For the reaction below, Kc = 9.2 x 10-5. What is the equilibrium concentration of D...
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)
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)
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
I got 4.69x10^-5 which was wrong. why??
For the reaction below, Kc = 1.10 10-8. What is the equilibrium concentration of OH if the reaction begins with 0.220 M HONH2? HONH2 (aq) + H2O (1) = HONH3+ (aq) + OH(aq)
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?
The equilibrium constant Kc for the reaction below is is 5.155×10-5 . C <--> D + E The initial composition of the reaction mixture is [C] = [D] = [E] = 1.1110×10-3 M. What is the equallibrium concentrations of each of the species in the reaction?
Consider the Reaction A+B <--> C+D, which has an equilibrium constant, Kc = 3.4 x 10^2. If one begins a reaction by placing 0.600 moles of A in a 1.0L container as well as 0.150 moles of B, what will be the equilibrium concentrations of A, B, C, D? Write your answer in the spaces below. a. [A] = ______ b. [B] = ______ c. [C] = ______ d. [D] = ______
3) The reaction below has a Kc value of 3.64 x 10-3. What is the value of Kp for this reaction at 25°C? 2 NaN3(s) - 2 Na(s) + 3 N2(g) A) 131 B) 53.2 C) 8.90 x 10-2 D) 29.9 E) 0.613 5) Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: [N2 Jeq - 3.6 M, [O2 Jeq - 4.1 M, [N20Jeg - 3.3 * 10-18 M. 2 N2(g) + O2(g)...
What are the equilibrium concentrations? Equation
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2. (10 pts) For the reaction (aq) the equilibrium constant is Kc 3.0 x 10's at 25 oC. If the initial concentration of IHA is 0.100 M, what are the equilibrium concentrations of HA, H3o and A"?
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=5.3 Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3.55×10−3M, [H2]= 4.82×10−4M , and [I2]= 4.82×10−4M. What is the value of Kc at this temperature? b The reversible...