Hey there!
* Converts 1750 dm³ in liters :
1 dm³ = 1 L so 1750 dm³ = 1750 liters
* Convertes 125,000 Pa in atm :
1 Pa = 9.86*10⁻⁶ atm so 9.86*10⁻⁶ / 125,000 => 1.233 atm
* Convertes 127ºC in K :
127 + 273.15 => 400.15 K
R = 0.082 atm.L/mol.K
Finally, it uses an equation of clapeyron :
p * V = n * R * T
1.233 * 1750 = n * 0.082 * 400.15
2157.75 = n * 32.8123
n = 2157.75 / 32.8123
n = 65.76 moles
hope this helps!
65.62 moles of an ideal gas if it occupies 1750 dm3 under 125,000 Pa at a temperature of 127 C.
Ideal gas is defined as one for which both the volume of molecules and forces between the molecules are so small that they have no effect on the behavior of the gas.
Example:
Ideal gases are nitrogen, oxygen, hydrogen and all noble gases some heavier gases like carbon dioxide and mixtures such as air also act as an ideal gas.
The ideal gas equation is formulated as PV= NRT in this equation:
Pressure of air = 1.23atm
Volume of gas = 1750dm3 = 1750 liter
R (gas constant)= 0.0820atm x Liter/ mole x kelvin
Temperature of gas =127C = 273+127 = 400K
1.23atm x 1750L = n x 0.0820atm x Liter/ mole x kelvin x 400K
n = 2152.5 / 32
n = 65.62 mole
65.62 moles of an ideal gas if it occupies 1750 dm3 under 125,000 Pa at a temperature of 127 C.
Learn more about ideal gas, Here:
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