A calcium bromide compound is represented by which formula?
2 answers:
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Answer:
Approximately upwards (assuming that
.)
Explanation:
External forces on this astronaut:
- Weight (gravitational attraction) from the earth (downwards,) and
- Normal force from the floor (upwards.)
Let denote the magnitude of the normal force on this astronaut from the floor. Since the direction of the normal force is opposite to the direction of the gravitational attraction, the magnitude of the net force on this astronaut would be:
.
Let denote the mass of this astronaut. The magnitude of the gravitational attraction on this astronaut would be
.
Let denote the acceleration of this astronaut. The magnitude of the net force on this astronaut would be
.
Rearrange to obtain an expression for the magnitude of the normal force on this astronaut:
.
There are some missing data in the text of the exercise. Here the complete text:
"<span>A sample of 20.0 moles of a monatomic ideal gas (γ = 1.67) undergoes an adiabatic process. The initial pressure is 400kPa and the initial temperature is 450K. The final temperature of the gas is 320K. What is the final volume of the gas? Let the ideal-gas constant R = 8.314 J/(mol • K). "
Solution:
First, we can find the initial volume of the gas, by using the ideal gas law:
</span>
<span>where
p is the pressure
V the volume
n the number of moles
R the gas constant
T the absolute temperature
Using the initial data of the gas, we can find its initial volume:
</span>
<span>
Then the gas undergoes an adiabatic process. For an adiabatic transformation, the following relationship between volume and temperature can be used:
</span>
<span>where </span>
for a monoatomic gas as in this exercise. The previous relationship can be also written as
where i labels the initial conditions and f the final conditions. Re-arranging the equation and using the data of the problem, we can find the final volume of the gas:
![V_f = V_i \sqrt[\gamma-1]{ \frac{T_i}{T_f} }=(0.187 m^3) \sqrt[0.67]{ \frac{450 K}{320 K} }=0.310 m^3 = 310 L](https://tex.z-dn.net/?f=V_f%20%3D%20V_i%20%20%5Csqrt%5B%5Cgamma-1%5D%7B%20%5Cfrac%7BT_i%7D%7BT_f%7D%20%7D%3D%280.187%20m%5E3%29%20%5Csqrt%5B0.67%5D%7B%20%5Cfrac%7B450%20K%7D%7B320%20K%7D%20%7D%3D0.310%20m%5E3%20%3D%20310%20L%20%20)
So, the final volume of the gas is 310 L.
"<span>A sample of 20.0 moles of a monatomic ideal gas (γ = 1.67) undergoes an adiabatic process. The initial pressure is 400kPa and the initial temperature is 450K. The final temperature of the gas is 320K. What is the final volume of the gas? Let the ideal-gas constant R = 8.314 J/(mol • K). "
Solution:
First, we can find the initial volume of the gas, by using the ideal gas law:
</span>
<span>where
p is the pressure
V the volume
n the number of moles
R the gas constant
T the absolute temperature
Using the initial data of the gas, we can find its initial volume:
</span>
<span>
Then the gas undergoes an adiabatic process. For an adiabatic transformation, the following relationship between volume and temperature can be used:
</span>
<span>where </span>
where i labels the initial conditions and f the final conditions. Re-arranging the equation and using the data of the problem, we can find the final volume of the gas:
So, the final volume of the gas is 310 L.