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inessss [21]
1 year ago
6

How many moles of NO2 form when 63.25 g N2O5 decompose? 2N2O5→ 4NO2 + 0₂

Chemistry
1 answer:
GREYUIT [131]1 year ago
7 0

Answer:

1.1713 moles

Explanation:

RFM of N2O5= (14*2)+(16*4)=108

Moles of N2O5= Mass/RFM= 63.25/108= 0.5856 moles

Mole ratio of N2O5:NO2 = 2:4

Therefore moles of NO2= 4/2*0.5856= 1.1713 moles

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Answer: The correct answer is option B i.e., 2.78 mol

Explanation:

Aluminium reacts with iodine to form Aluminium iodide

$2Al(s)+3I_{2}(s) \to Al_{2}I_{6}(s)$

From the equation, it is clear that 3 moles of iodine reacts with 2 moles of Aluminium to form Aluminium iodide

We know $No.\,of\,moles=\frac{weight}{molecular\,weight} \\

For 2 moles of Aluminium, $2=\frac{weight}{27}$\\ $weight=2 \times 27=54g$

3 moles of Iodine reacts with 54 g of Aluminium

? moles of iodine react with 50 g of Aluminium

$=\frac{3 \times 50}{54} =2.78 mol$

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3 years ago
The initial pressure and volume of a gas are 55.16 kilopascals and 0.500 liter. According to Boyle’s law, if the volume of the g
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P2 = 55.16*0.5/0.8

P2 = 34.48kPa

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3 years ago
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