Explanation:
Since, the given reaction is as follows.
Hence, rate law of the reaction is as follows.
R = ![k[NO][Cl_{2}]](https://tex.z-dn.net/?f=k%5BNO%5D%5BCl_%7B2%7D%5D)
As it is known that rate of a reaction depends on the initial concentration of products. So here, the rate of reaction will depend on the concentration of NO and 
. Since, power of the concentrations of each of these is equal to 1. Therefore, order of the reaction is equal to 1 + 1 = 2.
According to the rate law, reactants involved in the rate determining step are NO and . Hence, first step of the mechanism is the rate determining step.
Also, according to the rate of reaction doubling the concentration of NO will double the rate of reaction.
The number of reactants taking part in a single step of the reaction is known as molecularity of the reaction. Therefore, molecularity of the first step of the reaction is 2.
Both the given steps are not termolecular.
Answer : The complete chemical equation is,
Explanation :
As we know that, in a chemical equation the reacting species present on left side and the product formed present on right side and a right arrow inserted between the reactants and product that show a chemical reaction taking place.
In the chemical reaction, the phases of the substances are also included and subscripts and superscripts are also used for the numbers.
For the given chemical reaction, the balanced chemical equation including the phases, is given by:
Answer:
Explanation:
Hello!
In this case, since the chemical reaction between copper and nitric acid is:
By starting with 0.80 g of copper metal (molar mass = 63.54 g/mol) and considering the 1:1 mole ratio between copper and copper (II) nitrate (molar mass = 187.56 g/mol) we can compute that mass via stoichiometry as shown below:
However, the real reaction between copper and nitric acid releases nitrogen oxide, yet it does not modify the calculations since the 1:1 mole ratio is still there:
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Answer: 0.67 moles of 
Explanation:
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number 
of particles.
To calculate the moles, we use the equation:
According to stoichiometry:
3 moles of 
is produced by 2 moles of
Thus 1 mole of is produced by= 
of
Thus 0.67 moles of are required to produce 28.3 g of
