# If 1 mole of H2 gas was collected under 294.2K and 746.7 mmHg, what volume will it occupy?

Well,

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Using the ideal gas law equation (PV = nRT), where:

- (P) is the pressure (in atmospheres)
- (V) is the volume (in liters)
- (n) is the number of moles
- (R) is the ideal gas constant (0.0821 L·atm/mol·K)
- (T) is the temperature (in Kelvin)

Given:

- (n = 1 \text{ mole})
- (T = 294.2 \text{ K})
- (P = 746.7 \text{ mmHg})

First, we need to convert pressure from mmHg to atm: [ P = 746.7 \text{ mmHg} \times \frac{1 \text{ atm}}{760 \text{ mmHg}} = 0.981 \text{ atm} ]

Now, rearranging the ideal gas law equation to solve for volume ((V)): [ V = \frac{nRT}{P} ]

Substituting the given values: [ V = \frac{(1 \text{ mol})(0.0821 \text{ L} \cdot \text{atm/mol} \cdot \text{K})(294.2 \text{ K})}{0.981 \text{ atm}} ]

[ V = 24.53 \text{ L} ]

Therefore, 1 mole of H2 gas collected under 294.2 K and 746.7 mmHg will occupy approximately 24.53 liters.

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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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