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AQA A Level Chemistry

What is the only way that the value of Kc or Kp for a particular equilibrium can be changed A change in temperature
"What effect does changes to any of the following have on the value of the equilibrium constant: concentration of reactants or products, a change of pressure, adding a catalyst " No Effect
"One mole of ethanoic acid reacts with one mole of ethanol at 298K. When equilibrium is reached it is found that two thirds of the acid has reacted. Calculate the value of Kc. CH3COOH(l) + C2H5OH(l) <-------> CH3COOC2H5(l) + H2O(l) " 4
What is the formula for mole fraction? "number of moles of a substance/number of moles of all substances present
What is the formula for partial pressure? "partial pressure = total pressure x mole fraction
What is formula for total pressure of a mixture of gases in terms of its partial pressure. "total pressure = sum of the partial pressures
"A mixture of 16g of O2 and 42g of N2 , exerts a total pressure of 20000 Nm-2. What is the partial pressure of each gas ? " O2 = 5000N/M2 N2 = 15000N/M2
"When nitrogen (1 mole) and hydrogen (3 moles) react at constant temperature at a pressure of 8 x 106 Pa, the equilibrium mixture was found to contain 0.7 moles of ammonia. Calculate Kp N2(g) + 3H2(g) <-------> 2NH3(g) " "1.73 x 10-14 Pa-2
"1.000 moles of PCl5 vapour are heated to 500 K in a sealed vessel. The equilibrium mixture, at a pressure of 625 kPa, contains 0.600 moles of chlorine. Calculate Kp. PCl5(g) ⇌ PCl3(g) + Cl2(g) " 352KPa
For this equilibrium 2 SO2(g) + O2(g) ⇌ 2 SO3(g) calculate Kp if pO2 = 102 kPa, pSO2 = 251 kPa, pSO3 = 508 kPa. 0.402KPa-1
"A mixture of 1.90 moles of H2 and 1.90 moles of I2 were allowed to reach equilibrium at 710 K. The equilibrium mixture was found to contain 3.00 moles of HI. Calculate Kp: H2(g) + I2(g) ⇌ 2 HI(g) " 56.3
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