# How many moles of nitrogen gas will occupy a volume of 347 mL at 6680 mmHg and 27 #"^o#C?

Moreover, we employ the Ideal Gas Equation:

What is the mass of the nitrogen gas quantity?

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To calculate the number of moles of nitrogen gas, we can use the ideal gas law:

PV = nRT

Where: P = pressure (in atmospheres) V = volume (in liters) n = number of moles R = ideal gas constant (0.0821 L.atm/mol.K) T = temperature (in Kelvin)

First, we need to convert the given pressure from mmHg to atm and the volume from milliliters to liters. Then, we can solve for the number of moles.

Given: Pressure (P) = 6680 mmHg Volume (V) = 347 mL Temperature (T) = 27°C = 27 + 273 = 300 K

Converting units: Pressure (P) = 6680 mmHg * (1 atm / 760 mmHg) = 8.79 atm Volume (V) = 347 mL * (1 L / 1000 mL) = 0.347 L

Now, plugging the values into the ideal gas law equation:

8.79 atm * 0.347 L = n * 0.0821 L.atm/mol.K * 300 K

Solving for n (number of moles): n = (8.79 atm * 0.347 L) / (0.0821 L.atm/mol.K * 300 K) n ≈ 0.130 moles

So, approximately 0.130 moles of nitrogen gas will occupy a volume of 347 mL at 6680 mmHg and 27°C.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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