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12345 [234]
3 years ago
10

A gas occupies a volume of 2.67 Times 10 to the square root of two mL at 542.48 mm Hg pressure. What will be its volume at const

ant temperature if the pressure is changed to 778.05MM Hg
Chemistry
1 answer:
Ratling [72]3 years ago
3 0

Answer:

<u>The volume of the gas at constant temperature is:</u>

<u>186.16 mL</u>

Explanation:

Byole's Law : <u><em>The pressure exerted by the fixed amount of gas is inversely proportional to Volume at the constant temperatur</em></u>e.

P=k\frac{1}{V}

Here k = proportionality constant

PV= k

If P1 and V1 are initial pressure and Volume of gas and P2 , V2 are final volume of the gas , Then :

P_{1}V_{1}=P_{2}V_{2}

P1 = 542.48 mm Hg

V_{1} =2.67\times 10^{2}mL

P2 = 778.05 mm Hg

Insert the values of P1 , V1 and P2 in formula and calculate V2

P_{1}V_{1}=P_{2}V_{2}

542.48\times 2.67\times 10^{2}=778.05V_{2}

dividing the equation by 778.05

V_{2}=\frac{542.48\times 2.67\times 10^{2}}{778.05}

542.48\times 2.67\times 10^{2}mL= 144842.16

V_{2}=\frac{144842.16}{778.05}

V_{2}=186.16mL

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Explanation:

  • We can use the general law of ideal gas: <em>PV = nRT. </em>

where, P is the pressure of the gas in atm (P = 1.0 atm, Standard P).

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