The partial pressures of an equilibrium mixture of N2O4(g) and NO2(g) are PN2O4 = 0.34 atm and PNO2 = 1.20 atm at a certain temperature. The volume of the container is doubled. Calculate the partial pressures of the two gases when a new equilibrium is established.
Answer to relevant QuestionsFor the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) at 600. K, the equilibrium constant is 11.5. Suppose that 2.450 g of PCl5 is placed in an evacuated 500 mL bulb, which is then heated to 600. K. a. What would the pressure of ...Consider the decomposition of the compound C5H6O3 as follows: C5H6O3(g) → C2H6(g) + 3CO(g) When a 5.63-g sample of pure C5H6O3(g) was sealed in an otherwise empty 2.50- L flask and heated to 200oC, the pressure in the ...A mixture of N2, H2 and NH3 is at equilibrium according to the equation N2(g) + 3H2(g) ⇌ 2NH3(g) as depicted below. The volume is suddenly decreased (by increasing the external pressure), and a new equilibrium is ...A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred: 2FeSO4(s) ⇌ Fe2O3(s) + SO3(g) + SO2(g) SO3(g) ⇌ SO2(g) + ½O2(g) After equilibrium was reached, the ...Consider the following reaction: 2H2(g) + O2(g) → 2H2O(l) ΔH = –572 kJ a. How much heat is evolved for the production of 1.00 mole H2O(l)? b. How much heat is evolved when 4.03 g hydrogen is reacted with excess ...
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