Question

Calculate the pressure in atmospheres exerted by 10.0moles of hydrogen gas at 293 kelvins if it is stored in a 7.50 liter container. Your value should be a decimal number written to three significant figures. Given: R= 0.08205 liter x atmosphere/mole x kelvin

Answer 1

To determine the pressure of the gas, we need an equation which would relate pressure to the values given like the number of moles, temperature and the volume of the system. For simplicity, we can assume that the hydrogen gas is an ideal gas so we use the equation PV=nRT where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant and T is the temperature. 

PV = nRT
P = nRT / V
P = 10.0 mol  (0.08205 L - atm / mol-K) (293 K) / 7.50 L
P = 32.0542 atm

 Therefore, the pressure of the system would be 32.054 atm

Answer 2

Answer:

The correct answer is 32.1 atm. If you rearrange the ideal gas law equation to find pressure (P) and substitute the known values for the rest of the variables (n, T, and V), we get pressure equal to 32.1 atm.

Explanation:

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