Answer:
91.33 L
Explanation:
For an ideal gas, the product between the gas pressure and the gas volume is proportional to the absolute temperature of the gas. Mathematically:
where:
p is the pressure of the gas
V is the volume of the gas
T is the absolute temperature of the gas
For a transformation of the gas, we can write:
For the sample of krypton in this problem, we have:
(initial pressure)
(initial volume)
(initial temperature)
(final pressure, at stp)
(temperature at stp)
Therefore, the volume at stp is:
Answer:
pay attention to your teacher duck
Explanation: the answer is b height of the plant
Answer:
A solid has the molecules tightly packed together and are held in a fixed pattern.
A liquid has molecules that are packed together in a random fashion and can move freely.
A gas has molecules that are widely separated and randomly move and collide.
Explanation:
900J
Explanation:
Well, kinetic energy is expressed through the equation:
KE
=
1
2
m
v
2
m
is the mass of the object in kilograms
v
is the velocity of the object in meters per second
So, we plug in the values, which are
m
=
0.02
kg
v
=
300
m/s
And we get,
KE
=
1
2
⋅
0.02
kg
⋅
(
300
m/s
)
2
=
1
2
⋅
0.02
kg
⋅
90000
m
2
/s
2
=
900
kg m
2
/s
2
=
900J
Question 1 :
V1/T1 = V2/T2
3.0L/273K = V2/373K
To get the value of Z, cross multiply
3.0L x 373K = 273K x V2
1119 = 273V2
Divide both sides by 273
1119/273 = 273V2/273
4.10L = V2
The new volume is 4.10 liters
Question 2 :
P1/T1 = P2 /T2
P1 = 880 kPA= 880 *10^3 Pa
T1 = 250 K
T2 = 303 K
P2 =?
Substituting for P2
P2 = P1 T2/ T1
P2 = 880 kPa * 303 / 250
P2 = 266,640 kPa/ 250
P2 = 1066.56 kPa.
The new pressure of the gas is 1066.56 kPa
Question 3 :
Given that:
Volume of gas V = 4.80L
(since 1 liter = 1dm3
4.80L = 4.80dm3)
Temperature T = 62°C
Convert Celsius to Kelvin
(62°C + 273 = 335K)
Pressure P = 2.9 atm
Number of moles of gas N = ?
Apply ideal gas equation
pV = nRT
2.9atm x 4.8dm3 = n x (0.0082 atm dm3 K-1 mol-1 x 335K)
13.92 atm dm3 = nx 2.747 atm dm3 mol-1
n = 13.92/2.747
n = 5.08 moles
There are 5.08 moles of gas contained in the sample
Question 4 :
Volume of gas V = 3.47L
(since 1 liter = 1dm3
3.47L = 3.47dm3)
Temperature T = 85.0°C
Convert Celsius to Kelvin
(85.0°C + 273 = 358K)
Pressure P = ?
Number of moles of gas N = 0.100 mole
Apply ideal gas equation
pV = nRT
p x 3.47dm3 = 0.10 x (0.0082 atm dm3 K-1 mol-1 x 358K)
p x 3.47dm3 = 0.29 atm dm3
p = (0.29 atm dm3 / 3.47 dm3)
p = 0.085 atm
If 1 atm = 760 mm Hg
0.085atm = 0.085 x 760
= 64.6 mm Hg
The pressure of the gas is 64.6 mm hg