Answer:
The entropy change for a real, irreversible process is equal to <u>zero.</u>
The correct option is<u> 'c'.</u>
Explanation:
<u>Lets look around all the given options -:</u>
(a) the entropy change for a theoretical reversible process with the same initial and final states , since the entropy change is equal and opposite in reversible process , thus this option in not correct.
(b) equal to the entropy change for the same process performed reversibly ONLY if the process can be reversed at all. Since , the change is same as well as opposite too . Therefore , this statement is also not true .
(c) zero. This option is true because We generate more entropy in an irreversible process. Because no heat moves into or out of the surroundings during the procedure, the entropy change of the surroundings is zero.
(d) impossible to tell. This option is invalid , thus incorrect .
<u>Hence , the correct option is 'c' that is zero.</u>
I uploaded the answer to a file hosting. Here's link:
tinyurl.com/wpazsebu
Answer: There are 
of gas are in a container with a volume of 9.55 mL at 35 °C and a pressure of 895 mmHg
Explanation:
According to ideal gas equation:
P = pressure of gas = 895 mm Hg= 1.18 atm (760 mm Hg= 1 atm)
V = Volume of gas = 9.55 ml = 0.00955 L (1 L=1000ml)
n = number of moles = ?
R = gas constant =
T =temperature =
Thus there are of gas are in a container with a volume of 9.55 mL at 35 °C and a pressure of 895 mmHg
Because they can't get trapped in.
