A company is looking for the optimum conditions to produce hydrogen gas using the reaction between dilute sulfuric acid (H₂SO4) and magnesium metal. Predict what will happen to the reaction rate under the conditions described below and support your answer using collision theory. a) The temperature of H₂SO4 (aq) is decreased by 20°C b) Magnesium powder is used rather than the equivalent mass of cubes of metal.

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Consider a possible gas-phase reaction between Ca+ and CH4+ to yield Ca+2 and CH4. What important feature of the reactants is neglected in collision theory which might work to reduce the probability of reactive collisions between them?

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-