The dipole moment u can be calculated using the formula
U = rq
Where u represents the dipole moment
R indicates the bond length
Q = 1.6x10-19 C
Hence,
R = u/q
R = (0.797 d) ( 3.34x10^-30 Cm/ 1
d) /( 1.6x10^-19 C)(0.118)
R = 1.41x10^-10 m
<span>R = 141 pm</span>
Answer:
Explanation:
Considering the reaction: 2X + 3Y = 3Z, combining 2.00 moles of X with 2.00 moles of Y results in the production of 1.75 moles of Z.
2 mol 2 mol 1.75 mol
2X + 3Y = 3Z
2 mol is required with 3 mol to yield 3 mol.
3 mol Z / 3 mol Y = 1 to 1
should yield 2 mol Z
1.75 / 2 = 87.5 % production yield
Answer: Option (a) is the correct answer.
Explanation:
Under conditions of low pressure and high temperature, gas molecules exhibit negligible attractions or repulsions among themselves. Hence, gases behave ideally in these scenarios.
Conversely, at low temperatures, there is a reduction in the kinetic energy of gas molecules, while high pressure compels the molecules to be closer together.
Thus, attractive forces emerge between molecules in conditions of low temperature and high pressure, causing gases to be termed real gases.
Therefore, we conclude that the ideal gas law becomes less accurate when pressure increases and temperature decreases.
Greetings,
The number of lone pairs of electrons in a C2O molecule is...
4
Each Oxygen atom forms two bonds with Carbon.
I hope this was useful!
-Char
Hello, in this situation, the chemical reaction occurring is as follows: Next, we will ascertain the limiting reactant by calculating the moles of magnesium oxide produced from 3.86 g of magnesium and 155 mL of oxygen using the given mole ratios of 2:1:2 and applying the ideal gas equation, demonstrating that oxygen is the limiting reactant because it generates the least magnesium oxide. Subsequently, we determine the mass of magnesium consumed solely by the oxygen.
