The equilibrium of baking! (This is all made up!!!!) Baking soda undergoes therm

Question

The equilibrium of baking! (This is all made up!!!!) Baking soda undergoes thermal decomposition as follows Does this cause the cake to rise 2NaHCO_2(s) Na_2CO3(s) + CO-2(g) + H_2O(g) Write the equilibrium constant expression. Kc and Kp, for this reaction See Example 14.1 If K_c = 1.56 times 10^1 at 956 degree C. calculate K_p at this temperature See Example 14 4 Does this reaction lie predominately to the right or left, based on K_c? Explain Remember, reactions with K's greater than 1 will lie predominantly to the right, reactions with K's less than 1 will lie predominantly to the left What is this temperature in degree F? Is this baking temperature? What would happen if the temperature is lowered? Would this affect the equilibrium constant? How? Would it rise as much? (or at all) Does this represent a heterogeneous or homogeneous equilibria? Explain

Explanation / Answer

Kc=[Na2co3][H20][CO2]/[NaHCO3]^2

Kp=PH2O*PCO2

Kc=Kp/(RT)^2

Kp=1.56*(0.0821*1229)^2=15882.34

This reaction is predominantly to right

F=1.8C+32=1.89*956+32=1752.8F

If temperature is lowered equlibrium shifts to exists to right predominanlty

Heterogenous equilibrium

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