A sample of nitrogen gas has a pressure of 6.58 kPa at 539K. If the volume does not

change, what will the pressure be at -62°C.

2.58 kPa  

Step-by-step explanation:

Initial Pressure of the nitrogen gas = 6.85 kPa

Initial temperature of the nitrogen gas  539 K

Final Pressure of the nitrogen gas = ???

Final Pressure of the nitrogen gas = -62°C = (273+(-62))K

= 211 K

∴  The equation that can be used to approach this question relating to pressure and temperature at a fixed constant volume is Gay-Lussac's Law of Combine Volume. The expression for Gay-Lussac's Law is given as:

Thus, the pressure will be 2.58 kPa  at -62°C

Step-by-step explanation:

The formula to be used is:

P1/T1=P2/T2

At constant volume,we have

P1=6.58

P2=x(it wasn't given)

T1= 539

T2= -62°c(convert to kelvin:Celsius value + 273= {-62+273}= 211

6.58/539=X/211

Cross multiply and we have

X= 211×6.58/539

X=2.58 kPa

180

step-by-step explanation:

12-2=10

20-2=18

18x10=180

first anwser choice.

step-by-step explanation:

the greater/less or equal to symbol (> or < with the line at the bottom) is a closed/filled in circle.

-5c + 2 _< _27

subtract from both sides by 2

-5c _< _ 27

divide both sides by -5

c _< _ 5.4

flip the inequality sign

c _> _5.4

the only possible answer that would match the simplified inequality is the first answer choice