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3 years ago

A gas has a volume of 4.54 L at 1.65 atm and 75.0°C. At what pressure would the volume of the gas be increased to 5.33 L if the

Chemistry

1 answer:

gladu [14]3 years ago

6 0

Answer:

The new pressure is 1,52 atm

Explanation:

We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T. We convert the unit Celsius into Kelvin:

75°C=273+75=348K ; 103°C=273+103=376K

(P1xV1)/T1=(P2xV2)/T2

(1,65atm x4,54L)/348K= (P2x 5,33L)/376K

0,0215 atmxL/K=(P2x 5,33L)/376K

P2=(0,0215 atmxL/K x 376K)/5,33l= 1,52 atm

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3 years ago

At 20 âˆ˜C the vapor pressure of benzene C6H6 is 75 torr and that of toluene C7H8 is 22 torr. Assume that benzene and toluene fo

Olegator [25]

Answer:

a) Xbenzene = 0.283

b) Xtoluene = 0.717

Explanation:

At T = 20°C:

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3 years ago

A gas has an initial volume of 455 mL at 105ºC and a final volume of 235 mL. What is its final temperature in Celsius degrees?

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Hello!

To solve this problem we're going to use the Charles' Law. This Law describes the relationship between Volume and Temperature in an ideal gas. Applying this law we have the following equation:

$\frac{V1}{T1} = \frac{V2}{T2} \\ \\ T2= \frac{V2*T1}{V1}= \frac{235 mL * 105 ^{\circ}C }{455 mL}=54,23 ^{\circ}C$

So, the final temperature is 54,23 °C

Have a nice day!

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