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1) In general, how does the reaction rate depend on the concentrations of the reactants? 2)...
How does the value of Kc in Equation the reaction below depend on the starting concentrations of NO2 and N204? N204_<_> 2NO2(g) Kc- [NO2]^2/[N204] Kc is independent of the starting concentrations of reactants and products O b. Kc is independent of the starting concentrations of reactants and products. Oc. Kc is second order with respect to NO2 and inversely related to N204 using starting concentrations ke is directly related to NO2 and inversely related to N204 using starting concentrations
Kinetics of the permanganate and Oxalate Reaction. 2. Write out the general rate law for today's reaction with the two reactants. Use x and y for the orders of reaction for each reactant, and include the rate constant. How will the reaction rate be monitored? A B CtD Ra tekLAJEO 3. If different students use different concentrations of the same reactants, should there be any difference in calculated values for the rate constant? Why or why not? 4. Suggest two...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. What is the reaction order with respect to B? Also, how do you find the value of the rate constant k for this reaction? Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between A and B, aA+bB⇌cC+dD The dependence of the...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4 What is the value of the rate constant k for this reaction?
1) Give definition of half-lifetime. How is that defined? 2) How does the half-lifetime for a zero-order reaction depend on rate constant? how does that depend on reactant initial concentration? 3) How does the half-lifetime for a first-order reaction depend on rate constant and initial reactant concentration? 4) How does the half-lifetime for second-order reaction depend on rate constant and initial reactant concentration? 5) Someone monitored a reaction by observing the time it took for the reactant concentration halve. It...
Consider the following reaction: A+B→C+D The initial concentrations of the reactants A and B are 0.220 M and 0.320 M, respectively. The rate of reaction is 0.060 M⋅S-1, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. Express your answer in M-2⋅S-1 to three significant figures.
INFORMATION reaction must also be perimental mea data are plotted in the sult means that the rate Because a reaction is faster at higher temperatures, the rate constant for the reaction m larger. The activation energy of a reaction can therefore be determined from experime surements of the rate constant at several temperatures. When the collected data are ple form In(k) vs T. as shown in Figure 2. a straight line is produced. This result means constant varies exponentially with...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction. 6) An equilibrium in which all the components are gases is a A) heterogeneous equilibrium. D) homogeneous B) liquid C) catalytic E) reversible 7) The equilibrium...