Answer:
0.41 moles.
Explanation:
Given that:
Mass of helium = 4.00 g
Initial Volume = 24.4 L
initial Temperature = 25.0 °C =( 25 + 273) = 298 K
initial Pressure = 1.00 atm
The volume was reduced to :
i.e
final volume of the helium - 10.4 L
Change in ΔV = 24.4 - 10.4 = 10.0 L
Temperature and pressure remains constant.
The new quantity of gas can be calculated by using the ideal gas equation.
PV = nRT
n = 
n = 
n = 0.4089 moles
n = 0.41 moles.
Letter d, because they are both alkali metals (group one)
Answer:
P(total) = 1329 torr
Explanation:
Given data:
Pressure of nitrogen = 984 torr
Pressure of carbon dioxide = 345 torr
Total pressure of system = ?
Solution:
The given problem will be solve through the Dalton law of partial pressure of gases.
According to the this law,
The total pressure exerted by the mixture of gases is equal to the sum of partial pressure of individual gas.
Mathematical expression,
P(total) = P₁ + P₂ +.......+ Pₙ
Here we will put the values in formula,
P₁ = partial pressure of nitrogen
P₂ = partial pressure of carbon dioxide
P(total) = 984 torr + 345 torr
P(total) = 1329 torr
Answer:
E=hcλ or E=hν , where h is Planck's constant i.e, energy is directly proportional to frequency and inversely proportional to wavelength.
Answer:
Hydrogen has only 1 valence electron in its outermost shell.
Explanation:
