推 con0415:推班代用心 大家考試加油喔~~~~~~~~ 03/31 20:30
1.純水的[H+]=1.00*10^(-7)，它的pH值等於多少？
pH = -log[H+] = -log(1.00*10^(-7)) = 7.000
2. The value of Kp for the following reaction at 500K is 1.5*10^(-5) / atm^2.
What is the value of the equilibrium constant (K) (at 500K)？
N2 (g) + 3 H2 (g) ←→ 2NH3 (g)
Kp = Kc * (RT)^(Δn)
T = 500
Δn = 2 - 4 =-2
1.5*10^(-5) = Kc *(0.082*500)^(-2)
Kc = 2.52 * 10^(-2)
ps: ←→ 這是正逆反應的符號喔
因為我打不出來就用這個代替吧 ^^"
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