Consider the following reaction at 25.0 degree Celsius. 1) If the initial concentration of [Hg(OH)2] is 0.240 M and the initial concentration of [CaCl2] is 0.55 M. Calculate the concentration of [Hg(OH)2] after 30.0 seconds. 2) If the rate constant of this reaction at 100.0 °C is 5.03 M^-1S^-1. Calculate the activation energy of this reaction in (kJ/mol).

Given the same reactant concentrations, the below reaction at 257. °C is 94.6 times as fast as the same reaction at 163. °C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant. Round your answer to 2 significant digits. co(g) + Cl₂(g) - COCL, (g) Note: Reference the Fundamental constants table for additional information. E₁ - 1 kJ mol x10 X

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 362.0 °C 7.5 x 107 257.0 °C 5.6 x 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E = mol

For the formation of 1 mol of nitrosyl chloride at a given temperature, H = –44 kJ.NO(g) + ½ Cl2(g)  NOCl(g)The activation energy for this reaction is 59 kJ/mol. What is the activation energy for the reverse reaction? A) 59 kJ/molB) 15 kJ/molC) 103 kJ/molD) –44 kJ/molE) –103 kJ/mol

6. For a reaction at 25 °C, the activation energy of the forward reaction is 135 kJ and the activation energy of the backward 135 kJ (reverse) reaction is 187 kJ. Which of the following statements is true? 187 kJ a) The reaction is endothermic. b) The reaction is exothermic. c) The activation energy for the forward reaction increases by increasing temperature. d) The activation energy for the reverse reaction decreases by increasing temperature. e) None of the above.

A certain reaction is known to have an activation energy E-41.0 kJ/mol. Furthermore, the rate of this reaction is measured at 347. K and found to be 6.7 × 10² M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is lowered by 10% from 347. K to 312. K. The rate will choose one How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is added, which has the effect of lowering the activation energy by 10%, from 41.0 kJ/mol to 36.9 kJ/mol. The rate will choose one How will the rate of the reaction change? X Ś ?

The reaction C,H, (g) → 2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 745.0 K? k =

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 142.0 °C 6.1 x 1011 226.0 °C 3.7 x 10¹2 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. mol ×

A certain catalyzed reaction is known to have an activation energy E=66.0 kJ/mol. Furthermore, the rate of this reaction is measured at 351. K and found to be 1.5x 10-2M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is lowered by 10% from 351. K to 316. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 10%, from 66.0 kJ/mol to 72.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one stay the same rise about 10% rise more than 10% rise less than 10% fall about 10% fall more than 10% fall less than 10%

If the following chemical reactions have the same activation energy, which of them is likely to be faster at a given temperature? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b с d A(g) + 2B(g) → AB₂(g) A(g) + B(g) + C(g) → ABC(g) AB(g) + B(g) → AB₂(g) All will proceed at the same rate