Answer:
d. Enzymes are broken down by the reactions they catalyze.
Explanation:
Answer:
1.64 moles O₂
Explanation:
Part A:
Remember 1 mole of particles = 6.02 x 10²³ particles
So, the question becomes, how many '6.02 x 10²³'s are there in 9.88 x 10²³ molecules of O₂?
This implies a division of given number of particles by 6.02 x 10²³ particles/mole.
∴moles O₂ = 9.88 x 10²³ molecules O₂ / 6.02 x 10²³ molecules O₂ · mole⁻¹ = 1.64 mole O₂
_______________
Part B needs an equation (usually a combustion of a hydrocarbon).
The metalloid that has three valence electrons is Boron~
Answer: The partial pressure of
is 1.86 atm
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as ![K_c](https://tex.z-dn.net/?f=K_c)
The given balanced equilibrium reaction is,
![PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)](https://tex.z-dn.net/?f=PCl_5%28g%29%5Crightleftharpoons%20PCl_3%28g%29%2BCl_2%28g%29)
Pressure at eqm. 0.973 atm 0.548atm x atm
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{(p_{PCl_3}\times (p_{Cl_2})}{(p_{PCl_5})}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%28p_%7BPCl_3%7D%5Ctimes%20%28p_%7BCl_2%7D%29%7D%7B%28p_%7BPCl_5%7D%29%7D)
Now put all the given values in this expression, we get :
![1.05=\frac{(0.548)\times (x)}{(0.973)}](https://tex.z-dn.net/?f=1.05%3D%5Cfrac%7B%280.548%29%5Ctimes%20%28x%29%7D%7B%280.973%29%7D)
By solving the term 'x', we get :
x = 1.86 atm
Thus, the partial pressure of
is 1.86 atm
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