Consider the following reaction that occurs between hydrochloric acid, HCI, and
ID: 500118 • Letter: C
Question
Consider the following reaction that occurs between hydrochloric acid, HCI, and zinc metal: HCI_(aq) + Zn_(s) rightarrow H_2 (g) + ZnCI_2 (aq) Will this reaction occur fastest using a 6 M solution of HCI or a 0.5 M solution of HCI? Explain Again consider the reaction between hydrochloric acid and zinc. How will increasing the temperature affect the rate of the reaction? Explain. Based on the following kinetic energy curves, which reaction will have a faster rate - A or B? Explain. Also, which reaction, A or B, would benefit most in terms of increased rate if the temperature of the system were increased? Which of the following reactions will have the fastest rate? The slowest? a) 2C_12 H_26 (s) + 37 O_2 (g) rightarrow 24 CO_2 (g) + 36 H_2 O (g) b) S_2 O_8^2- (aq) + 2 I^- (aq) rightarrow 2 SO_4^2- (aq) + I_2 (s). c) Ba^2+ (aq) + SO_4^2- (aq) rightarrow BaSO_4 (s) White phosphorus reacts immediately and rapidly with oxygen when exposed to air. What an you say about the amount of activation energy required for this reaction?Explanation / Answer
1) The reaction is fastest with 6M HCl because as the concentration of reactant increases the reaction moves towards faster.
2) The temperature will effect the rate of reaction.As the teperature increases the splitting of HCl increases and the kinetic energy of reactants also increases so the rate of reaction increases.
3) A , because the kinetic energy is more
4) reaction (c) is fastest because the reactants are aqueous ions they will react fast
reaction (a) is slowest because C12H26 is the solid so reaction will be slow for the solid as the reactant.