# How many moles of gas are present in a gas cylinder at #18*atm# at a temperature of #123# #""^@C#?

Approx.

Using the Ideal Gas Equation as a source.

If the caretaker is allowing compressed gas cylinders to get that hot, he really needs to be beaten. I would really like to talk to him about it.

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To find the number of moles of gas present in the cylinder, you can use the ideal gas law equation:

[PV = nRT]

Where:

- (P) is the pressure in atm,
- (V) is the volume in liters,
- (n) is the number of moles of gas,
- (R) is the ideal gas constant ((0.0821 , \text{atm} \cdot \text{L/mol} \cdot \text{K})),
- (T) is the temperature in Kelvin.

First, convert the given temperature from Celsius to Kelvin:

[T(K) = T(^@C) + 273.15]

[T(K) = 123 ^@C + 273.15 = 396.15 K]

Now, rearrange the ideal gas law equation to solve for (n):

[n = \frac{PV}{RT}]

Substitute the given values:

[n = \frac{(18 , \text{atm})V}{(0.0821 , \text{atm} \cdot \text{L/mol} \cdot \text{K})(396.15 , \text{K})}]

You would also need the volume of the gas cylinder to calculate the number of moles.

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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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