Answer:
![[N_2]=0.0866M](https://tex.z-dn.net/?f=%5BN_2%5D%3D0.0866M)
Explanation:
Hello there!
In this case, in agreement to the chemical reaction, it is possible for us to figure out the equilibrium concentration of the N2 product, via an ICE table plugged in the equilibrium expression:
![Kc=\frac{[N_2][O_2]}{[NO]^2}\\\\2.4x10^3=\frac{x*x}{(0.175-2x)^2}](https://tex.z-dn.net/?f=Kc%3D%5Cfrac%7B%5BN_2%5D%5BO_2%5D%7D%7B%5BNO%5D%5E2%7D%5C%5C%5C%5C2.4x10%5E3%3D%5Cfrac%7Bx%2Ax%7D%7B%280.175-2x%29%5E2%7D)
In such a way, when solving for x via quadratic equation or just a solver, it is possible to obtain:
In such a way, since the root 0.0884 M produce a negative concentration of NO (0.175-2*0.0884=-0.0018M), we infer that the correct root is 0.0866 M; therefore, the concentration of N2 at equilibrium is equal to x:
![[N_2]=x=0.0866M](https://tex.z-dn.net/?f=%5BN_2%5D%3Dx%3D0.0866M)
Best regards!
Electrons because the amount of valence electrons determines the bonds it can form and often times during a chemical bond or the forming of a compound an element will lose some of its electrons.
Answer:
=60 milligrams
Explanation:
12 x 5
=60 milligrams
Have a nice day!!!!!!! :-)
<u>KA</u>
Atmospheric
pressure<span>, sometimes also called barometric pressure, is the pressure exerted by the weight of air in
the </span>atmosphere of Earth<span> (or that of another planet)</span>
1 atm is equivalent to = 101325
Pa
= 760 mmHg
= 760 torr
= 1.01325 bar
So 1.23 atm is equal to
= 124629.8 Pa
= 934.8 mmHg
= 934.8 torr
<span>= 1.2462 bar</span>
Answer:
The volume of 0.80 grams of O2 is 0.56 L
Explanation:
Step 1 : Data given
Mass of O2 = 0.80 grams
Molar mass of O2 = 32 g/mol
STP = 1 mol, 1atm, 22.4 L
Step 2: Calculate moles of oxygen
Moles of O2 = Mass of O2 / molar mass of O2
Moles O2 = 0.80 grams / 32 g/mol
Moles O2 = 0.025 moles
Step 3: Calculate volume of O2
1 mol = 22.4 L of gas
0.025 moles = 0.025*22.4L = 0.56 L
The volume of 0.80 grams of O2 is 0.56 L
