I got 4.69x10^-5 which was wrong. why??
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I got 4.69x10^-5 which was wrong. why?? For the reaction below, Kc = 1.10 10-8. What...
For the reaction below, Kc = 1.10 × 10⁻⁸. What is the equilibrium concentration of OH⁻ if the reaction begins with 0.190 M HONH₂? HONH₂ (aq) + H₂O (l) ⇌ HONH₃⁺ (aq) + OH⁻ (aq)
Question 8 of 10 Submit For the reaction below, Kc = 1.10 x 10-4. What is the equilibrium concentration of C if the reaction begins with 0.200 MA and 0.750 MB? 2 A (aq) + B (aq) = C (aq) 123 +/- 0 x 100 Tap here or pull up for additional resources
For the reaction below, Kc = 9.2 x 10-5. What is the equilibrium concentration of D if the reaction begins with 0.16 M A? A (aq) + 2 B (s) = C(s) + 2 D (aq)
For the reaction below, Kc = 7.2 × 10⁻⁴. What is the equilibrium concentration of NOF if the reaction begins with 0.92 M NO and 0.92 M F₂? 2 NO (g) + F₂ (g) ⇌ 2 NOF (g)
help! i got it wrong Question 14 of 62 Submit What is the pH of a 0.0380 M solution of HONH3CI (Kb of HONH2 is 1.1 x 10-8)? 3.6 1 2 3 7 +/- 8 : 9 0 +/- x 100 Tap here or pull up for additional resources
Just revisiting this question to understand why I got it wrong. Please show work Consider the reaction at 25°C: 2A (aq) B (aq) C (aq) +2D (aq) An experiment was performed with the following initial concentrations: [A] 3.00 M, [B] 3.00 M, [C] = 0.100 M, [D] = 0.800 M The reaction was allowed to proceed until equilibrium was reached at which time [A]-0.900 M What is the value of Wmax for the maximum work that could have been performed...
For the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C. Determine the initial and equilibrium concentrations of Br if the initial and equilibrium concentrations of Br2 are 5.90 × 10−3 M and 5.20 × 10−3 M, respectively. [Br]i = M [Br]e = M
How do you do these problems? I got all of them wrong and don't understand why. - 10. Which of the changes will increase the value of K, for the reaction? 2 SO2(g) + O2(g) - 2 SO3(g) AH = -200 kJ/mol A. Lowering the temperature B. Increasing the pressure (CCAdding 02 D. Removing SO, 3. Which reaction describes why the pH is not 7 for the dissolution of NaNO2 in water? ADNa+ + 2 H2O = NaOH + H2O*...
the equilibrium constant Kc for the reaction below is is 5.877×10-5 . c->d+e The initial composition of the reaction mixture is [C] = [D] = [E] = 1.995×10-3 M. What is the equilibrium concentration of C?
8. The standard cell potential (E°cell) for the reaction below is +1.10 V. Calculate the cell potential for this reaction when the concentration of [Cu2+] = 1.0 × 10-5 M and [Zn2+] = 3.5 M. Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq)