Answer:
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure. 17.5 “Temperature and Reaction Rate”).
Explanation:
Answer : The correct expression for equilibrium constant will be, ![K=[O_2]^5](https://tex.z-dn.net/?f=K%3D%5BO_2%5D%5E5)
Explanation :
Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.
The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.
As we know that the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.
The given equilibrium reaction is,
The expression of 
will be,
Therefore, the correct expression for equilibrium constant will be,
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Answer:
The answer to your question is P2 = 1.52 atm
Explanation:
Data
Volume 1 = V1 = 4.54 l
Pressure 1 = P1 = 1.65 atm
Temperature 1 = T1 = 75°C
Volume 2= V2 = 5.33 l
Pressure 2 = P2 = ?
Temperature 2 = 103°C
Process
1.- Convert temperature to °K
Temperature 1 = 75 + 273 = 348°K
Temperature 2 = 103 + 273 = 376°K
2.- Use the combine gas law to find the final pressure
P1V1/T1 = P2V2/T2
-Solve for P2
P2 = P1V1T2 / T1V2
-Substitution
P2 = (1.65 x 4.54 x 376) / (348 x 5.33)
-Simplification
P2 = 2816.62 / 1854.84
-Result
P2 = 1.52 atm
