Air is mainly composed of N2 (78%), O2 (21%) and other trace gases. Now, the total pressure of air is the sum of the partial pressures of the constituent gases. The partial pressure of each gas, for example say O2, can be expressed as:
p(O2) = mole fraction of O2 * P(total, air) ----(1)
Thus, the partial pressure is directly proportional to the total pressure. If we consider a sealed container then, as the temperature of air increases so will its pressure. Based on equation (1) an increase in the pressure of air should also increase the partial pressure of oxygen.
Answer:
The relationship between the volume and temperature of a given amount of gas at constant pressure is known as Charles's law in recognition of the French scientist and balloon flight pioneer Jacques Alexandre César Charles.
Explanation:
Answer:
4.7K
Explanation:
Given parameters:
Initial volume = 75L
Initial pressure = 125psi
to atm gives 8.5atm
Initial temperature = 288K
New volume = 6.1L
New pressure = 25psi
to atm gives 1.7atm
Unknown:
New temperature = ?
Solution:
To solve this problem, we use the combined gas law which is given below:
= 
P, V and T are pressure, volume and temperature
1 and 2 are initial and new states
= 
T2 = 4.7K
Answer:
The total pressure is 0,804 atm
Explanation:
We use Dalton's law according to which the sum of the partial pressures is equal to the total pressure of a gas mixture. We convert the pressure in Pascals to atmosphere (it can also be done in reverse):
101300Pa ----1 atm
4500Pa----x= (4500Pa x 1atm)/101300Pa= 0,044 atm
P total= p1 + p2= 0,76 atm + 0,044 atm=0,804 atm
Answer:
well it turns into N3H12PO4
Explanation:
