Answer:
C. 548mL
Explanation:
Attached is an image of the explanation. Hope this helps!
Notice that " s o 4 " appears in two different places in this chemical equation. s o 2− 4 is a polyatomic ion called "sulfate."
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<u>Answer:</u> The mass of nitric oxide is 12.72 grams
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For ammonia:</u>
Given mass of ammonia = 8.00 g
Molar mass of ammonia = 17 g/mol
Putting values in equation 1, we get:
- <u>For oxygen gas:</u>
Given mass of oxygen gas = 17.0 g
Molar mass of oxygen gas = 32 g/mol
Putting values in equation 1, we get:
The given chemical reaction follows:
By Stoichiometry of the reaction:
5 moles of oxygen gas reacts with 4 moles of ammonia
So, 0.53 moles of oxygen gas will react with = of ammonia
As, given amount of ammonia is more than the required amount. So, it is considered as an excess reagent.
Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
5 moles of oxygen gas produces 4 moles of NO
So, 0.53 moles of oxygen gas will produce = of NO
Now, calculating the mass of NO from equation 1, we get:
Molar mass of NO = 30 g/mol
Moles of NO = 0.424 moles
Putting values in equation 1, we get:
Hence, the mass of nitric oxide is 12.72 grams