Answer:

Explanation:
Hello,
In this case, we can use the ideal gas equation:

So we know the temperature, pressure and volume, therefore we can easily compute the required moles as shown below:

Best regards.
Answer : All of the above are valid expressions of the reaction rate.
Explanation :
The given rate of reaction is,

The expression for rate of reaction for the reactant :
![\text{Rate of disappearance of }NH_3=-\frac{1}{4}\times \frac{d[NH_3]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20disappearance%20of%20%7DNH_3%3D-%5Cfrac%7B1%7D%7B4%7D%5Ctimes%20%5Cfrac%7Bd%5BNH_3%5D%7D%7Bdt%7D)
![\text{Rate of disappearance of }O_2=-\frac{1}{7}\times \frac{d[O_2]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20disappearance%20of%20%7DO_2%3D-%5Cfrac%7B1%7D%7B7%7D%5Ctimes%20%5Cfrac%7Bd%5BO_2%5D%7D%7Bdt%7D)
The expression for rate of reaction for the product :
![\text{Rate of formation of }NO_2=+\frac{1}{4}\times \frac{d[NO_2]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20formation%20of%20%7DNO_2%3D%2B%5Cfrac%7B1%7D%7B4%7D%5Ctimes%20%5Cfrac%7Bd%5BNO_2%5D%7D%7Bdt%7D)
![\text{Rate of formation of }H_2O=+\frac{1}{6}\times \frac{d[H_2O]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20formation%20of%20%7DH_2O%3D%2B%5Cfrac%7B1%7D%7B6%7D%5Ctimes%20%5Cfrac%7Bd%5BH_2O%5D%7D%7Bdt%7D)
From this we conclude that, all the options are correct.
Reaction Rate is the rate at which a substance undergoes a chemical change.
Answer:
The answer to your question is M = 36.49 g
Explanation:
Data
mass = 8.21 g
volume = 4.8064 L
Temperature = 200°C
Pressure = 1.816 atm
M = ?
Process
1.- Convert temperature to °K
°K = 273 + 200
°K = 473
2.- Calculate the number of moles
n = (PV)/RT
n = (1.816)(4.8064)/(0.082)(473)
n = 0.225
3.- Calculate the molar mass
M --------------- 1 mol
8.21 g ---------- 0.225 moles
M = (1 x 8.21)/0.225
M = 36.49 g
Because in difrent materials atoms are more compact or less compact.if they are less compact then it will be easear for them to move