## What are the units for k rate?

The units of the rate constant, k, depend on the overall reaction order. The units of k for a zero-order reaction are M/s, the units of k for a first-order reaction are 1/s, and the units of k for a second-order reaction are 1/(M·s).

## How do you find the values and units of the rate constant k?

2 Answers

- rate=k[NOBr]x.
- The rate is second order in respect to NOBr, and the rate law is written rate=k[NOBr]2. If you double the concentration, the rate will quadruple.
- rate before doubling concentration=k[NOBr]2.

**What is the unit symbol for k?**

Kelvin | |
---|---|

Unit system | International system of units (SI) |

Unit of | Temperature |

Symbol | K |

Named after | William Thomson, 1st Baron Kelvin |

**How do I calculate k?**

To determine K for a reaction that is the sum of two or more reactions, add the reactions but multiply the equilibrium constants. The following reactions occur at 1200°C: CO(g)+3H2(g)⇌CH4(g)+H2O(g) K1=9.17×10−2.

### What are the units of k in the following rate law rate k x 2?

Answer and Explanation: For a given reaction with a rate=k[X]2 r a t e = k [ X ] 2 , the rate of reaction is second order. Therefore, the units for k are 1M. s.

### What are the units of k in the following rate law rate k x ][ y 1 2?

Chemical Kinetics

Question | Answer |
---|---|

What are the units for K in Rate= k[X] and k[X]^0[Y]^0? | 1/s |

What are the units for K in Rate= k[X][Y]^1/2? | M-1/2s-1 |

What are the units for K in Rate= k[X]^2? | M-1s-1 |

Which of the following represents the integrated rate law for a first-order reaction? | ln[A]t/[A]o= -kt |

**What are the units of k for the rate law rate Kab 2?**

The units for k should be mol−2 L2/s so that the rate is in terms of mol/L/s.

**What is the value for K?**

The value of K in free space is 9 × 109. Was this answer helpful? 3.5 (10) (21) (3)

#### How do you find K in physics?

W = kx. W is the weight of the added mass. Therefore, the spring constant k is the slope of the straight line W versus x plot. Weight is mass times the acceleration of gravity or W = mg where g is about 980 cm/sec2.

#### What are the units of k for a third order reaction?

What is the unit of rate constant of the third order reaction? mol-2L2s-1 is the unit of third order reaction.

**Do constants have units?**

Fundamental Constants. Fundamental constants are some numbers with units that cannot (yet) be calculated from some physical theory, but must be measured.

**What are the units of k in a third order reaction?**

Every time the order is increase by one we divide by M or mols/L. So therefore, for a third order, the units of k would be 1/M^2*s or L^2*mol^-2*s^-1. Hope this helps!

## What is the unit of rate constant for second-order reaction?

For the units of the reaction rate to be moles per liter per second (M/s), the units of a second-order rate constant must be the inverse (M−1·s−1). Because the units of molarity are expressed as mol/L, the unit of the rate constant can also be written as L(mol·s).

## What are the units for third order reaction?

Third Order Reaction Examples

Reaction Order | Units of k |
---|---|

Zero | mol/L/s |

First | s-1 |

Second | L/mol/s |

Third | mol-1 L2 s-1 |

**How do you find k?**

Calculating K from Known Initial Amounts and the Known Change in Amount of One of the Species

- Write the equilibrium expression for the reaction.
- Determine the molar concentrations or partial pressures of each species involved.
- Determine all equilibrium concentrations or partial pressures using an ICE chart.

**How do you find K for a 2nd order reaction?**

The order of the reaction is second, and the value of k is 0.0269 M-2s-1. Since the reaction order is second, the formula for t1/2 = k-1[A]o-1. This means that the half life of the reaction is 0.0259 seconds….

1/Concentration(M-1) | Time (s) |
---|---|

3 | 30 |

### How do you find K in standard form?

If you’ve already learned the Quadratic Formula, you may find it easy to memorize the formula for k, since it is related to both the formula for h and the discriminant in the Quadratic Formula: k = (4ac − b2) / 4a.