Find the mass of the empirical formula.
You must be given a sample of some kind to calculate the weight or know how many moles are present. Then you figure out what one mol would be. The key step is multiplying the empirical formula numbers by what it takes to make 1 mol.
It would be clearer if we were working from some choices.
Answer:
250 light minutes takes
Explanation:
1 astonomical unit is equal to 1.50x10¹¹m
The light travels at the speed of 3.0x10⁸m/s. That means in 1 second, travels 3.0x10⁸m. To solve this question we must find the distance of neptune to the sun in meters. In this way we can find the seconds (And minutes) that need the light to travel from the sun to neptune:
<em>Distance from Sun to neptune:</em>
30AU * (1.50x10¹¹m / 1AU) = 4.5x10¹²m
<em>Time transcurred:</em>
4.5x10¹²m * (1s / 3.0x10⁸m) = 15000s
15000s * (1min / 60s) =
<h3>250 light minutes takes</h3>
Answer:
The answer to your question is 100.8 g
Explanation:
Data
mass of Barium chloride = 90 g
mass of Barium sulfate = ?
Balanced chemical reaction
BaCl₂ + H₂SO₄ ⇒ BaSO₄ + 2HCl
Process
1.- Calculate the molar mass of BaCl₂ and BaSO₄
BaCl₂ = 137.3 + (2 x 35.5) = 208.3g
BaSO₄ = 137.3 + 32 + (16 x 4) = 233.3g
2.- Use proportions to find the mass of BaSO₄
208.3 g of BaCl₂ --------------------- 233.3 g of BaSO₄
90 g of BaCl₂ --------------------- x
x = (90 x 233.3) / 208.3
x = 20997/ 208.3
x = 100.8 g
3.- Conclusion
There will be produced 100.8 g of BaSO₄
The iupac name is ethylene glycol
Answer:
D metallic
Explanation:
The chemical bonding which rises from electrostatic attractive force between the conduction electrons and the positively charged metal ions is called metallic bonding.
<u>It is sharing of the free electrons among the structure of the positively charged ions which are known as cations.
</u>
<u>In this type of bonding, these free electrons freely move in the crystal mattice of the metal. </u>
The bonding accounts for properties of metals, such as ductility, strength, electrical and thermal conductivity and resistivity and luster.
