# A 425 mL volume of hydrogen chloride gas, #HCl#, is collected at 25°C and 720 torr. What volume will it occupy at STP?

The volume at STP will be 370 mL, rounded to two significant figures.

Since your question involves the pressure, volume, and temperature of HCl gas, you will need to use the combined gas law in order to solve this problem. Temperature will need to be converted to Kelvins and pressure will need to be converted to kPa.

The current value for STP as determined by the IUPAC (International union of Pure and Applied Chemistry), is

Known

Unknown

Rearrange the equation in order to isolate

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Using the combined gas law and the ideal gas law, we can calculate the volume of HCl gas at STP.

Given: Initial volume (V₁) = 425 mL Initial temperature (T₁) = 25°C = 298 K Initial pressure (P₁) = 720 torr

STP conditions: Standard temperature (T₂) = 0°C = 273 K Standard pressure (P₂) = 1 atm = 760 torr

Using the combined gas law: (P₁ * V₁) / T₁ = (P₂ * V₂) / T₂

Substituting the values: (720 torr * 425 mL) / 298 K = (760 torr * V₂) / 273 K

Solving for V₂ (volume at STP): V₂ = (720 torr * 425 mL * 273 K) / (760 torr * 298 K) V₂ ≈ 391.6 mL

Therefore, the volume of hydrogen chloride gas at STP would be approximately 391.6 mL.

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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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