Given that 6.9 moles of carbon monoxide gas are present in a container of volume

Question

Given that 6.9 moles of carbon monoxide gas are present in a container of volume 30.4L , What is the pressure of the gas (in atm) if the temperature is 62 degree C? If 2.00 g of N_2 gas has a volume of 0.40 L and a pressure of 6.0 atm, what is its Kelvin temperature? Methane gas, CH_4, is sold in a 43.8 L cylinder containing 5.54 kg. What is the pressure inside of the cylinder in kilopascals at 20 degree C? Which sample contains more moles, 3.14 L of Ar at 85.0 degree C and 1111 mmHg pressure or 11.07 g of Cl_2?

Explanation / Answer

11)PV = nRT

R = 0.0821,V = 30.4,T= 335k,n = 6.9

6.2423 ATM

Up to 13 th questions I think you solved

14)v1 = 3.14,p1=1111mmHg= 1.46atm, T 1= 358k

R= 0.082L.atmK^-1mol^-1

PV/RT = n = 1.51

For cl2 = 11.07/70=0.157 moles

AR has more moles

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