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_(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 "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_3at27^@C when its volume is 5 litre in van der Waals equation ? (a=4.17, b = 0.03711)

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) .

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.

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)).

Calculate the pressure exerted by 10.2g of NH_(3) 3 dm^(3) vessel at 25^(@)C (a) using ideal gas equation (b) using van der Waals equation . The van der Waals constants are : a=4.17 dm^(6)" atm"mol^(-2),b=0.0371 dm^(3)mol^(-1)