Answer:
The pressure in the gas is 656mmHg
Explanation:
In calculating the pressure of the gas;
step 1: convert the height of the mercury arm to mmHg
9.60cm = 96.0 mmHg
step 2: convert 752 torr to mmHg
I torr is 1 mmHg
752 torr = 752mmHg
Step 3: since the level of mercury in the container is higher than the level of mercury exposed to the atmosphere, we substrate the values to obtain our pressure.
So, 752mmHg - 96mmHg = 656mmHg
The pressure in the gas container is therefore 656mmHg.
N. B : if the mercury arm is in lower position, you add.
41.083 atm is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation.
Explanation:
Data given for argon gas:
number of moles = 1 mole
volume = 0.5 L
Temperature = 19 degrees or 292.15 K
a= 1.345 (L2⋅atm)/mol2
b= 0.03219L/mol.
R = 0.0821
The real pressure equation given by Van der Waals equation:
P =( RT ÷ Vm-b) - a ÷ Vm^2
Putting the values in the equation:
P = (0.0821 x 292.15) ÷(0.5 - 0.03219) - 1.345÷ (0.5)^2
= 23.98÷0.4678 - 1.345 ÷0 .25
= 51.26 - 5.38
= 45.88 atm is the real pressure.
The pressure from the ideal gas law
PV =nRT
P =( 1 x 0.0821 x 292.15) ÷ 0.5
= 4.797 atm
the difference between the ideal pressure and real pressure is
Pressure by vander waal equation- Pressure by ideal gas law
45.88 - 4.797
= 41.083 atm.is the difference between the two.
the cycle will continue until to fuel is present. that is why chain reaction occurs in a fission reaction
2 NI₃= N₂ + 3 I₂
2 x 394.71 g --------------- 3 x 253.80 g
3.58 g ---------------------- ( mass of I₂ )
3.58 x 3 x 253.80 / 2 x 394.71 =
2725.812 / 789.42 => 3.4529 g of I₂
1 mole I₂ --------------- 253.80 g
?? ----------------------- 3.4529 g
3.4529 x 1 / 253.80 => 0.0136 moles of I₂
Answer C
hope this helps!
Answer:
M.Mass = 120 g/mol
Explanation:
Data Given:
Volume = V = 0.0650 L
Temperature = T = 547 °C = 820.15 K
Pressure = P = 70.5 kPa = 0.695 atm
Gas Constant = R = 0.082057 L.atm.mol⁻¹.K⁻¹
Formula Used:
Assuming that the gas is ideally then according to ideal gas equation,
P V = n R T
Solving for n,
n = P V / R T
Putting Values,
n = (0.695 atm × 0.0650 L) ÷ (0.082057 L.atm.mol⁻¹.K⁻¹ × 820.15 K)
n = 6.71 × 10⁻⁴ moles
Now, Knowing that,
Moles = Mass / M.Mass
Or,
M.Mass = Mass / Moles
Putting values,
M.Mass = 8.06 × 10⁻² g / 6.71 × 10⁻⁴ mol
M.Mass = 120 g/mol
