Question

what is the mass of a 256.0 ml sample of carbon dioxide gas at stp conditions?
how many carbon atoms are in 256.0 ml sample of carbon dioxide gas at stp?

how many atoms total are in 256.0 ml sample of carbon dioxide gas at stp?​

Answer 1

Answer:

3.047×10*23

Explanation:

dirst covert ml to gram to the co2 .for coversion of ml to gram multiply ml to the density

0.001977 is the density of co2.

0.001977×256

=0.5061 gm of co2 present in 256 ml of liquid.

to calculate atom multiply first co2 gram weight with avegedro number.

0.5061×6.022×10*23

3.047×10*23

Answer 2

The answer is as follows;

The answer is as follows; Mass of CO₂ = 0.18 grams

The answer is as follows; Mass of CO₂ = 0.18 grams Number of atoms in 18.066 × 10²¹ atoms.

GIVEN

Volume of Carbon Dioxide gas = 256.0 ml

TO FIND

• The mass of a 256.0 ml sample of carbon dioxide gas at stp conditions.

• How many atoms total are in 256.0 ml sample of carbon dioxide gas at stp?

SOLUTION

We can simply solve the above problem as follows;

We know that,

Number of moles of Carbon dioxide in 22.4l of carbon dioxide at STP = 1 mole

So;

Number of moles of moles of CO₂ in 256 ml of CO₂ =

$= \frac{1}{22.4} \times \frac{256}{1000} = 0.01mol$

We know that,

Mole = Given weight/Molecular weight

Molecular weight of CO₂ = 18 grams

Therefore,

Mass of CO₂ = 18 × 0.01 = 0.18 grams

Now,

We know that,

18 grams of CO₂ = 6.022 × 10²³ molecules of CO₂

SO,

0.18 grams of CO₂ =

$= \frac{6.022 \times {10}^{23} }{18} \times 0.18$

= 6.022 × 10²¹ molecules of CO₂

Now,

We know that,

Number of atoms in 1 molecule of CO₂ = 1 + 2 = 3 atoms

Number of atoms in 6.022 × 10²¹ molecules of CO₂ = 6.022 × 10²¹ × 3 = 18.066 × 10²¹ atoms

Hence, The answer is as follows;

• Hence, The answer is as follows; Mass of CO₂ = 0.18 grams
• Hence, The answer is as follows; Mass of CO₂ = 0.18 grams Number of atoms in 18.066 × 10²¹ atoms.

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