Sodium chloride reacts with silver nitrate according to the following reaction, with the equal sign in place of a reaction arrow.

For the reaction below, the concentrations at equilibrium are [SO₂] = 0.60 M, [O₂] = 0.25 M, and [SO₂] = 1.6 M. What is the value of the equilibrium constant, Ke? 2 SO₂(g) + O₂(g) →→→ 2 SO₂(g) • Report your answer using two significant figures. Provide your answer below:

5) For the reaction shown below, at a particular time, the following concentrations are obtained: [CO] = 0.034 M, [CO2] = 3.6 x 10-17 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? 2 CO (g) « C (s) + CO2 (g)​​​Kc = 7.7 x 10-15

IPse_assessment_id=_2032637_1&course Remaining Time: 1 hour, 28 minutes, 28 seconds. * Question Completion Status: O Decreasing the amount of H2. QUESTION 2 *Which of the following statements about a system at chemical equilibrium is true? O The forward and reverse reactions both stop. O The forward reaction has a faster rate than the reverse reaction. O The reverse reaction has a faster rate than the forward reaction. The forward reaction rate is equal to the reverse reaction rate. O There are no more reactants left. QUESTION 3 Which statement about organic compouunds is falee? Click Save and Submit to save and submit. Click Save All Answers to save all answers. search DELL prt s

Can you help me calculate the equilibrium constant using this data? (2 data sets) equilibrium reaction: Co(H2O)62+ (aq) + 4 Cl- (aq) ⇄ CoCl42- (aq) + 6 H2O (l)

Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.

Consider the reaction 2A --> A₂. If the initial concentration of A is 4 M, and after 10 minutes the reaction appears to stop when the concentration of [A] is 2.0 M

A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.240 M, [H*] = 2.00 x 10-4 M, and [A-] = 2.00 x 10-4 M. Calculate the value of pK, for the acid HA. pKa