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How can the rate law for a a chemical reaction be used to determine an instantaneous reaction rate?
The rate law for a chemical reaction expresses how the rate of the reaction depends on the concentration of reactants. By plugging in the instantaneous concentrations of the reactants into the rate law equation, we can calculate the instantaneous reaction rate at a specific moment in time.
A first order reaction is found to have a rate constant t k equals .0000739 find the half life of this reaction?
Since the reaction is first-order, the half-life is constant and equals ln(2)/k, and the units of k are s-1. In this case, the half-life is ln(2)/(.0000739 s-1) = 9379.529 seconds.
The decomposition reaction of ammonia gas on platinum surface has a rate constant k equals 2.510-4 mol l-1s-1 what is the order of the reaction?
The rate constant is not indicative of the order of the reaction. To determine the order of the reaction, experimental data (such as concentration vs. rate data) is needed. The order of the reaction can be found by examining how changes in reactant concentrations affect the rate of the reaction.
What is the significance of s-1 in chemistry?
In chemistry, the symbol s-1 represents the unit of inverse seconds, which is used to measure the rate of a reaction. It indicates how quickly a chemical reaction is occurring, with a higher value of s-1 indicating a faster reaction rate.
What describes a reaction that reaches equilibrium?
The product and reactants reach a final, unchanging level.
What is the instantaneous rate of the reaction at t equals 800. seconds?
6.8 X 10^-5 M/s
How can the rate law for a a chemical reaction be used to determine an instantaneous reaction rate?
The rate law for a chemical reaction expresses how the rate of the reaction depends on the concentration of reactants. By plugging in the instantaneous concentrations of the reactants into the rate law equation, we can calculate the instantaneous reaction rate at a specific moment in time.
A first order reaction is found to have a rate constant t k equals .0000739 find the half life of this reaction?
Since the reaction is first-order, the half-life is constant and equals ln(2)/k, and the units of k are s-1. In this case, the half-life is ln(2)/(.0000739 s-1) = 9379.529 seconds.
Can a peers instantaneous download rate never exceed its instantaneous upload rate in Bit torrent?
yes
What is the rate of change in a position at a given point in time?
The rate of change in position at a given point in time is instantaneous speed, instantaneous velocity.
What is The rate in change of position at a given point in time?
The rate of change in position at a given point in time is instantaneous speed, instantaneous velocity.
What is the rate of change in position in a given point of time?
The rate of change in position at a given point in time is instantaneous speed, instantaneous velocity.
What would happen to the rate of a reaction with rate law rate equals k NO 2 H2 if the concentration of NO were halved?
It will decrease by half.
How do you work out the rate of reaction when your independent variable is pH and your timing in seconds?
It is irrelevant what the independent variable is, whenever you work out rate of reaction you also divide 1 by the time in seconds. For example if it took 100 seconds your rate would be 0.01s-1.
What is application of differentiator?
Finding the rate of change - in particular, the instantaneous rate of change.
What best explains how a plot of concentration vs time for a reactant of a chemical reaction can be used to determine the instantaneous rate of a reaction at time equals 10 s?
1) Find time = 10 s on the curve. 2) Draw a line tangent to the point time = 10 s on the curve. 3) Use two points on the tangent line to find the slope of the line. 4) The slope of the line is the instantaneous rate in M/s.
What is the net rate of the reaction at equilibrium?
At equilibrium, the net rate of the reaction is zero, meaning that the rate of the forward reaction equals the rate of the reverse reaction. This balance results in no net change in the concentrations of the reactants and products over time. Although individual molecular events continue to occur, the overall concentrations remain constant.
