In the gas phase, nitrogen dioxide is actually a mixture of nitrogen dioxide (NO2) and dinitrogen tetroxide (N2O4). If the density of such a mixture is 3.06 g/L at 74°C and 1.70 atm,calculate the partial pressures of the gases and KP for the dissociation of N2O4. Pressure of NO2: ?atm Pressure of N2O4: ?atm KP=?

Consider the following reaction:2SO3(g) 2SO2(g) + O2(g)If 8.04×10-2 moles of SO3, 0.396 moles of SO2, and 0.261 moles of O2 are at equilibrium in a 19.8 L container at 1.31×103 K, the value of the equilibrium constant, Kp, is

Consider the following reaction:2CH2Cl2(g) CH4(g) + CCl4(g)If 0.222 moles of CH2Cl2, 0.220 moles of CH4, and 0.375 moles of CCl4 are at equilibrium in a 15.3 L container at 489 K, the value of the equilibrium constant, Kp, is .

following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).

4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68

12. Consider the chemical reaction 2HCl(g) H2(g) + Cl2(g). It contains 8.0 mol HCI, 0.20 mol H₂ and 0.40 mol Cl₂ in a 1.00 L flask at equilibrium. Calculate Kc and Kp at 300. °C. for the reaction.

11. PLease refer to the attached photo. THank youuu

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