The pressure exerted by 0.57 moles of CO2 at a temperature of 25°C and a volume of 500 ml is 28 atm.
<u>Explanation:</u>
According to ideal gas law,
PV = nRT
where P represents the pressure of a gas,
V represents the volume of a gas,
n represents the number of moles,
R represents the gas constant = 0.0821 L atm / mol K.
T represents the temperature of a gas.
Given V = 500 ml = 0.5 l, T = 25°C = 298 K, n = 0.57 mol
PV = nRT
P = nRT / V
= (0.57 0.0821
298) / 0.5
P = 28 atm.
The pressure of a gas is 28 atm.
Answer:
2.21 x 10⁻⁷m⁻¹
Explanation:
Given parameters:
Energy of the photon = 9.02 x 10⁻¹⁹J
Unknown:
Wavelength of the photon = ?
Solution;
The wavelength and energy of a photon are related using the expression below;
E =
h is the Planck's constant = 6.63 x 10⁻⁴m²kg/s²
c is the speed of light
E is the energy
h c = E x wavelength
Wavelength = =
Wavelength = 2.21 x 10⁻⁷m⁻¹
Answer: 0.0624 atm
Explanation:-
According to the ideal gas equation:
P = Pressure of the gas = ?
V= Volume of the gas = 45.0 L
T= Temperature of the gas = -10.0°C = 263 K
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas
Moles of gas=
The pressure of sulfur hexafluoride gas in the reaction vessel after the reaction is 0.0624 atm