Malakai S.

asked • 07/26/22

Gas Homework Help

Assume that you have 11.10 g of the deadly gas hydrogen cyanide, HCN. What is the volume of the gas at STP? Round your answer to the nearest hundredth of a liter without units. 

J.R. S.

tutor
Convert 11.10 g to moles and moles to liters using 22.4 L / mole
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07/27/22

Ajay K.

I am sorry J.R.S., but using 22.4L / mol as a conversion factor does not contain enough significant digits to round the answer to the nearest hundredth. You would need to use the value of 22.41 L /mol to get the correct answer.
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07/28/22

1 Expert Answer

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Ajay K. answered • 07/28/22

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First you have to determine how many moles of HCN you have using its molar mass.

11.10g HCN x 1 mole / 27.0253g = 0.41 mol HCN


Then you must use the ideal gas law equation PV=nRT and solve for volume in liters, V = nRT / P

where, n is the number of moles, n = 0.41 mol, R is the gas constant 0.08206 L atm / mol K, and T is the temperature in Kelvin. Remember that STP, standard temperature and pressure is 273.15 K and 1 atmosphere pressure, so P = 1 atm and T = 273.15 K.


Then solving for volume in liters V = [0.41 mol x (0.08206 L atm / mol K) x (273.15 K)] / 1 atm = 9.19

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J.R. S.

tutor
No need to use the ideal gas law if you know that at STP 1 mol of gas is 22.4 liters.
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07/28/22

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