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[References The equilibrium constant K, for the equation CS2 (9) + 4H, (9) CH4(9) + 2H,S(9)...
The equilibrium constant KC for the equation CS2 + 4H2 = CH4 + 2H2S at 900 °C is 27.8. What is the value of KC for the following equation? 1/5CH4 + 2/5 H2S = 1/5CS2 + 4/5H2
(References The equilibrium constant (K.) for the reaction PC13 (9) + Cl2 (9) - PCs (9) equals 49 at 230°C. If 0.372 mol each of phosphorus trichloride and chlorine are added to a 2.80 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PCL mol Cl2 mol PCL Submit Answer Try Another Version 5 Item attempts remaining
References The equilibrium constant (K.) for the reaction PC1: (9) + Cl2(g) – PC1s (9) equals 49 at 230°C. If 0.702 mol each of phosphorus trichloride and chlorine are added to a 4.50 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PC mol Cl, mol PCLS Submit Answer Try Another Version 6 item attempts remaining
[References) Use the References to access important values if needed for this question. 1 pt 1 pt Consider the following reaction: 1 pt 2CH2Cl2(g) —CH (9)+CCI(g) 1 pt 1 pt If 0.157 moles of CH,Cl2, 0.302 moles of CH4, and 0.338 moles of CCI, are at equilibrium in a 16.9 L container at 409 K, the value of the equilibrium constant, Kp, is 1 pt 1 pt 1 pt 1 pt Submit Answer Try Another Version 9 item attempts remaining...
(1). Examine the following equation and discuss the stresses and chemical shifts. CH() + 2H,S.) A CS2(g) + 4H2(g) addition of CS, gas. (b) - removal of H2S gas, (c)- addition of CH4 gas. (d) - Increased pressure. (e)- If the reaction is heated and more CS, gas is evolved. Is the reaction exo-or endo-thermic? (f) - What is the equilibrium constant (K) if the measured concentrations at equilibrium where determined to be [CH] = 0.75 M, [H2) = 1.00...
pt The equilibrium constant, K, for the following reaction is 5.03 at 395 K. pt 2CH2Cl2(8) ? CH,(g) + CCl4(g) pt pt Calculate Kat this temperature for the following reaction: pt 1/2CH (8)+1/2CC14(8) CH,Cl2(g) pt pt K. pt Submit Answer Try Another Version 2 item attempts remaining pt pt
Use the References to access in Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2 Ag+ (aq) + Fe(s) —2Ag(s) – Fe2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant AGº for this reaction would be than zero Submit Answer Try Another Version 2 item attempts remaining
Hello i need help with this, thank you s Principle [References) At a particular temperature, K = 7.0 x 10-6 for the reaction 2 CO2(g) = 2 CO(g) + O2(g) If 4.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species. (CO2) = (CO) = [02] = Submit Answer Try Another Version 9 item attempts remaining
Use the References to access important valuesit needed for this question The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2CH2(g) CH4(8) CCI(8) Calculate the equilibrium concentrations of reactant and products when 0.393 moles of CH CI are introduced into a 1.00 L vessel at 350 K. M [CH2CH2 = [CH41 (CCM) M M Submit Answer Retry Entire Group 8 more group attempts remaining
Use the References to access important values if needed for this question. Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. CH2COOH(aq) + H20(1)= H,0*(aq) + CH,COO (aq) Submit Answer Retry Entire Group 9 more group attempts remaining Write the equilibrium constant expression K for the following reaction taking place in dilute aqueous solution (CH), NH (aq) + H,01 = (CH)2NH,+ (aq) + OH+ (aq) Submit Answer Retry Entire Group 9 more group...