Can someone please help asap!
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The image is not given in the question, it is attached below:
<u>Answer:</u> The excess reactant is NO, the limiting reactant is CO and the products are shown in the image attached below.
<u>Explanation:</u>
In the given image:
Red spheres represent oxygen atoms, blue spheres represent nitrogen atoms and black spheres represent carbon atoms
The combination of 1 black and 2 red spheres will represent carbon dioxide compound
The combination of 2 blue spheres will represent nitrogen molecule
The combination of 1 blue and 1 red sphere will represent nitrogen monoxide compound
The combination of 1 black and 1 red sphere will represent nitrogen monoxide compound
Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.
Excess reagent is defined as the reagent which is left behind after the completion of the reaction.
We are given:
Given moles of NO = 6 moles
Given moles of CO = 4 moles
For the given chemical equation:
By stoichiometry of the reaction:
If 2 moles of CO reacts with 2 moles of NO
So, 4 moles of CO will react with = of NO
As the given amount of NO is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.
Thus, CO is considered a limiting reagent because it limits the formation of the product.
Hence, the excess reactant is NO, the limiting reactant is CO and the products are shown in the image attached below.
Answer:
Explanation:
Hello!
In this case, since the equation for the ideal gas is:
For each gas, given the total volume, temperature (28.1+273.15=301.25K) and moles, we can easily compute the partial pressure as shown below:
Best regards!