Answer:
A. increase equilibrium constant
B. decrease equilibrium constant
A. increase equilibrium constant
C. no effect
B. decrease equilibrium constant
Explanation:
The periodic table is an important but rather dry scientific tool. It lists all the chemical elements, ordered by their atomic numbers. Elements with similar behavior are grouped in the same column (called a group), with metals generally on the left and non-metals (gases) on the right. Rows are called “periods” - hence, periodic table.
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Answer:
so the reaction rate increases by a factor 6.
Explanation:
For the given equation the reaction is first order with respect to both ester and sodium hydroxide
So we can say that the rate law is
![Rate(initial)=K[NaOH][CH_{3}COOC_{2}H_{5}]](https://tex.z-dn.net/?f=Rate%28initial%29%3DK%5BNaOH%5D%5BCH_%7B3%7DCOOC_%7B2%7DH_%7B5%7D%5D)
now as per given conditions the concentration of ester is increased by half it means that the new concentration is 1.5 times of old concentration
The concentration of NaOH is quadrupled means the new concentration is 4 times of old concentration.
The new rate law is
![Rate(final)=K[1.5XNaOH][4XCH_{3}COOC_{2}H_{5}]](https://tex.z-dn.net/?f=Rate%28final%29%3DK%5B1.5XNaOH%5D%5B4XCH_%7B3%7DCOOC_%7B2%7DH_%7B5%7D%5D)
the final rate = 6 X initial rate
so the reaction rate increases by a factor 6.