Question

Question 1
If a gas at 25.0 °C occupies 5 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 4 atm?
Group of answer choices

a.)5L

b.)20L

c.)1.25L

d.)9L

e.)6L


Question 2
A gas occupies 20 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 80.0 mm Hg?
Group of answer choices

a.)60L

b.)2L

c.)4L

d.)10L

e.)20L


Question 3
What needs to be true about the temperature of a gas to apply boyle's law?
Group of answer choices

a.)It needs to increase in temperature

b.)Temperature doesn't matter

c.)It needs to decrease in temperature

d.)Temperature needs to stay the same

Question 4
What pressure is required to compress 200 liters of air at 1.00 atmosphere into a cylinder whose volume is 20.0 liters?
Group of answer choices

a.)20 atm

b.)220atm

c.)10atm

d.)1 atm

e.)4000amt


Question 5
A gas occupies 60 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg?
Group of answer choices

a.)60L

b.).666L

c.)40L

d.)100L


Question 6
If the starting pressure of a gas is 100 atm and it has a volume of 5 ml then what would the volume be if the pressure was lowered to 1 atm?
Group of answer choices

a.)105ml

b.)20ml

c.)500ml

d.)100ml

e.)95ml


Question 7
If the pressure pushing in on a gas doubles what would happen to the volume that the gas take up?
Group of answer choices

a.)It would double

b.)It would stay the same

c.)It would increase

d.)It would cut in half


Question 8
________ Law describes the relationship between pressure and volume.
Group of answer choices

a.)Gay-Lussac's

b.)Ideal

c.)Boyles

d.)Charles


Question 9
In the equation P1V1=P2V2 what do the numbers mean?
Group of answer choices

a.)1 is the lowest and 2 is the highest

b.)1 is the starting and 2 is the ending

c.)they tell you haw much pressure and volume there is

d.)They don't mean anything


Question 10
Which of these is a measure of how much force is applied to an object from gas particle bouncing into it?
Group of answer choices

a.)Volume

b.)Density

c.)Pressure

d.)Force


Question 11
Calculate the decrease in temperature (in Celsius) when 2.00 L at 21.0 °C is compressed to 1.00 L.
Group of answer choices

a.)147.0 K

b.)169,0 K

c.)125.0 K

d.)110.1 K


Question 12
600.0 mL of air is at 20.0 °C. What is the volume at 60.0 °C?

(Hint: Convert Celsius to Kelvin first)

Group of answer choices

a.)670 mL

b.)550 mL

c.)695 mL

d.)682 mL


Question 13
A sample of gas occupies 3 L at 300 K. What volume will it occupy at 200 K?
Group of answer choices

a.)2 L

b.)3 L

c.)1 L

d.)4 L


Question 14
A sample of oxygen occupies a volume of 1.6 L at 91°C. What will be the temperature when the volume of oxygen is reduced to 1.2 L?

(Hint: Convert Celsius to Kelvin first)

Group of answer choices

a.)373 K

b.)273 K

c.)190 K

d.)270 K


Question 15
________ Law describes the relationship between temperature and volume.
Group of answer choices

a.)Ideal Gas

b.)Gay-Lussac's

c.)Boyles

d.)Charles



WHOEVER ANSWERS FIRST IS THE BRAINLIEST

Answer 1

1. 1.25 L

2 idk but it is not 4L

3. Idk

4. 10atm

5. 40L

6. 500ml

7. It would cut in half

8. Bottles

9. C

10. Pressure

11.-126 degrees C

12. 682ml

13. 2L

14. 273 k

15. Charles

Answer 2

Answer:

1 ) Option c : 1.25

2) Option d : 10 L

3) Option d: Temperature needs to stay the same.

4) Option c: 10 atm

5) Option c : 40L  

6) Option c : 500ml

7) Option d : It would cut in half.

8)Option c : Boyles law

9) Option b : 1 is the starting and 2 is the ending

10)Optionc : Pressure

11)Option a : 147.0

12)Option d : 682mL

13)Option a :2 L

14)Option b : 273 K

15)Charles

Explanation:

According to Boyles Law, at constant temperature, volume of gas is inversely propotional to the pressure exerted by the gas.

Or the product of pressure and volume occupied by gas is constant at isothermal conditions.

                                  $P_1 V_1 = P_2 V_2$

1) Given, $V_1$ = 5L $P_1$= 1 atm $P_2$= 4atm

  $V_2 = \frac{P_1V_1}{P_2}$

        = $\frac{5X1}{4}$= 1.25L

2) Given $V_1$ = 20L $P_1$= 40 mmHg $P_2$= 80 mmHg

    $V_2 = \frac{P_1V_1}{P_2}$

         = $\frac{20X40}{80}$ = 10L.

4) Given $V_1$ = 200L $P_1$= 1 atm $V_2$= 20L

    $P_2 = \frac{P_1V_1}{V_2}$

        = $\frac{200X1}{20}$= 10atm.

5) Given $V_1$ = 60L $P_1$= 40 mmHg $P_2$= 60 mmHg

     $V_2 = \frac{P_1V_1}{P_2}$

         = $\frac{60X40}{60}$ = 40L

6)Given $V_1$ = 5L $P_1$= 100 atm $P_2$= 1 atm

    $V_2 = \frac{P_1V_1}{P_2}$

         = $\frac{100X5}{1}$ = 500 ml

7) Given $P_2 = 2 P_1$

We have according to Boyle's Law; $P_1V_1 = P_2V_2$

                 $P_1V_1=2P_1 V_2$

therefore  $V_2 = \frac{V_1}{2}$; volume cuts in half.

9)   $P_1V_1 = P_2V_2$ where subscripts 1 and 2 are before and after. That is $P_1$ is starting pressure and $P_2$ is pressure at end.

10)The measure of how much force is applied to an object for a  gas particleto  bounce back into it is called pressure.

Pressure may also be defined as the force per unit area.

According to Charle's law,Volume occupied by fixed amount of gas is directly propotional to absolute temperature in which pressure remains constant.

Or, $\frac{V}{T}$ = constant.

11)Here given $V_1 = 2 L$   $T_1 = 21^{0} C$ = 294 K    $V_2 = 1L$

                   $\frac{V_1}{T_1} = \frac{V_2}{T_2}$

                  $T_2 = \frac{V_2XT_1}{V_1}$= $\frac{1X294}{2}$ = 147K

Converting 147 K to Celsius, we find -126.0 °C.

Therefore a total decrease of 147.0 °C, from 21.0 °C to -126.0 °C.

12) $V_1 = 600m L$   $T_1 = 20^{0} C$ = 293 K    $T_2 = 60^oC$= 333K

                   $\frac{V_1}{T_1} = \frac{V_2}{T_2}$

               $V_2 = \frac{V_1XT_2}{T_1}$= $\frac{600X333}{293}$ = 682 mL.

13) $V_1 = 3L$   $T_1$ = 300 K    $T_2 = 200K$

                   $\frac{V_1}{T_1} = \frac{V_2}{T_2}$

               $V_2 = \frac{V_1XT_2}{T_1}$= $\frac{3X200}{300}$ = 2L

14)Here given $V_1 = 1.6 L$   $T_1 = 91^{0} C$ = 364 K    $V_2 = 1.2L$

                   $\frac{V_1}{T_1} = \frac{V_2}{T_2}$

                  $T_2 = \frac{V_2XT_1}{V_1}$= $\frac{1.2X364}{1.6}$ = 273