The reaction of ethyl acetate with sodium hydroxide, ch3cooc2h5(aq)+naoh(aq)⇌ch3coona(aq)+c2h5oh(aq) is first order in ch3cooc2h
5 and first order in naoh. if the concentration of ch3cooc2h5 was increased by half and the concentration of naoh was quadrupled, by what factor would the reaction rate increase? express your answer numerically.
This problem involves the rate law of a chemical reaction relates the concentrations or pressures of the reactants with the rate of reaction together with some constant parameters. In this problem, we turn this into a mathematical problem by first assigning variables to the reactants.
Let:
x = concentration of ethyl acetate, [CH<span>3COOC2H5] </span>y = concentration of sodium hydroxide, [NaOH]
The rate law is then equal to rate = xy since the reaction is first order in both reactants. It was then said that <span>the concentration of ethyl acetate was increased by half and the concentration of NaOH was quadrupled. In mathematical form, this translates to the following expression: </span> rate = 0.5x*4y = 2xy
Thus, the reaction rate increased by a factor of 2.
In this case, according to the given chemical reaction, it is possible for us to calculate the produced grams of nitrogen monoxide by starting with 25.0 g of nitrogen via their 1:2 mole ratio and the molar masses of 30.1 g/mol and 28.02 g/mol, respectively and by some stoichiometry: