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A 430 mL container of nitrogen gas is at a pressure of 600 mmHg.
If the temperature is held constant, what volume container would
be needed if the pressure were lowered to 500 mmHg? NOTE: You
must show your calculation on the attached scratch paper, including which of the Gas Law formulas you used.
A. 358 mL
B. 516 mL
C. 698 mL
D. need more information
(Show your work please)

A 430 mL container of nitrogen gas is at a pressure of 600 mmHg If the temperature is held constant what volume container would be needed if the pressure were l class=

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dsdrajlin

Answer:

B. 516 mL

Explanation:

Step 1: Given data

  • Initial volume of the gas (V₁): 430 mL
  • Initial pressure of the gas (P₁): 600 mmHg
  • Final volume of the gas (V₂): ?
  • Final pressure of the gas (P₂): 500 mmHg

Step 2: Calculate the final volume occupied by the gas

If we assume constant temperature and ideal behavior, we can calculate the final volume of the nitrogen gas using Boyle's law.

P₁ × V₁ = P₂ × V₂

V₂ = P₁ × V₁ / P₂

V₂ = 600 mmHg × 430 mL / 500 mmHg = 516 mL

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