A 10.3 L cylinder contains 10.67 moles of Cl2 at 21.2 C. What is the pressure (atm)

Explanation:

we know that ideal gas equation is

PV=nRT

P=nRT/V

V=10.3L

n=10.67

T=21.2+273=294

R=0.0821

P=10.67*0.0821*294/10.3

P=25.00atm

P = 25.0 atm

Explanation:

Given data:

Volume of gas = 10.3 L

Number of moles of Cl₂ = 10.67 mol

Temperature = 21.2 °C

Pressure of gas = ?

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

21.2+273 = 294.2 K

10.3 L × P = 10.67 mol ×  0.0821 atm.L/ mol.K  × 294.2 K

P = 257.72 atm.L /  10.3 L

P = 25.0 atm

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.