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5 Cards in this Set
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Define lattice enthalpy |
Lattice enthalpy is the enthalpy change when one mole of an ionic compound is formed from its gaseous ions under standard conditions |
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The change that produces lattice enthalpy is spontaneous but has a negative entropy change. Why is this change able to take place spontaneously? |
Enthalpy change of H is more negative than TS |
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How do different factors affect lattice enthalpy? |
• Higher LE with a greater charge • Smaller ionic radii lead to greater LE |
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Kc =1.89. What does this value suggest about the position of equilibrium? |
As value of Kc is greater than 1, it suggests that the position of equilibrium favours the RHS towards products |
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Explain why it is difficult to predict what would happen to the position of equilibrium after both temperature and pressure is increased? 2CO(g)+2NO(g)<-> 2CO2(g)+N2 (g) H = -788Kj/mol |
Effect of temperature and pressure on equilibrium. Increased temperature shifts equilibrium to left. Increased pressure shifts equilibrium to right as fewer gaseous moles on RHS |
