61.24 is the molar mass of a gas which has a density of 0.00249 g/mL at 20.0 degrees celcius and 744.0 mm Hg.
Explanation:
given that:
density = 0.00249 g/ml (
) or 2.49 grams/litre
P = 744 mm Hg OR 0.978 atm
T = 20 Degrees or 293.15 Kelvin
R = 0.08206 Litre atm/mole K
molar mass =?
Formula used/
PV = nRT equation 1
here n is number of moles:
n = 
putting the value of n and value of density in the equation 1:
PV = 
x RT
molar mass = x 
= density x
= 
= 61.24 is the molar mass of the gas.
Answer:
the volume delivered by the pipette = 22.32 mL
Explanation:
To calculate this, let us first note that the density of water relates it weight and its volume (density = mass ÷ volume), hence we are going to use density to determine the volume.
Density of water = mass/volume = 0.997 g/ mL
mass = 22.25g
Density = 0.997g/mL
volume = ?
∴ the volume delivered by the pipette = 22.32 mL
<em>Please note that this calculation is based on the fact that the weight of the empty flask has been determined and canceled out.</em>
Answer:
323.15 °C
Explanation:
Considering the ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Thus, at constant volume and number of moles, Pressure of the gas is directly proportional to the temperature of the gas.
P ∝ T
Also,
Using Charle's law
Given ,
P₂ = 2P₁
T₁ = 25 °C
T₂ = ?
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (25 + 273.15) K = 298.15 K
Using above equation as:
New temperature = 596.3 K
Also,
T(K) - 273.15 = T( °C)
<u>So, Temperature = 596.3 - 273.15 °C = 323.15 °C</u>
Answer:atomic number 10 noble gas
Explanation:
