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3 years ago

What is the atomic mass of an atom?

Chemistry

1 answer:

Alborosie3 years ago

4 0

Answer:

1 unit

Explanation:

It is expressed as a multiple of one-twelfth the mass of the carbon-12 atom, 1.992646547 × 10−23 gram, which is assigned an atomic mass of 12 units.

1/12 * 12 = 1. I think so.

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A compound has an empirical formula of C2H6. What additional piece of evidence is needed to determine the molecular formula?

iragen [17]

I think the correct answer from the choices listed above is option A. The additional piece of information needed to determine the molecular formula would be percent composition of carbon. A molecular formula is <span>a formula that gives the number of atoms of each of the elements present in one molecule of a specific compound.</span>

3 0

4 years ago

Read 2 more answers

A certain substance X has a normal freezing point of -6.4 C and a molal freezing point depression constant Kf= 3.96 degrees C.kg

Brut [27]

Answer: $1.0\times 10^2g$

Explanation:

Depression in freezing point is given by:

$\Delta T_f=i\times K_f\times m$

$\Delta T_f=T_f^0-T_f=(-6.4-(13.6))^0C=7.2^0C$ = Depression in freezing point

i= vant hoff factor = 1 (for non electrolyte like urea)

$K_f$ = freezing point constant = $3.96^0C/m$

m= molality

$\Delta T_f=i\times K_f\times \frac{\text{mass of solute}}{\text{molar mass of solute}}\times \text{weight of solvent in kg}}$

Weight of solvent (X)= 950 g = 0.95 kg

Molar mass of non electrolyte (urea) = 60.06 g/mol

Mass of non electrolyte (urea) added = ?

$7.2=1\times 3.96\times \frac{xg}{60.06 g/mol\times 0.95kg}$

$x=1.0\times 10^2g$

Thus $1.0\times 10^2g$ urea was dissolved.

8 0

4 years ago

How many atoms are there in 5.8 mol of iron

kkurt [141]

4.0 mol. 6.02 x 10. 23 atoms. 3. How many moles are in 2.5g of lithium? 2.5 grams Li. 1 mole. = 0.36 mol. 6.9 g. 4. Find the mass of 4.8moles of iron. 4.8 moles.

5 0

3 years ago

Three samples of wood with the same volume were weighed. Sample A has a mass of 224.96 g, sample B has a mass of 0.55632 Ibs, an

san4es73 [151]

Answer:

Sample C has the highest density

Explanation:

Step 1: data given

Sample A has a mass of 224.96 grams

Sample B has a mass of 0.55632 lbs = 252.3425 grams

Sample C has a mass of 0.30648 kg = 306.48 grams

The volume is for all the sample equal

Step 2: Calculate density

We suppose the volume is 1000 mL

Density = mass / volume

Density sample A = 224.96 grams / 1000 mL = 0.22496 g/mL

Density sample B = 252.3425 grams / 1000 mL = 0.2523425 g/mL

Density sample C = 306.48 grams / 1000 mL = 0.30648 g/mL

Sample C has the highest density

6 0

3 years ago

What is the molecular formula of a compound with the empirical formula HSO4 and a formula mass of 194.13 amu?

nadya68 [22]

Answer:

Molecular formula = H₂S₂O₈

Explanation:

Given data:

Empirical formula = HSO₄

Formula mass = 194.13 amu

Molecular mass = ?

Solution:

Molecular formula = n × empirical formula

n = molar mass of the compound / empirical formula mass

Empirical formula mass = 1.008 + 32.065 + 16× 4

Empirical formula mass = 97.073

n = 194.13 / 97.073

n= 2

Molecular formula = n × empirical formula

Molecular formula = 2 (HSO₄)

Molecular formula = H₂S₂O₈

4 0

4 years ago