# A #0.275*L# volume of an unspecified gas exerts a pressure of #732.6*mm*Hg# at a temperature of #-28.2# #""^@C#. What is the molar quantity of this gas?

Approx.

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To find the molar quantity of the gas, you can use the ideal gas law equation:

PV = nRT

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

First, convert the pressure from mmHg to atm and the temperature from Celsius to Kelvin:

732.6 mmHg * (1 atm / 760 mmHg) = 0.96447 atm -28.2°C + 273.15 = 244.95 K

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

0.96447 atm * 0.275 L = n * 0.0821 L atm / K mol * 244.95 K

Solve for n:

n = (0.96447 atm * 0.275 L) / (0.0821 L atm / K mol * 244.95 K) n ≈ 0.01129 mol

So, the molar quantity of the gas is approximately 0.01129 mol.

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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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