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(b) The second step in the manufacture of sulfuric acid is the conversion of SO2 into sulfur trioxide, SO3, using Equilibrium 1.
2SO2(g) + O2(g) 2SO3(g) ∆H = −197 kJ mol−1 Equilibrium 1 An industrial chemist carries out some research into Equilibrium 1.
• The chemist fills a 10.2 dm3 container with SO2(g) at RTP, and then adds 12.0g of O2(g).
• The chemist adds the vanadium(V) oxide catalyst, and heats the mixture. The mixture is allowed to reach equilibrium at a pressure of 2.50atm and a temperature of 1000K.
• A sample of the equilibrium mixture is analysed, and found to contain 0.350 mol of SO3.
(ii) Determine the value of Kp for Equilibrium 1 at 1000K.
Show all your working.
Give your answer to 3 significant figures.