Solid Ca:(PO4)2 is placed into 10.0 L of water. When equilibrium is established, the concentration of Ca²+ is 2.3 × 10 4 M. What is Kc for this equilibrium? Cas(PO4)2 (s) = 3 Ca²+ (aq) + 2 PO43- (aq)

A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =

reaction K Br(aq) + AgNO3(aq) → KNO3(aq) + AgBr(s) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) 2NaClO₂ (s) 2NaCl (s) + 30₂ (g) 2 HBr(aq) + NaOH(aq) → NaBr(aq) + H,O (1) 00000000000000 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X 000 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base Ś

Consider the reaction, PCI5(g) = PCI3(g)+ Cl2(g) where the value for Kc is 5.1 x 10- 5. The initial concentration of PCI5 is 1.16 M. What is the concentration (molarity) of PCI3 at equilibrium? Report your answer to two decimal places using scientific notation. X ÷ T ab ab () ?

N₂(g) + 3H₂(g) = 2NH₂ (g) In the Haber process, A mislabeled tank pumps happens to the equilibrium? in extra ammonia. what

For the steam hydrocarbon reforming process, the equilibrium law expression is [CO₂(g)][H₂(g)]* [CH][H₂0² Kc The reaction described by this equilibrium is CH4 (a) + H₂O(g) = CO₂(g) + H₂(g) CH4 (q) + 2H₂O(g) = CO₂(g) + 4H₂(g) CO₂(g) + 4H₂(g) = CH₁ (a) +2H₂O(g) CO₂(g) + H₂ (a) CH4 (q) + H₂O(g)

The preparation of cis-platin [Pt(NH 3) 2CI 2], an anticancer drug, uses an equilibrium reaction: K 2PECI 4(aq) + 2NH 3(aq) = 2 KCI(aq) + Pt(NH 3) 2CI 2(aq). Which of the following conditions would lead to an increase in the amount of Pt(NH 3) 2CI 2 formed? The use of a low concentration of NH3 The addition of a large concentration of KCI The use of a large concentration of NH3 The use of a stoichiometric ration of K2PTCI4 and NH3

Can you help me with this question, please? Which one is the answer right?

Consider the following equilibria: 2SO3(g)    2SO2(g) + O2(g)                       Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷   2NO2(g) + O2(g)                       Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g)   ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103

For the reaction 2 NO2 (g) <=> N2O4 (g),  K= 0.67. If [NO2] = 2.0 M, and the [N2O4] = 1.0 M  , which of the following is true?     The reaction is at equilibrium     The reaction will move to the reactant side     The reaction cannot reach equilibrium     The reaction will move to the product side