Oxygen gas having a volume of 1010 cm3 at 20.7°c and 1.04 x 105 pa expands until its volume is 1570 cm3 and its pressure is 1.07 x 105 pa. find (a) the number of moles of oxygen present and (b) the final temperature of the sample.

final temperature is 469.71 K = 196.71 °C

Explanation:

Given data

volume V = 1010 cm3 = 0.00101 m³

temperature = 20.7°C  = 20.7 + 273 = 293.7 K

pressure P1 = 1.04 x 10^5 Pa

volume = 1570 cm3

pressure P2 = 1.07 x 10^5 Pa

to find out

number of moles of oxygen and   final temperature

solution

we know that for ideal gas

PV = nRT

put here all value to get n

R gas constant = 8.314472 J/mol−K  and T = 293.7 K and  V = 0.00101 m³

and P = 1.04 x 10^5

so n = ( 1.04 x 10^5  × 0.00101 ) / ( 8.314472 ×  293.7 )

n = 0.043015  moles

and

now we use equation

P1V1 /T1 = P2V2 / T2

1.04 x 10^5 × 1010  / 293.7 = 1.07 x 10^5 × 1570  / T2

T2 = 49338663  / 105040 = 469.71 K

so final temperature is 469.71 K = 196.71 °C

12000j is work done

the body's situation won't change the forces are equal opposit and on the same body