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Given the following equilibrium:
2 NO + O2 ↔ 2 NO2 ΔH= -27 kJ/mol
Increasing the temperature of this system will cause:
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- Consider the following equilibrium for which ∆H < 0.2 SO2 (g)+ O2 (g) ⇌ 2 SO3 (g) How will each of the following changes affect an equilibrium mixture of the three gases: (f) SO3 (g) is removed from the systemUsing any data you can find in the ALEKS Data resource, calculate the equilibrium constant x at 25.0 °c for the following reaction. N₂(g) + 3H₂(g) 2 NH3(g) Round your answer to 2 significant digits. K = 1 0 x10 XConsider the following equilibrium: N₂O₂ (g) 2NO₂ (g) 2 AG=5.4 kJ Now suppose a reaction vessel is filled with 2.57 atm of dinitrogen tetroxide (N₂O4) at 138. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. rise fall O yes no 10 FAED alo Ar
- Given the following reaction: N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) ΔH = -46.0 kJ/mol Which way will the reaction shift if the temperature is increased?The equilibrium constant for the reaction 2 N2(g) + 5 O2(g) ⇆ 2 N2O5(g) was measured at two temperatures: Temperature, K Kp 343 2.5x10−8 944 7.6x10−6 What is ΔHo for the reaction (in kJ/mol)?Consider the following reaction at equilibrium. What effect will doubling the temperature have on the system? CH4 ( + 2 02 () = CO2 (g) + 2 H2O () AH° = -882.0 kJ O No shift will occur because the volume of the system has not changed. No shift will occur because the total number of gas molecules on both sides of the chemical equation are equal. O A shift left towards reactants will occur. O No shift will occur because none of the concentrations have changed. O A shift right towards products will occur.
- Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X SNitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
- Consider the system N2(g) + 3 Cl2(g) 2 NCI3(g) AH = +232 kJ Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by each of the following. decreasing the temperature removing nitrogen trichloride gas 1. forward reaction compressing the system at constant temperature 2. reverse reaction adding chlorine gasThe steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?2 Consider the following equilibrium: A + 2 B 3C +D Are the reactants or K = 1.5 ×10³ products favored at equilibrium?