Hey there!
Molar mass Na2SO4 = 142.04 g/mol
Number of moles:
n = m / mm
n = 25 / 142.04
n = 0.176 moles of Na2SO4
Therefore, use the Avogadro constant
1 mole Na2SO4 ------------------- 6.02x10²³ molecules
0.176 moles Na2SO4 ------------ molecules ??
0.176 x ( 6.02x10²³ ) / 1
=> 1.059x10²³ molecules of Na2SO4
hope this helps!
C+2H2 -------> CH4
from reaction 2 mol 1 mol
from the problem x mol 10 mol
x=2*10/1 = 20 mol
Answer: 20 mol of H2.
Answer:
The solubility of a substance in water increases as the temperature rises, especially for gases.
The solubility of a substance in water with temperature generally increases for ionic solids.
Explanation:
Solid substances dissolved in liquid water, the solubility increases with temperature. Gases tend to naturally have high entropy or kinetic energy than solid substances so the same still applies.
This phenomenon is due to the increase in kinetic energy acquired by the particles of the solid at higher temperatures which allows the solvent molecules to effectively break apart the solute molecules that are held together by intermolecular attractions
Answer:
101.56 of H₂O
Explanation:
The balanced equation for the reaction is given below:
CH₄ + 2O₂ —> CO₂ + 2H₂O
Next, we shall determine the mass of CH₄ that reacted and the mass of H₂O produced from the balanced equation. This is illustrated below:
Molar mass of CH₄ = 12 + (4×1.01)
= 12 + 4.04
= 16.04 g/mol
Mass of CH₄ from the balanced equation = 1 × 16.04 = 16.04 g
Molar mass of H₂O = (2×1.01) + 16
= 2.02 + 16
= 18.02 g/mol
Mass of H₂O from the balanced equation = 2 × 18.02 = 36.04g
SUMMARY:
From the balanced equation above,
16.04 g of CH₄ reacted to produce 36.04 g of H₂O.
Finally, we shall determine the mass of water, H₂O produced by the reaction of 45.2 g of methane, CH₄. This can be obtained as illustrated below:
From the balanced equation above,
16.04 g of CH₄ reacted to produce 36.04 g of H₂O.
Therefore 45.2 g of CH₄ will react to produce = (45.2 × 36.04)/16.04 = 101.56 g of H₂O.
Thus, 101.56 of H₂O were obtained.
