Contain o.4mul.ol Hz Brg in the reaction reached state Ke for meel equal to 0.25 M. Calculate the Concentration of Constitucnts? A Ciute SDE 425 K temperature the quilibrium d-0.4 mmel. when 4 Fila Sia L Send or Sgrature * Tand trck Sture nd e len in te nise Cletd. Use stoichiometry to determine the equilibrium [Fe3+] and [SCN-] in each test tube. y = 6170.7x - 0.0153 Solution 0.002M iron(III) nitrate in 1M nitric acid(mL) 0.002M potassium thiocyanate(mL) DI water(mL) Absorbance(A) 1 3 2 1 0.128 2 2 3 1 0.269The K. for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, 12, and H2 are 0.120 M, 0.182 M, and 0.108 M respectively, which statement is correct? H2 +l2=2HI O Q = 0.733. The reaction will proceed towards the right to reach equilibrium %3D O Q = 0.733. The reaction will proceed towards the left to reach equilibrium O Q = 0.194. The reaction will proceed towards the left to reach equilibrium %3D O Q = 0.194.The reaction will proceed towards the right to reach equilibrium %3D
- aland Veterinary. Free income tax Bailey Family Foun.. I Review | Constants | Periodic Table MISSED THIS? Read Section 16.8 (Pages 701 - 710) ; Watch KCV 16.8, IWE 16.9 Equilibrium |0.125 – 1 |0.125 So Consider the reaction [CO2][H3] [CO][H2O] K. = 102 (0.125-z)? CO (g) + H2O (g) = CO2 (g) + H2 (g) K. = 102 at 500 K Since there was no product at the start of the reaction, the final concentration of CO2 is equal to 0 + x = x. A reaction mixture initially contains 0.125 M CO and 0.125 M H2O. Part D What will be the equilibrium concentration of H2? Express the concentration in molarity to three significant figures. ? να ΑΣφ M (H2] =om/ilrn/takeAssignment/takeCovalentActivity.do?locator%=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K. for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) Calculate the equilibrium concentration of H,S when 0.362 moles of NH HS(s) are introduced into a 1.00 L vessel at 298 K. [H,S] =| M Submit Answer Retry Entire Group 8 more group attempts remaining Previous Next 9:14 PM 10/14/202 prt sc delete home end num 8. backspace lock 近Brn/takeAssignment/take CovalentActivity.do?locator=assignment-take $ Write the equilibrium constant expression, K, for the following reaction: (If either the numerator or denominator is blank, please enter 1.) 2NOBr(g) 2NO(g) + Br₂ (g) K = Submit Answ F4 % F5 [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support A MacBook Air F6 & F7 * DII F8 DD F9 13 F10 Previous * ☐ Next> Save an F
- What is the equilibrium equation for the reaction: 3 NH4NO3(s) = N20(g) + 2 H2O(/)? O A) Ke = [N2O][H2O12 %3D 6. 5- B) Kc = [N20][H2O] 8. 9. -- N20]H20]2 Kc %3D NHẠNO3] O D) K = [N20]Fill in the correct “changes” in concentration terms for the following unbalanced equations, (e.g. “+y”, “-2y”, shown in bold in the Ex.) etc, in order to establish equilibrium.NOTE: if you start with a species on the product’s side, that side must lose an amount. Const. T & P. Example: 2 SO3ó 2 SO2 + Cl2(IS balanced) “x” “x” Change: +2y -2y -y a)CH4(g) + O2(g) ó CO2(g) + H2O(g)(unbalanced) “x”“x” Change:_______________ ______ b)H2O(g) + ó H2(g) + O2(g)(unbalanced) “x” “x” Change:__________ ______The expression for K for the reaction below is 2 NaHCO3 (s) = NazCO3 (3) + CO2 (g) + H20 (g) K = (PCO2) . (PH20) O a. (PCO2) (PH2O) K = [ NAHCO; ]? Ob. к - [Рсо?) + (РH20) [ NayCO3 ]. (PCO2). (PH20) K = 2. [ NAHCO; ] Od. 1 O. K = (РCО) + (РH20)