Project One

You conduct an experiment where everything but the number of cigarettes a person smokes is held constant You discover that a person smoking two packs of cigarettes a day quadruples (4x) the rate of aging over that of a one-pack-a-day smoker. Based on the data you have been given what is the value for n in the rate equation? Rate of aging = k [packs of cigarettes smoked]

please help and make things clear thank you so much (:

Determine whether the following statements are true or false, and explain your answer in one sentence. a) The rate law for an overall reaction 2A (g) -> B (g) is: Rate = k[A]^2 b) The rate law for an elementary step 2A (g) -> B (g) is: Rate = k[A]^2 c) The rate of an overal reaction is the rate of the slowest elementary step within its mechanism.

Rate laws can be entered as strings in the answer box. For example, for aA(aq) + bB(aq) → CC(aq) with the rate being second order in A and first order in B you enter k*[A]^2*[B] and for aA(g) + bB(g) cC(g) with the rate being second order in A and first order in B using pressures you enter k*P_{A}^2*P_{B}. The reaction 2NO(g) + O2(g) → 2NO2(g) is second order in NO and first order in 02. Write the rate law for the reaction in terms of pressures PNO and Po2 . Let us agree not to use subscripts on subscripts. So, to enter the pressure of 02 use P_{02} and not P_{O_2}. Units can be entered using mol/(L s) note the parenthesis and the space between L and s. Enter the units of r when the pressure is measured in bar and time in min. (use the backslash / but be sure to use () when more than one unit is is the denominator) Units of r = Enter the units of r when the amount is measured in mol L1 and time in min (use the backslash / but be sure to use () when more than one unit is is the…

Route 1:RME = 82.92%MI= 1.34 Route 2RME = 93.33%MI = 1.57 Route 3RME = 57.34%MI = 1.89 Compare the value of Reaction Mass Efficiency (RME) and Mass Intensity (MI) generally, and choose which metrics is more significant in green measurement. Justify your answer.

If 2.0 × 10-4 moles of  H2O2H2O2 in 50 mL solution is consumed in 3 minutes and   25  seconds, what is the rate of consumption of H2O2H2O2?  Express the rate in mol per liter·second to two significant digits.

If tripling the concentration of a single reactant R in a multi-reactant reaction (while leaving all other conditions unchanged) leads to a nine−fold increase in rate, it can be deduced

The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. Answer:

what are the roles of following in crime scene investigation and how do they interact with each other? scene of crime officer(SOCO) forensic scientist police pathologist fire department gas/electricity adviser specialist dog units

Use the graph and the best fitting line to predict the concentration of NO2NO2 at 2000 ss . Express the concentration to two significant figures and include the appropriate units.

Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen: 2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is curved, but if the logarithm of this concentration is plotted, we instead get a straight line. Based on this, which statement is true? a)  This decay is a second order in peroxynitric acid. b)  The slope of the straight-line graph is the rate constant. c)  One needs the concentration of peroxynitric acid to calculate its half-life. d)  The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].

4PH3 P4 + 6H₂ What is the rate of disappearance of PH3 from 0 to 75 seconds? Time [PH₂] [P4] [H₂] 0 2.00 0 0 75 1.50 ? ? 150 1.25 0.19 1.13 225 1.13 0.22 1.31 300 1.07 0.23 1.40 RatepH3 [?] x 10 M/s Coefficient (green) Exponent (yellow) Enter

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Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C1O₂(aq) + 2OH(aq) → CIO₂ (aq) + CIO3(aq) + H₂O(1) Under a certain set of conditions, the initial rate of disappearance of chlorine dioxide was determined to be 2.30 x 10-1 M/s. What is the initial rate of appearance of chlorite ion under those same conditions? O 5.75 x 10-2 M/s O 1.15 x 10-¹ M/s O 2.30 x 10-1 M/s O 4.60 x 10-¹ M/s O 9.20 x 10-1 M/s

Explain how  the rate of reaction rate in pressure cookers was increased by including these subtopics:1. Chemical reaction(s) involved with chemical equation(s) 2. Reactants, products, and possible catalysts involved in the chemical reaction 3. Explain with collision theory and energy potential diagrams: how the rate of reaction is affected by temperature, surface area, nature of reactants, concentration, etc. by using collision theory? 4.Discuss whether the reaction is endothermic or exothermic (use Hess’s Law, Le Châtelier’s Principle, or Kinetic Molecular Theory to explain in increasing rate of reaction and relevance by including all 4 required subtopics )

Consider the reaction a A(aq) → bB(aq) (1) Where a and b are stoichiometric coefficients for the balanced chemical reaction The average reaction rate r can be measured if the concentration change of the reagents or products is known: 1 ΔΙΑ 1 Δ r = and r = At b At a where A and B notate the concentration of A and B in solution, and A is always defined as the difference between "final" and "initial": A[4] = [A],2 - [4],1 and At = t2 – t . - A particular case of eq. (1) could be A(aq) → 2 B(aq) If the initial concentration of B is 0.2569 mol L1, and after 415.6 s it increases to 0.4633 mol L1, what is the rate of the reaction in mol L1s? mol L-1 s1. (Use scientific notation)

Time [Z] (hours) (mg/L) |160 2 |140 3 |130 6 100 8 80 10 |60 |12 40 Calculate k, the elimination rate constant, responsible for drug degradation (in mg/L*hr).

Explain how the rate of reaction rate in pressure cookers was increased by including these subtopics:1. Chemical reaction(s) involved with chemical equation(s)2. Reactants, products, and possible catalysts involved in the chemical reaction3. Explain with collision theory and energy potential diagrams: how the rate of reaction is affected by temperature, surface area, nature of reactants, concentration, etc. by using collision theory?4. Discuss whether the reaction is endothermic or exothermi

The chemical reaction A(aq) + B(aq) à C(aq) + D(aq) + E(aq) has an experimentally determined rate law of rate = k[A][B]. An experiment using the method of isolation was used to determine the order with respect to CH3I. This experiment yielded the following Rate law: rate = k’[A]. What is true of this experiment and its findings? the experiment illustrated that the reaction pseudo 2nd order     [A]>>>[B]                  [A] = [B]                    [A]<<<[B}

For each scenario below, describe: (a) How could they have been prevented. (b) What should be the appropriate response to minimize harm. During a chemistry experiment, Jude carefully pours an unknown solution from a test tube into a beaker. His groupmate, John surprises him from behind. Jude accidentally drops the beaker and glass pieces caught his sandaled foot.

A group of students enrolled in a Physical Chemistry Laboratory class performed an experiment on the THE STUDY OF AN ADSORPTION ISOTHERM: ACETIC ACID SOLUTIONS ON ACTIVATEDCARBON. The data gathered by the group are documented in the tables below. Solve for the unknown data.   answer 1,2,3

Why does the product (a•b), rather than the sum (a + b) appear in the Law of Mass Action? This is sometimes brought up to demonstrate how/why nonlinear terms arise in differential equations. The law of mass action states that The rate of a chemical reaction involving an interaction of two or more chemical species is proportional to the product of the concentrations of the given species.  This is NOT an assignment...I'm just curious and trying to understand mathematical relations better. Thanks!

A student is preparing a solution of sucrose at a specific concentration. They are doing this by weighing out sucrose on a scale, placing it in a volumetric flask, dissolving it in water, and then diluting it up to the mark on the volumetric flask with water. How would the experimental (actual) molar concentration for C12H22O11 differ from the calculated concentration ( higher, lower, or the same) given the following scenarios? Explain.

so that means route a is preferrable in a small lab and route b is preferred in a chemical plant?