A container holds 100.0 mL of nitrogen at 21° C and a pressure of 736 mm Hg. What will be its volume if the temperature increase
1 answer:
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Answer : The correct option is, (I)
Solution : Given,
Mass of NO = 45.8 g
Mass of = 12.4 g
Molar mass of NO = 30 g/mole
Molar mass of = 2 g/mole
Molar mass of = 17 g/mole
First we have to calculate the moles of NO and .
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 mole of react with 5 mole of
So, 1.53 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
From the reaction, we conclude that
As, 2 mole of react to give 2 mole of
So, 1.53 mole of react to give 1.53 mole of
Now we have to calculate the mass of
Therefore, the maximum mass of produced 26.0 grams.
A phospholipid structure is shown in the picture attached. It has three parts: the hydrophobic tail, the hydrophilic head and the phosphate group in the center. Thus, the function of the phosphate group is to link the hydrophobic and hydrophilic parts of a phospholipid. Specifically, the phosphate group is part of the hydrophilic head. So, it is used to connect the phospholipids to polar compounds.
