Answer:- 324.3 grams.
Solution:- We have been given with 6.0 moles of nitrous acid and asked to calculate it's grams. Moles to grams is a unit conversion and for doing this conversion we multiply the given moles by the molar mass of the compound.
Molar mass is the formula mass and to calculate this the atomic masses of each atom are multiplied by their respective subscripts that is the number of the atom in the compound .
For example, 
has one nitrogen atom and one oxygen atom. So, the molar mass of this is = atomic mass of N + 2(atomic mass of O)
= 14 + 2(16)
= 14 + 32
= 46 gram per mol
gram per mol is the unit of molar mass. So, the molar mass of is 46 grams per mol.
Let's calculate the molar mass of nitrous acid using the same concept.
molar mass of [
= 1 + 14 + 2(16)
= 1 + 14 + 32
= 47 grams per mol
Now, 6.9 moles of nitrous acid could easily be converted to grams as:
= 324.3 g
Hence, the mass of 6.9 moles of nitrous acid is 324.3 grams.
Answer:
You can view more details on each measurement unit: molecular weight of CaCl2 or grams This compound is also known as Calcium Chloride. The SI base unit for amount of substance is the mole. 1 mole is equal to 1 moles CaCl2, or 110.984 grams.
Answer:
yes the Bohr model predicts their spectra accurately
Explanation:
The Bohr model based on one electron system
The atom H has a single atom and the ion Be+3 has a single atom as well and this proves that the Bohr model predicts their spectra accurately .
also apply the equation model to further explain
E = 
z = atomic number
for H the value of z = 1
for Be+3 the value of z = 4
when this values are substituted into the equation above
E = 
, E = 
this results show that the energy level of Be+3 is higher than the energy level of H by a factor of 16 , and this shows that their line patterns are similar
Answer:
8.25 moles
Explanation:
Given parameters:
Number of moles of Al produced = 11 moles
Unknown:
Number of moles of oxygen produced = ?
Solution:
To solve this problem, we need to understand the problem.
The decomposition of an aluminium oxide must has produced oxygen and aluminium,
2Al₂O₃ → 4Al + 3O₂
now since the known is the oxygen gas; we can find the unknown aluminium:
3 mole of O₂ was produced with 4 mole of Al
x mole of O₂ will be produced with 11 moles of Al
x = 
= 8.25 moles
Answer:
The final pressure is approximately 0.78 atm
Explanation:
The original temperature of the gas, T₁ = 263.0 K
The final temperature of the gas, T₂ = 298.0 K
The original volume of the gas, V₁ = 24.0 liters
The final volume of the gas, V₂ = 35.0 liters
The original pressure of the gas, P₁ = 1.00 atm
Let P₂ represent the final pressure, we get;
∴ The final pressure P₂ ≈ 0.78 atm.
