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hram777 [196]
3 years ago
11

When nitrogen dioxide gas dissolves in water, an aqueous solution containing dissolved nitric acid and nitrogen monoxide forms.

In terms of mass balance, 138.03 g of NO_2 completely reacts with 18.02 g of H_2O to form 126.04 g of HNO_3 and 30.01 g of NO. 3NO_2(g) + H_2O(l) rightarrow 2HNO_3(aq) + NO(aq) 1. When 359 g of NO_2 is used, how many grams of H_2O are consumed? 2. How many grams of HNO_3 are produced? 3. How many grams of NO are produced?
Chemistry
1 answer:
xeze [42]3 years ago
5 0

Answer:

1. Based on the given question, 138.03 grams of NO₂ is reacting completely with 18.02 grams of H2O. However, in case when 359 grams of NO₂ is used then the grams of water consumed in the reaction will be,  

= 359 × 18.02 / 138.03 = 46.87 grams of water.  

2. As mentioned in the given case 138.03 grams of NO₂ generates 126.04 grams of HNO₃. Therefore, 359 grams of NO₂ will produce,  

= 359 × 126.04 / 138.03  

= 327.81 grams of HNO₃.  

3. Based on the given question, 138.04 grams of NO₂ is generating 30.01 grams of NO. Therefore, 359 grams of NO₂ will generate,  

= 359 × 30.01 / 138.04

= 78.04 grams of NO.  

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Answer:

a) 1 litre of  10% solution and 7 litre of 20% solution

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Explanation:

Given:

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Solution:

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Let x be the amount of 50% solution.

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Then(10-x) be the 20% solution

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50%(x)+10%(10-x)=25%(10)

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x=\frac{1.5}{0.3}

x=3.75

Now, (10-x)=(10- 3.75)=6.26

So there will be 3.75 litres of 50% solution and 6.25 litres of 20% solution

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