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- Which of the following are variables (i.e. not constants)? (Select all that apply!) 1) rate constant (k) 2) dB/dt for the reaction A ó B 3) reaction velocity (V) 4) ∆Gactual 5) standard state equilibrium constant (Keq') 6) ∆G°’Exercises20A.1(a) Predict how the total pressure varies during the gas-phase reaction2 ICl(g)+H2(g)→I2(g)+2 HCl(g) in a constant-volume container.20A.1(b) Predict how the total pressure varies during the gas-phase reactionN2(g)+3 H2(g)→2 NH3(g) in a constant-volume container.20A.2(a) The rate of the reaction A+2 B→3 C+D was reported as2.7moldm−3 s−1. State the rates of formation and consumption of theparticipants.20A.2(b) The rate of the reaction A+3 B→C+2 D was reported as2.7moldm−3 s−1. State the rates of formation and consumption of theparticipants.20A.3(a) The rate of formation of C in the reaction 2 A+B→2 C+3 Dis 2.7moldm−3 s−1. State the reaction rate, and the rates of formation orconsumption of A, B, and D.20A.3(b) The rate of consumption of B in the reaction A+3 B→C+2 Dis 2.7moldm−3 s−1. State the reaction rate, and the rates of formation orconsumption of A, C, and D.20A.4(a) The rate law for the reaction in Exercise 20A.2(a) was found to bev=kr[A][B]. What are the units of kr…b) The equilibrium constant Keq for the reduction of nickel (II) oxide, NiO, to nickel metal at754°C is 255.4.NiO + CO Ni + CO2How would the reaction progress shift if the quantities of reagents housed in a 5.0 Litervessel, were as follows:NiO 2.5 moles Ni: 3.5 moles CO: 13.0 moles CO2 : 1.175 moles(c) If the total pressure in the vessel is 2.5 atm, find the partial pressures for CO and CO2 .
- < Progress:0/9 groups Due Apr 18 at 11:55 PM Use the References to access important values if needed for this question. In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+(aq) is pink and CoCl42-(aq) is blue. ... At Low Temperature the pink color predominates. ... ... At High Temperature the blue color is strong. ... If we represent the equilibrium as:...Co2+(aq) + 4Cl-(aq) CoCl42-(aq)We can conclude that: fill in the blank 1 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. fill in the blank 2 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. fill in the blank 3 3. When the temperature is decreased the equilibrium concentration of Co2+: A. Increases B. Decreases…A chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)Issue 5The data in the table below was compiled for the following reaction. A + B → C + D At temperature T, the following initial velocity data was obtained. Experience [A] (mol/L) [B] (mol/L) Initial speed (mol/L s) 1 0,020 0,020 5,0 x 10-3 2 0,040 0,020 1,0 x 10-2 3 0,040 0,060 4,5 x 10-2 Determine the rate law equation and the rate constant at temperature T with the appropriate units.
- pls answer d, e, f thank u 2NO(g)+O2(g)⇌2NO2(g) + Heat a) where will the reaction be shifted (right or left) if there is an increase in temperature? b) increase in pressure c) increase in volume d.) addition of catalyst e.) cooling the system f.) What happens to the concentration of NO2 if there is a decrease in pressure? g.) removal of NO2 h.) adding more O2 i.) removal of NO?A chemical equilibrium 2 A ⇄ 2B has a forward rate constant, kf = 8 M –1 s–1, and a reverse rate constant, kr = 22 s–1. If the system has a concentration of [A] = 0.22 M at equilibrium, what is the concentration of B at equilibrium? (can't be in scientific notation)II. Instruction: Writing the Reaction Quotient and Finding K for an Overall Reaction Nitrogen dioxide is a toxic pollutant that contributes to photochemical smog. One way it forms is through the following sequence: (1) N2(g) + O2(g) ↔ 2NO(g) Kc1 5 4.3x1025 (2) 2NO(g) + O2(g) ↔ 2NO2(g) Kc2 5 6.4x109 (a) Show that the overall Qc for this reaction sequence is the same as the product of the Qc expressions for the individual reactions. (b) Given that both reactions occur at the same temperature, find Kc for the overall reaction.
- For the reaction N2 + 3H2 --> 2NH3 The rate law is Rate = k[N2][H2]Which of the following will decrease the rate of the reaction. Select one: a. increasing the temperature b. increasing [N2] c. decreasing the [H2] d. both a and b e. none of these effect rateAt 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25 × 10−4. If [H2S] = 4.80 × 10−3 M and [H2] = 1.40 × 10−3 M, calculate [S2]. Please write to text formet answerIn Lab Experiment 2, you studied the following equilibrium: Fe3+(aq) + SCN–(aq) ⇌ Fe(SCN)2+(aq) If you knew the equilibrium constant K and the initial concentrations of Fe3+(aq) and SCN–(aq), what would be the simplest way to determine the equilibrium concentration of Fe(SCN)2+(aq)? A. By writing the equilibrium constant equation and solving it for [Fe(SCN)2+]equ. B. By measuring the absorbance of the equilibrium samples and using the Beer–Lambert law. C. By ensuring that SCN– is not in excess relative to Fe3+(aq). D. [Fe(SCN)2+]equ is always equal to the initial concentration of SCN–. E. By plotting the absorbance of Fe(SCN)2+(aq) versus concentration and determining the slope.