What is the value of 1 atomic mass unit in terms of grams?

$1.66 \times 10^{- 24} g$

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$12.66 \times 10^{- 24} g$

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$0.66 \times 10^{- 24} g$

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$0.166 \times 10^{- 23} g$

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Solution

The correct options are
A
$1.66 \times 10^{- 24} g$

D
$0.166 \times 10^{- 23} g$

AMU is the mass exactly equal to 1/12 of the mass of 1 atom of carbon 12 isotope.

Mass of one atom of carbon -12 isotope is equal to $1.9924 \times 10^{- 23} g$ .

Therefore, $1 A M U = \frac{1}{12} \times 1.9924 \times 10^{- 23}$

= $0.166 \times 10^{-}^{2}^{3} g$

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Similar questions

Gram Atomic mass is just the atomic mass expressed in grams ...ie, atomic mass with gram as units. Our book says that gram atomic mass and gram atom are the same thing (similarly for gram molecule and gram molecular mass) . But later a formula is given that : Gram atom = mass in grams / Atomic mass [RAM].

There are questions also that use this formula ( similarly for gram molecule) in which we have to find the number of "gram atoms " in a given mass of substance.

So what is the real meaning of gram atom and the formula ( and is is similar for gram molecules) ?

Question 1
If one mole of carbon atoms weighs 12 grams, what is the mass (in grams) of 1 atom of carbon?

Magnesium is two times heavier than C-12 atom, what shall be the mass of Mg atom in terms of atomic mass unit?

Q. Calculate the gram molecular mass of water from the values of gram atomic mass of Hydrogen and of Oxygen.
Gram atomic mass of Hydrogen

= 1 g

Gram atomic mass of Oxygen

= 16 g

The mass of 1-mole atoms of an element expressed in grams is called its gram atomic mass.

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What is the value of 1 atomic mass unit in terms of grams?

The correct options are A 1.66×10−24g D 0.166×10−23g AMU is the mass exactly equal to 1/12 of the mass of 1 atom of carbon 12 isotope. Mass of one atom of carbon -12 isotope is equal to 1.9924×10−23g. Therefore, 1AMU=112×1.9924×10−23 =0.166×10−23g