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------------------------------------------------ How many moles of helium occupy a volume of 5.00 L at 227.0°C and 5.00 atm? (R = 0.0821 atm•L/mol•K)

A. 25.0 mol
B. 5.00 mol
C. 0.609 mol
D. 1.64 mol
E. 6090 mol

To calculate the number of moles, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

To determine the number of moles, we can use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Given:

P = 5.00 atm

V = 5.00 L

T = 227.0°C = (227.0 + 273) K = 500 K (converting to Kelvin)

Now, we can rearrange the ideal gas law equation to solve for the number of moles:

n = (PV) / (RT)

Substituting the given values into the equation:

n = (5.00 atm * 5.00 L) / (0.0821 atm·L/(mol·K) * 500 K)

Calculating this expression gives the number of moles, which is approximately 0.609 mol.

Therefore, the correct option is c) 0.609 mol.

To know more about ideal gas law, refer here:

brainly.com/question/30458409

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