Consider the reaction:
CO(g) + 1/2 O2(g) CO2(g)
Write the equilibrium constant for this reaction in terms of the
equilibrium constants, Ka and
Kb, for reactions a
and b below:
a.) |
C(s) + O2(g) |
CO2(g) |
............. | Ka | |
b.) |
C(s) + 1/2 O2(g) |
CO(g) |
............. | Kb |
Consider the reaction: CO(g) + 1/2 O2(g) CO2(g) Write the equilibrium constant for this reaction in...
A)Consider the reaction: 1/2 N2(g) + O2(g)<->NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a.) N2O4(g) <-> 2NO2(g) Ka b.) N2(g) + 2 O2(g) <-> N2O4(g) Kb B) Consider the reaction: P(s) + 3/2 Cl2(g)<->PCl3(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a.) P(s) + 5/2 Cl2(g) <-> PCl5(g) Ka...
Write the equilibrium constant expressions for the follow- ing reactions: (a) 2 CO(g) + O2(g) 2 2 CO2(8) (b) Mg(s) + HCl(aq) 2 MgCl2(aq) + H2(8) (c) HF(aq) + H2O(l) 2 H30+(aq) + F(aq) (d) S(s) + O2(8) 2 SO2(8) e 1 11
At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g) <----> 2CO(g) +O2(g) are 1.6*10^-11 and 1.3*10^-10, respectively. a. what is the value of the equilibrium constant for the reaction: (3) CO2(g) + H2(g) <----> H2O(g) + CO(g) at this temperature? b. demonstrate how the calculations of equilibrium constants matches the calculations of dG0r when adding two reactions or more ; determine dG0r for reactions (1) and (2) and use these values in order...
Do not understand need answers Consider the reaction Write the equilibrium o nt for this reaction in terms of the eqr 1rium constants, K, and K, for reactions a and b below a.) P(s) + 5/2 Cl2(g) PCIs(g) K b.) PCl (g) + C(g)PCls(g) Kb
16. For the system CO + CO2(g) → CaCO(s) the equilibrium constant expression is a. [CO] b. 1/[CO] c. COCO/CaCO, d. Cacos/CaoCO 17. The value of K, for the reaction 2NOH). N204) is 1.52 at 319 K. What is the value of ko at this temperature for the reaction N04() → 2NOR ? b. 1.23 c. 5.74 x 10 d. 0.658 18. The value of Ke for the reaction C() + COX() -----2CO(g) is 1.6. What is the equilibrium concentration...
The equilibrium constant, K, for the following reaction is 55.6 at 698 K H, (B)+1(B) = 2 HI(g) Calculate the equilibrium concentrations of reactants and product when 0.359 moles of H, and 0.359 moles of lare introduced into a 1.00 L vessel at 698 K [Hz] - M (HI) - Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is Al(s) + 3/2 Bry(1) AlBry(8) We could also write...
Consider the reaction below. 2 CO (g) + O2 (g) ?? 2 CO2 (g) Given :Kc = 0.7 at 2000 *C What is ?Go rxn for this reaction at 2000 *C ?
Consider the following reaction at equilibrium for which ΔH ° = –283.0 kJmol-1: 2 CO(g) + O2(g) → 2 CO2(g). Predict the change in the partial pressure of CO2 as O2 is removed from the reaction vessel at constant pressure and temperature.
The following endothermic reaction is at equilibrium. 2 CO(g) + O2(g) 42 CO2 (g) What is the effect of the following changes on the position of the equilibrium? a) CO2 (g) is removed no shift b) The volume of the container is decreased by a factor of 2. shifts to make more product c) The temperature is decreased. shifts to make more products d) CO (g) is added no shift e) He (g) is added and the pressure doubles shifts...
Consider the four reactions listed below for the next question. 1. FeO(s)+CO(g)<->Fe(s)+Co2(g) K=0.403 2. 2C(s)+O2(g)<->2CO(g) K=1x10at16 power 3. 2Cl2(g)+2H2O(l)<->4HCl(aq)+O2(g) K=1.9x10 at-15 power 4. C(s)+2H2(g)<->CH4(g) K=27.5 a.Which reaction has the smallest tendency to occur? 1. Reaction a 2. Reaction b 3. Reaction c 4. Reaction d