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Chapter 12: Q7E (page 702)

Describe the effect of each of the following on the rate of the reaction of magnesium metal with a solution of hydrochloric acid: the molarity of the hydrochloric acid, the temperature of the solution, and the size of the pieces of magnesium.

Short Answer

Expert verified

The effect on the rate of the reaction of magnesium metal with a solution of hydrochloric acid increases with the molarity of hydrochloric acid, increase with increased temperature and increase with the reactant size.

Step by step solution

01

Molarity of the hydrochloric acid

Molarity means the number of moles of solute present per litre

The rate of reaction is dependent on the frequency at which molecules collide. Increasing the molarity means increasing the concentration of molecules, then increasing the collision between the molecule and increasing the rate of reaction.

02

The temperature of the solution.

Temperature increases the number of particles to cross the activation energy barrier to starting making a product.

Rate of reaction increase with increased temperature because the molecule collides more frequently.

03

the size of the pieces of magnesium.

The rate of reaction depends on reactant size because the greater the surface area thus faster the rate of reaction.

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Most popular questions from this chapter

Acetaldehyde decomposes when heated to yield methane and carbon monoxide according to the equation: \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CHO}}\)(g) ⟶\({\bf{C}}{{\bf{H}}_{\bf{4}}}\)(g) +\({\bf{CO}}\)(g)

Determine the rate law and the rate constant for the reaction from the following experimental data:

Trial

(\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CHO}}\)) (mol/L)

\(\frac{{ - \Delta \left( {{\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CHO}}} \right)}}{{\Delta t}}\)(mol )(Ls−1)

1.

1.75 × 10−3

2.06 × 10−11

2.

3.50 × 10−3

8.24 × 10−11

3.

7.00 × 10−3

3.30 × 10−10

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Nitrogen monoxide reacts with chlorine according to the equation:

2NO(g) + Cl\({}_2\)(g)⟶ 2NOCl(g) The following initial rates of reaction have been observed for certain reactant concentrations:

What is the rate law that describes the rate’s dependence on the concentrations of NO and Cl2? What is the rate constant? What are the orders with respect to each reactant?

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The annual production of \({\bf{HN}}{{\bf{O}}_{\bf{3}}}\) in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel.

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The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in \({{\bf{O}}_{\bf{2}}}\), what is the rate of formation of \({\bf{N}}{{\bf{O}}_{\bf{2}}}\) when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M? The rate constant for the reaction is \({\bf{5}}{\bf{.8 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}{\bf{ L}}{{\bf{ }}^{\bf{2}}}{\bf{ mo}}{{\bf{l}}^{{\bf{ - 2}}}}{\bf{ s}}{{\bf{ }}^{{\bf{ - 1}}}}\).
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