Zero Order Reactions and Rate Laws

The video tutorial explains zero order reactions, where the rate is independent of reactant concentration. It covers the integrated rate law, showing that the concentration of reactant over time forms a straight line graph. The effect of stoichiometric coefficients on the rate is discussed, highlighting that textbooks often assume a coefficient of one. An example of ammonia decomposition on a platinum surface is provided, illustrating a zero order reaction where the rate is limited by catalyst surface area, not reactant concentration.

What is the rate of a zero order reaction dependent on?

• Concentration of reactant

• Pressure

• Rate constant

• Temperature

In a zero order reaction, what happens to the rate if the concentration of reactant is doubled?

• Rate remains constant

• Rate halves

• Rate doubles

• Rate quadruples

Which mathematical concept is used to derive the integrated rate law for zero order reactions?

• Algebra

• Integration

• Differentiation

• Statistics

What is the form of the integrated rate law for a zero order reaction?

• y = mx + b

• y = ax^2 + bx + c

• y = a/x

• y = e^x

In the graph of a zero order reaction, what does the y-intercept represent?

• Rate constant

• Initial concentration of reactant

• Time

• Final concentration of reactant

What does the slope of the line represent in a zero order reaction graph?

• Negative rate constant

• Variable rate constant

• Positive rate constant

• Zero rate constant

How does the slope of the graph change if the stoichiometric coefficient of the reactant is 2?

• Slope remains the same

• Slope becomes positive

• Slope becomes negative 2k

• Slope becomes zero

If the stoichiometric coefficient is 1, what is the slope of the graph?

• Positive k

• Zero

• Negative 2k

• Negative k

What is an example of a zero order reaction?

• Decomposition of ammonia on platinum

• Combustion of methane

• Photosynthesis

• Rusting of iron

Why does increasing the concentration of ammonia not affect the rate in the given example?

• Ammonia is not reactive

• Pressure is too high

• Surface area of catalyst is limiting

• Temperature is too low