Answer:
you did not show the options
Explanation:
If you double the concentration of A, the rate is doubled. If you doubled the concentration of B, since the rate law has B^2, the rate is multiplied by 4. If you double both A & B's concentrations, then the rate would be multiplied by 2*4 = 8, which is the last option.
Answer:
15.41.
Explanation:
- From the balanced equation:
<em>2SO₂(g) + O₂(g) ⇄ 2SO₃(g).</em>
<em />
The equilibrium constant = Keq = [SO₃]²/[SO₂]²[O₂].
<em>∴ Keq = [SO₃]²/[SO₂]²[O₂]</em> = (0.56 mol/L)²/(0.344 mol/L)²(0.172 mol/L) = <em>15.41.</em>
Answer:
Equilibrium constant Kc for the reaction will be 1.722
Explanation:
O2(g)+NO(g)→CO(g)+ NO2(g)
0.88 3.9 --- ---
0.88x 3.9-x x x
GIVEN:
0.88X-X= 0.11
⇒ X=0.77
CO2(g)+NO(g) → CO(g) + NO2(g)
0.88 3.9 --- ---
0.88-x 3.9-x x x
= 3.13 0.77 0.77
=0.11
Kc = ![\frac{[CO] *[NO2]} {[CO2]*[NO]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BCO%5D%20%2A%5BNO2%5D%7D%20%7B%5BCO2%5D%2A%5BNO%5D%7D%20)
=
= 1.722
