1) LDA, THF, -78 °C 2) heptanal 3) NH4CI, H₂O

None

part c?

Using the following equations, determine each of the following:

11) Into a 1.00 liter flask is placed 0.822 moles of SO3. At equilibrium 36.7% of the SO3 has decomposed. What is the value of the equilibrium constant? 2 SO3 (g) « 2 SO2 (g) + O2 (g)​​​Kc = ?

please see attached image

Br NO₂ (1) NaOH, 70 °C (2) H3O*(quench)

HF(g) + H,O(1) H,0*(aq)+ F"(aq) K = 1.1 x 10-3 F (aq) + HF(g) HF;(ag) K= 2.6 x 10- a. Is fluoride in pH 7.00 drinking water more likely to be present as F"(aq) or HF2 (aq)? O HF2 (aq) O F(aq) b. What is the equilibrium constant for this equilibrium? Number 2 HF(g) + H,0(1) H,0*(aq) + HF, (aq) c. What are the pH and equilibrium concentration of HF2" in a 0.150 M solution of HF? (HF, - Number Number pH = M Check Answer View Solution

How will the equalibrium shift? Heat + N2 (g) + 3O2 (g) <----> 2NO (g) a) how will it shift with an addition of NH3 b) how will it shift with increase in pressure?

4