Answer:
2.49 × 10⁶ molecules
Explanation:
Given data
- Pressure (P): 9.25 × 10⁻¹⁴ atm
- Volume (V):
We can calculate the moles of gas using the ideal gas equation.
P × V = n × R × T
n = P × V / R × T
n = 9.25 × 10⁻¹⁴ atm × 1.10 × 10⁻³ L / (0.0821 atm.L/mol.K) × 300.0 K
n = 4.13 × 10⁻¹⁸ mol
1 mole contains 6.02 × 10²³ molecules (Avogadro's number). The number of molecules in 4.13 × 10⁻¹⁸ moles is:
4.13 × 10⁻¹⁸ mol × (6.02 × 10²³ molecule/1 mol) = 2.49 × 10⁶ molecule
Okay so, 24.00 mL of a 0.25 M NaOH solution is titrated.
Answer:
M = 0.177
Explanation:
First, we have to find the molar mass of potassium iodine (KI).
K = 39.098
I = 126.904
Now, add these values together to get the molar mass of KI
39.098 + 126.904 = 166.0028
Now, it's time to do a grams to moles conversion.
35.0 g KI * 
= 
= 0.212 mol KI
Now, we can find the molarity of this solution.
Molarity (M) = 
M = 
= 0.177 M
The molarity (M) of this solution is 0.177.
Answer:
The atomic number of Nitrogen is seven. So it contains seven protons and seven electrons in neutral form. Also, the electronic configuration cited above contains seven electrons among which two electrons are present in first shell and five electrons are present in valence shell respectively.
Explanation:
