- Write the expression for Kp for the reaction below.
MgCO3(s) MgO(s) + CO2(g)
_ 2. Ozone is formed from oxygen. 3 O2(g) 2 O3(g) Calculate the value of Kp, given that Kc = 2.5 10–29 at 298 K. (R = 0.08206 Latm/molK) 3. At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask.
The H2 and I2 react according to the balanced equation below.
H2(g) + I2(g) 2 HI(g)
When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the
equilibrium constant, Kc, for the reaction?
4. The equilibrium constant (Kc) for the following reaction is 6.7 10–10 at 630 C. N2(s) + O2(g) 2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? 1/2 N2(g) + 1/2 O2(g) NO(g) _ 5. The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as
follows.
N2(g) + 3 H2(g) 2 NH3(g) H = –92.2 kJ
Given a system that is initially at equilibrium, describe 2 actions that will cause the reaction to proceed to the
left.
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