What is the pressure of `2 "moles"` of `NH_(3)` at `27^(@)C` when its voulume is `5 "litre"` in van der waals equation `(a= 4,17,b= 0.03711)`?

What is the pressure of 2 mole of NH_(3) at 27^(@)C when its volume is 5 lit. in van der Waal's equation ? (a = 4.17, b = 0.03711)

What is the pressure of 2 mole of NH_(3) at 27^(@)C when its volume is 5 lit. in can der Waal's equation ? (a = 4.17, b = 0.03711)

What is the pressure of 2 mole of NH_3at27^@C when its volume is 5 litre in van der Waals equation ? (a=4.17, b = 0.03711)

The van der Waals constants for CO_(2) are a = 0.37 N- m^(4) //m o l^(2) and b = 43 xx 10^(-6) m^(3) // m o l . What is the pressure exerted by the gas at 0^(@)C , for a specific volume of 0.55 litre // mole, assuming Van der Waals equation to be strictly true? Also calculate the pressure under the same condition, assuming CO_(2) as an ideal gas.

A quantity of 2 mol of NH_(3) occupies 5L at 27^(@)C . Calculate the pressure of the gas using the van der Waals equation if a = 4.17 "atm "L^(2)" mol"^(-2) and b = 0.3711 L "mol"^(-1) .

What do the constants a and b signify in van der Waals' equation ?

Write the van der Waals equation for 5 mole of ideal gas.

Two moles of ammonia were found to occupy a volume of 5 L at 27^(@)C . Calculate the pressure using van der Waals equation (a="4.17 bar L"^(2)"mol"^(-2), b="0.0371 L mol"^(-1)).