Answer:
5.50 moles of magnesium oxide is 221.6742 grams
Explanation:
to do this you multiply the number of moles by the molar mass
<span>The ideal gas law.
PV=nRT
pressure x volume = moles x Faraday's constant x Temp Kelvin (C+273)
Original data
Pressure 1 atmosphere
Volume 1 liter
Temp 25C = 298K
New data
Volume 0.5 liter
pressure X
Temp 260C = 533K
P1v1T1 = P2v2T2
plug and chug.
(1)(1)(293) = (x)(0.5)(533)
Solve for X, which is the new pressure. </span>
Answer: Decreasing the temperature inside the container will decrease the pressure of a gas inside a closed cubical container.
Explanation:
According to Gay-Lussac's Law : 'The pressure of the gas increases with increase in temperature of the gas when volume of the gas is kept constant'.
At constant volume, pressure of the gas will decrease on decreasing the temperature or vice versa.
Decreasing the temperature inside the container will decrease the pressure of a gas inside a closed cubical container.
Answer:
wavelength = 6×10⁻⁷m
f = 0.5 ×10¹⁵ Hz
Explanation:
Given data:
Energy of photon = 3.2×10⁻¹⁹ J
Wavelength of photon = ?
Frequency of photon = ?
Solution:
E = h.f
f = frequency
h = planck's constant
E = energy
f = E/h
f = 3.2×10⁻¹⁹ Kg.m².s⁻²/ 6.63×10⁻³⁴ m².Kg/s
f = 0.5 ×10¹⁵ s⁻¹
s⁻¹ = Hz
f = 0.5 ×10¹⁵ Hz
Wavelength:
speed of light = wavelength × frequency
wavelength = speed of light / frequency
wavelength = 3×10⁸ m.s⁻¹ /0.5 ×10¹⁵s⁻¹
wavelength = 6×10⁻⁷m
