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guajiro [1.7K]
3 years ago
14

In the reaction of 3NO2 + H2O + NO + 2HNO3, if 6.0 moles of NO2 are present how many moles of NO are produced?

Chemistry
1 answer:
mina [271]3 years ago
5 0

Answer:

we can use ratio to find the moles of NO first we have to make the balance equation

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What is one molar volume of the gas ammonia (nh3) at stp?
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Gaseous butane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 1.74 g of butane is
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Answer : The mass of CO_2 produced will be, 5.3 grams.

Explanation : Given,

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First we have to calculate the moles of C_4H_{10} and O_2.

\text{Moles of }C_4H_{10}=\frac{\text{Mass of }C_4H_{10}}{\text{Molar mass of }C_4H_{10}}=\frac{1.74g}{58g/mole}=0.03moles

\text{Moles of }O_2=\frac{\text{Mass of }O_2}{\text{Molar mass of }O_2}=\frac{11g}{32g/mole}=0.34moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

2C_4H_{10}+13O_2\rightarrow 8CO_2+10H_2O

From the balanced reaction we conclude that

As, 2 moles of C_4H_{10} react with 13 mole of O_2

So, 0.03 moles of C_4H_{10} react with \frac{13}{2}\times 0.03=0.195 moles of O_2

From this we conclude that, O_2 is an excess reagent because the given moles are greater than the required moles and C_4H_{10} is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of CO_2.

As, 2 moles of C_4H_{10} react to give 8 moles of CO_2

So, 0.03 moles of C_4H_{10} react to give \frac{8}{2}\times 0.03=0.12 moles of CO_2

Now we have to calculate the mass of CO_2.

\text{Mass of }CO_2=\text{Moles of }CO_2\times \text{Molar mass of }CO_2

\text{Mass of }CO_2=(0.12mole)\times (44g/mole)=5.3g

Therefore, the mass of CO_2 produced will be, 5.3 grams.

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