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What is the effect of decreasing the temperature of an exothermic reaction in equilibrium state?
What happens to the equilibrium position in a Haber process, when the pressure of the system is reduced?
In the reaction:-
2NOCl <--> 2NO + Cl2
what is the effect of roving some of NO formed ?
Write the expression for the equilibrium constant for the reaction:-
3Fe(s) + 4H2O(g) –> Fe3O4(s) + 4H2(g)
Calculate the value of K for the reaction:-
2SO3(g) + O2(g) –> 2SO3(g)
at a temperature of 1700K, given that [SO2] = 0.048M, [SO2] = 0.0284M and [O2] = 0.093M.
At a given temperature, the equilibrium constants K = 6.5 and Q = 3.3, predict the direction of the reaction.
Calculate the [ COCl ] in the equilibrium reaction
CO(g) + PCl5(g) –> PCl3(g) + COCl(g) give that [ CO ] = 0.24M, [ PCl5 ] = 0.082M and [ PCl3 ] = 0.047M and equilibrium constant is 5.2°C at a certain temperature.
If the Kc of the reaction:
N2(g) + O2(g) –> 2NO(g) at 2000°C is 4.08×10^-², calculate the value of Kp for the reaction.
Find the Kc for the reaction
NiSO4(s) + 6H2O(g) –> NiSO4.6H2O(s) at a temperature of 25°C .
If the equilibrium constant K for the reaction:
N2(g) + O2(g) –> 2NO(g) at 2000°C is 4.2, calculate the value of the equilibrium constant for the reaction below:
NO(g) –> 1/2N2(g) + O2(g).
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