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- Determine Kp for the reaction shown if at equilibrium, half of the initial SO2 reacted to form 2.00 atm of SO3. The initial partial pressures of SO2 and O2 were equal. 2 SO2(g) + O2(g) 2 SO3(g) (A) 0.250 atm (B) 0.333 atm (C) 0.500 atm (D) 1.00 atmarrow_forwardAt a certain temperature, the value of the equilibrium constant, K, for the reaction represented below is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature? H2(g) + Br2(g) = 2HBr(g) (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5arrow_forwardThe equilibrium for the formation of dinitrogen tetraoxide gas (N204) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: K. = 1.7 x 10-26 at 40.0°C 2 NO2 (g) <→ N2O4 (g) What is the value of Kp at this same temperature? -25 (A) 4.4 x 10 (B) 6.6 x 10-28 (C) 5.2 x 10-27 (D) 6.5 x 10-30 (E) 5.9 x 1025arrow_forward
- 5. Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. Given that the initial pressure is 1.00 atm and at equi- librium the pressure is 0.500 atm, determine the final pressure in the reaction vessel at equilibrium. 2N2O5(g) = 4NO2(g) + O2(8) (A) 0.750 atm (B) 1.00 atm (C) 1.25 atm (D) 1.75 atmarrow_forwardChange the values of Kc to values of KP or the values of KP to values of Kc. (a)Cl2(g) + Br2(g) 2BrCl(g) Kc=4.7 x 10-2 at 25C (b)2SO2(g) + O2(g) 2 SO3(g) Kp=48.2 at 500C (c)CaCl2 x 6H2O(s) CaCl2(s) + 6H2O(g) Kp=5.09 x 10-44 at 25 C (d) H2O(l) H2O (g) Kp= .196 at 60Carrow_forward9. The equilibrium constant for the reaction 2 BrCl (g) → Br2 (g) + Cl2 (g) at 25°C is Keq = 0.0172. What is the equilibrium constant for the reaction Br2 (g) + Cl2 (g) →2 BrCl (g)? (а) -0.0172 (b) 0.131 (c) 7.62 (d) 58.1 (e) none of thesearrow_forward
- A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? No, because the value of Kc can be determined experimentally only.Yes, because the partial pressures of all the reactants and products are specified. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forwardA flask is charged with 1.600 atm of N2O4(g) and 1.06 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? Yes, because the partial pressures of all the reactants and products are specified. No, because the value of Kc can be determined experimentally only. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forwardA flask is charged with 1.720 atm of N₂O4(g) and 0.88 atm NO₂(g) at 25°C. The equilibrium reaction is given in the equation below. N₂04(9) 2NO₂(g) After equilibrium is reached, the partial pressure of NO₂ is 0.512 atm. (a) What is the equilibrium partial pressure of N₂O4? 1.904 atm (b) Calculate the value of K, for the reaction. 0.137 (c) Is there sufficient information to calculate K for the reaction? O Yes, because the partial pressures of all the reactants and products are specified. Ⓒ Yes, because the temperature is specified. O No, because the value of K. can be determined experimentally only. If K can be calculated, find the value of K. Otherwise, enter 0. 2.30e-4 Xarrow_forward
- The reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = atmarrow_forward2 NOBr(g) 2 NO(g) + Br,(g) AH = 16.1 kJ How does the equilibrium shift after the following stresses? a) Adding more Br, Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say b) Remove some NOBr Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say c) Decrease the temperature Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say What is much different about this third process compared to the first two?arrow_forwardQuestion 2 of 35 View Policies Show Attempt History Current Attempt in Progress Incorrect. At 20 °C, the following concentrations were found for the gases in an equilibrium mixture for the reaction N₂O(g) + NO₂(g) = 3NO(g) [NO₂] = 0.41 M, [NO] = 8.2 x 10-8 M, and [N₂O] = 0.025 M. What is the value of Kp for this reaction? Enter your answer in scientific notation. Kp = i 5.4 x 10 i -20 0/1 :arrow_forward
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