Consider the exothermic reaction: SiCI_4 (g) +2H_2 O(I) SiO_2(s) +4HCI(g). At eq
ID: 485217 • Letter: C
Question
Consider the exothermic reaction: SiCI_4 (g) +2H_2 O(I) SiO_2(s) +4HCI(g). At equilibrium, 3.00 mol SiCI_4, 2.50 mol H_2 O, 1.50 mol SiO_2, and 3.00 mol HCI are present in a 50.0 L container at 25 degree C. a. Do you need to consider the volume occupied by liquid water? Justify your answer. b. Calculate the value for K_c at 25 degree C for the reaction shown above. c. Calculate the value for K_p at 25 degree C for the reaction shown above. d. If the system described by the equation above is initially at equilibrium, predict the direction of the shift in the position of equilibrium (left, right, no shift, or cannot be determined) and justify your prediction for each of the following. Temperature and container volume remain constant, except where noted. i. Some gaseous HCI is added. ii. Some gaseous SiCI_4 is removed. iii. To the container is added 0.50 mol solid SiO_2. iv. From the container is removed 1.00 mol liquid H_2 O. v. To the container is added 1.50 mol gaseous neon. vi. To the container is added 1.0 g of solid platinum to act as a catalyst. vii. Container volume is halved; temperature remains constant. viii. Temperature is raised by 10 degree C; container volume remains constant. ix. Container volume is halved and temperature is lowered by 10 degree C. x. For each of the changes shown in Part d above, what effect (decrease, increase, no effect, or cannot be determined) would there be on the value for the equilibrium constant for the reaction?Explanation / Answer
A. From the data given in 50liter of solution water present is equally to 2.5 moles. Water present = 2.5*18=45 litres.
B. Kc= [SiO2][HCL]^4/[SiCL4][H2O]^2
=1.5*4/(3*2.5)=0.8