Astudent collects 285 ml of o2 gas at a temperature of 15°c and a pressure of 0.983 atm. the next day, the same sample occupies 292 ml at a temperature of 11°c. what is the new pressure of the gas? 0.946 atm 1.00 atm 0.704 atm

According to the combined gas laws,

Plugging in the values and solving for the final pressure:

Final pressure

-

0.946 atm

Explanation:-

From the question we see,

First day pressure P 1 = 0.983 atm

First day temperature T 1 =15 C + 273 = 288 K

First day volume V 1 =285 mL

Second Day volume V 2 = 292 mL

Second day Temperature T 2 = 11 C + 273 = 284 K

Using the relation

P 1 V 1 / T 1 = P 2 V 2 / T 2

We get Second Pressure P 2 = P 1 V 1 T 2 / ( T 1 V 2)

= 0.983 atm x 285 mL x 284 K / ( 288 K x 292 mL)

= 0.946 atm

Hence the new pressure of the gas on the second day is 0.946 atm

the formula for the conversion of temperature from degree celsius to kelvin is:

the sample of water at is converted to kelvin temperature by using the above formula as:

on comparing the two samples of water at or we can say that at and at respectively. the difference between the temperatures of two samples of water is:

hence, one can say that the sample of water at is greater than the sample of water at by .