A certain substance, X, decomposes. 75 % of X remains after 100 minutes. How much X remains after 200 minutes if the reaction order with respect to X is the following order: zeroth order, first order, second order
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1. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹) 2. A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 16.0% of the substance to decompose? 3. How long will it take for the concentration of A to decrease from 0.500 M to 0.100 M in the first-order reaction A → B?...
A certain substance, initially at 0.10 M in solution, decomposes by second-order kinetics. If the rate constant for this process is 0.40 L/mol • min, how much time is required for the concentration to reach 0.020 M?
The reaction, A → products, is known to be
zeroth order with respect to the concentration of A and zeroth
order overall. The rate constant for the reaction is 0.0750
M·hr-1 at a certain temperature.
If the initial concentration of A is 0.875 M. What will be the
concentration of A after 10.0 hr?
Answer M
How long would it take for 80.0% of the starting material (A) to
undergo reaction?
Answer hr
The reaction, A → products, is known...
A certain substance, initially present at 0.500 M, decomposes by second-order kinetics with a rate constant of 4.00 × 10-1 L/mol min. Calculate the time (in minutes) required for the system to reach a concentration of 0.116 M. ___ min?
1. The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. Assume k = 10.09 x 10-4 s-1 . If the initial concentration of A was 0.82 mol L-1 and then decreased to 0.11 mol L-1 , how much time elapsed in minutes? 2. Consider the following balanced chemical equation: H2O2 (aq) + 3 I-(aq) + 2 H+(aq) → I3- (aq) + 2 H2O (l) In the first 62.9 seconds of the...
The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. Assume k = 2.46 x 10-4 s-1 . If the initial concentration of A was 0.89 mol L-1 and then decreased to 0.04 mol L-1 , how much time elapsed in minutes?
please help with question 25 a and b. showing all work
25. a. (3pts) A radioactive sample of substance X has initial mass = 3.25mg. It decays by a first- order reaction. If its half-life = 5.6 days, calculate its mass after 11.2 days. Given k = 0.0490. k= b. (4pts) Compound Z decomposes by a second-order reaction. We are told the initial concentration is 0.660M. If the value of k = 7.12 x 10 sec"!, what will the concentration...
A certain reaction obeys second-order kinetics with respect to its only reactant (call it R) and has a rate constant of 0.0520 L mole-1 s-1. If the initial concentration of reactant R is 0.265 moles/liter, what is the concentration of R after 3.50 minutes? _______________
10 and 11
10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows second order kinetics with a rate constant of 0.020 L mol-' s at a certain temperature. 2 NOCI (g) → 2 NO(g) + Cl2(g) If the initial concentration of NOCI in a closed reaction vessel is 0.050 M, what will be the concentration be after 30 minutes? 11. The reaction 2 NO2 (g) → 2 NO(g) + O2(g), is second order with respect to...
please help with question 25 a and b. showing all work
25. a. (3pts) A radioactive sample of substance X has initial mass 3.25mg. It decays by a first- order reaction. If its half-life = 5.6 days, calculate its mass after 11.2 days. Given k = 0.0490. On k= b. (4pts) Compound Z decomposes by a second-order reaction. We are told the initial concentration is 0.660M. If the value of k 7.12x 10sec, what will the concentration be after 2...