can you solve this with using RICE table? The reaction W (g) + Y (g) =2(g)...
Consider this reaction at 721 K: H2(g) + I2(g) 2HI (g) If we start with 1.00 Molar H 2 and 2.00 Molar I2, what is the equilibrium concentration of HI? Kc = 50.5 (Hint: need quadratic) 1.87 M 0.157 M 3.83 M 3.50 x 10 -4M 1.04 x 10 -3M 8.67 x 10 -6M 0.604 M 5.80 M
For the following reaction at 600 °C: 2502(g) + O2 (g) = 2SO3(g) Kc = 4.32 What are the equilibrium concentrations of all species in a mixture that was prepared with (SO3) = 0.500 M, [SO2] = 0 M. and [02] = 0.350 M? My I.C.E table for 2SO2 (g) + O2 (g) = 2803(g) Initial concentration Change Equilibrium OM +2x 0+2x 0.350 M +x 0.350+x 0.500 M -2x 0.500-2x I know that what ever side has zero the reaction...
the reaction between oxygen and nitrogen gases at high temperatures contribute to air pollution: N2(g) + O2 = 2 NO ; Kc 1.0*10^-5 at 1500 K ; suppose air has [N2] = 0.080 M and [O2] =0.020 M what is the concentration of NO at equilibrium (do it using small x approximation and don't use quadratic formula)
When determining the equilibrium concentrations for the reaction AB(g) = A(g) + B(g) Kc = [A][B] [AB] a simplifying assumption can be used under certain conditions to avoid solving a quadratic equation. Kc = [AB] – [AB] Classify each situation by whether the simplifying assumption can be used or whether the quadratic formula is required. Simplifying assumption can be used Quadratic formula required (AB) - 0.0168 M, K. = 2.26 x 10-6 (AB) = 0.154 M, K. = 2.72 x...
Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of CS2 is 0.15 M, what is the equilibrium constant (Kc) for the reaction.Hint: You might need an I.C.E. Table for this one. please show work
Please help with this question 5. Using the Reaction, Initial, Change, Equilibrium (RICE) table started for calculating equinor concentrations of the reaction shown. what is the expression for the equilibrium constant 2NOCI(g) S 2NO(g) + Cl2(g) [NOCIJ [NO] (C12] 0.20 M OM ом NOCH N ICHT d. 2 + (0.2-2x) e. 4x² (0.2–2x)2 x3 (0.2-x)? 4x 4x3 (0.2x)
QUESTION 2 Ammonia is produced industrially using an equilibrium reaction between hydrogen and nitrogen. The table to the right shows the equilibrium constant values at various temperatures during the reaction. Use this table to answer the following questions. Do not include units. N2 (9) + 3 H2 (9) #2 NH3 (9) 1) Which reaction (forward / reverse / neither) is being favored at a temperature of 300°C? T("C) Kc 25 6.4 x 102 2) Which temperature would be most favorable...
quick!!!!!! Given the reaction at 300K: 2A(g) = 3B(g) + C(g) Kc = 5.5 x 10-5. If 12.0 moles of A is added to a 3.0L container (hint, you need molarity not moles in your ICE table), what will the concentration of A be at equilibrium? Neglect x for this problem. Report your answer to 2 significant figures. Answer: 3.8
can someone help me ? 2) At a given temperature, the Keg for the reaction 2HI(g) + H2(g) + 12 (g) is 1.4 x 10-2 If the concentration of both Hz and Iat equilibrium is 2 x 10*M, find the equilibrium concentration of HI (hint: you don't need an ICE table for this). (2 points if all correct) 3) 0.035 moles of SO2, 0.500 moles of So,Cl2, and 0.080 moles of Cl, are combined in an evacuated 5.00 L flask...
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration of HI (g) at equilibrium if the initial concentration of each substance is 0.0600 M and the reaction mixture is allowed to come to equilibrium. (Hint: ICE Table)