Consider the following reaction and its equilibrium constant: CH4(g)+ NH3(g)↔HCN(g)+ 3 H2(g)Kc= 15 A reaction mixture contains 0.33M CH4, 0.022M NH3,0.55M HCN and 1.0M H2. Which of the following statements is true concerning this system?
a. The reaction will shift in the direction of products.
b. Kcwill decrease.
c. The reaction quotient, Qc, will decrease.
d. The system is at equilibrium

Please explain how to do this

The activity series is shown in the attached picture. if the element is below the other, then you can displace the other. following the activity series as a guide, the reactions are as follows: nickel and aluminum chloride3 ni + 2 alcl₃  → 3 nicl₂ + 2 albarium and copper bromideba + cubr  →  no reaction because cu is less oxidizable than bapotassium nitrate and aluminum3 kno₃ + al  → al(no₃)₃ + 3 ksodium phosphate and zincnaso₄ + zn  → znso₄ + na

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Ibelieve the answer is d. titaniumhope my answer has you : )

Naoh + hbr -> nabr (salt) + h2o ca (oh)2 + 2hbr - - - > ca (br)2 + 2h2o