## Which graph is correct for zero order?

For a zero-order reaction, t12=[A]02k. Thus, as the initial concentration increases, the half-life increases. Hence, graph A is correct.

**What does a zero order graph look like?**

Other graphs are curved for a zero order reaction….Rate Laws from Graphs of Concentration Versus Time (Integrated Rate Laws)

For a zero order reaction, | rate = k | (k = – slope of line) |
---|---|---|

For a 1st order reaction, | rate = k[A] | (k = – slope of line) |

For a 2nd order reaction, | rate = k[A]2 | (k = slope of line) |

**How do you find the order of a reaction graphically?**

If you get a straight line with a negative slope, then that would be first order. For second order, if you graph the inverse of the concentration A versus time, you get a positive straight line with a positive slope, then you know it’s second order.

### How do you know if a graph is zero or first order?

Zero order, you have a straight line with a negative slope only when you graph concentration A versus time. First order, would be natural log of concentration A versus time. If you get a straight line with a negative slope, then that would be first order.

**What is graphical representation of first order reaction?**

Graphical Representation of a First-Order Reaction For first-order reactions, the equation ln[A] = -kt + ln[A]0 is similar to that of a straight line (y = mx + c) with slope -k. This line can be graphically plotted as follows. Thus, the graph for ln[A] v/s t for a first-order reaction is a straight line with slope -k.

**How do you know if its zero order or first order?**

If an increase in reactant increases the half life, the reaction has zero-order kinetics. If it has no effect, it has first-order kinetics. If the increase in reactant decreases the half life, the reaction has second-order kinetics.

#### How do you know if a graph is zero first or second-order?

**What is the order of reaction graph?**

First order, would be natural log of concentration A versus time. If you get a straight line with a negative slope, then that would be first order. For second order, if you graph the inverse of the concentration A versus time, you get a positive straight line with a positive slope, then you know it’s second order.

**What is the difference between zero order drugs and first order drugs?**

First order kinetics occur when a constant proportion of the drug is eliminated per unit time. Zero order: a constant amount of drug is eliminated per unit time.

## Which of the following is not true for zero order reaction?

Hence, on increasing concentration of reactants, rate of reaction does not increase. From Rate Law for Zero Order reaction, we can conclude that rate of reaction is independent of concentration of reactants. Hence, Option “A”, \ “B” \ \& \ “C” are not true.

**How do you determine the order of a reaction graphically?**

**How do you know if a reaction is zero order or first order?**

If the reactant concentration increases, the reaction has zero-order kinetics. It has first-order kinetics if it has no effect. The reaction has second-order kinetics if increasing the reactant decreases the half life.

### What is the difference between first order and zero order graphs?

Zero order graphs will only be linear when graphed [A] vs time while First order graphs will only be linear when graphed ln [A] vs time. Both of their slopes are -k so it may be confusing to read at first.

**How do you plot a zero order reaction on a graph?**

Graph of Zero Order Reaction The integral form of zero order reactions can be rewritten as [A] =–kt+[A0] [ A] = – k t + [ A 0] Comparing this equation with that of a straight line (y = mx + c), an [A] against t graph can be plotted to get a straight line with slope equal to ‘-k’ and intercept equal to [A] 0 as shown below.

**What is the difference between first order and zero order reactions?**

In a zero order reaction, a straight line is obtained when you plot the concentration of the reactant [A] vs time t. For a first order reaction, on the other hand, plotting ln [A] vs t will give a straight line with a negative slope. The only similarity between the two graphs is the slope, which is -k (where k is the rate constant of the reaction).