For letters b and d, did I solve it correctly?what are the correct units?
1. Consider the below decomposition reaction at 25 °C, NOdg) â NO(g) + 0(g). Data for this reaction is given Time(s) NOJM 0.01000 0.00662 0.00495 0.00395 0.00329 200 400 600 800 350 300 250 000 0.00282 Appropriately graph the data above to show that the l reaction is second order. Be sure to correctly label the x and y-axes. Hint: I have already put in the correct axes scales for you. a. 10 100 50 Using the graph to the right, determine the value of the rate constant, with correct units, for the reaction above. b. 1000 =-0736 ms-1 c. What is the reaction rate when the concentration of NO, is [NO))-0.00567 M? d. Calculat the concentration of NO, at 2.000 sec e. if the rate constant at 45 "C is 0.650 Mt's', calculate the value of the activation energy, E, of the above reaction.
Calculate the final volume of the reaction mixture after the contents of beaker B are added to beaker A. Report your answer in liters.
All S2O32- is consumed at the end of the reaction. Therefore, the moles of S2O32- consumed can be calculated using the equation below. (moles S2O32-)consumed = Mstock x (Vstock)
The I3- produced in reaction 1 reacts with S2O32- in reaction 2 as shown. I3- (aq) 2S2O32- (aq) â 3I- (aq) S4O62- (aq)
Therefore, for every mole of I3- produced, 2 moles of S2O32- have reacted. (moles I3-)produced = (moles S2O32-)consumed / 2
Calculation is the same as d, but using I3- instead of S2O32-.
Fill in the following table. Look below the table for instructions on how to calculate the values for each column of the table.
a
b
c
d
e
f
g
h
i
Trial
Ît
Î[I3-] / Ît (M/s)
log(Î[I3-] / Ît)
V 0.2 M KI added (mL)
[Iâ]0(M)
log[Iâ]0
V of 0.2 M (NH4)S2O8 (mL)
[S2O8]0 (M)
log[S2O8]0
1
19
.011
-1.94
25
.077
-1.35
25
.077
-1.11
2
40
.0055
-2.24
25
.077
-1.11
12.5
.038
-1.42
3
85
.0030
-1.84
25
.077
-.1.11
6.25
.019
-1.72
4
42
.0055
-2.26
12.5
.038
-1.42
25
.077
-1.11
Conclusions
If a large amount of heat was released at the start of the reaction, what effect would this have on the rate measurements?
The rate of reaction would be much slower due to its exothermic reaction properties.
Click the box underneath the graph to show the trendline. It will automatically calculate your slope and intercept. Record them below.
Determine the value of q from the graph. Explain your answer.
What is the rate law for the reaction?
For each trial, calculate the rate constant. What is average value of the rate constant?
In this experiment, you assumed that [S2O82â] >> [S2O32â]. To find out if this assumption is correct, calculate the ratio of [S2O82â] / [S2O32â] for Trial 3. (In Trial 3, the [S2O82â] was lowest, and therefore the ratio [S2O82â] / [S2O32â] is the smallest).
In this experiment, you assumed that only a small amount of S2O82â was used during the time trial so that the concentration of this reactant did not change appreciably during the course of the reaction. Calculate how much S2O82â was used in Trial 3 and the percent remaining at the end of the reaction. Was this assumption valid?
o logldelta 13/delta t and log($208)0 log[delta 13]/delta t show trendline Slope: -0.331 Intercept: -2.077
Mole ratio lab v3b Rukes APChemistry Determination of the mole ratio of a chemical reaction The method of continuous variations is a means of determining the stoichiometric mole ratio of the reactants in a chemical reaction. The stoichiometric ratio, as given by the coelficients in the balanced chemical equation, represents the ratio at which chemicals must be combined to produce al product with no excess rcactant. Sincc there is no âwasted" reactant, the maximum amount of product is made for the given amount of both reactants. In themethod of continuous variations, several trials are performed. In each trial, there is a fixed amount of total reactant (measured by moles or volume or mass, etc.), but with the two reactants mixed together in different ratios. Some measure of the amount of product is made for each trial (volumc of gas produccd, mass of precipitate, color of product solution, etc.). When the amount of product is maximized, the stoichiometric ratio has been used. A similar technique fixes the amount of one reactant and increases the other until the maximum amount of product is reached In this lab the two chemicals being mixed are solutions of known molarity. The total volume of solutions is kept constant over several trials. The chemicals will release heat when mixed together and raise the temperature of the mixture. Since the volume of the solutions mixed is held constant, the temperaturc changc recorded wl be proportional to the amount of heat produced and therefore also the "anount of reaction" that occurred. Objectives - To graphically determine the stoichiometric mole ratio of a reaction. CAUTIONS: All solutions are basic and can be harmful to skin and eyes. Sodium hypochlorite can also bleaclh clothing. Wear goggles, gloves and aprons. ︵ Pre-lab: complete on a separate sheet. 1. Accurately graph the following data gathered from an experiment which mixes 0.5 M solutions of AgNO3 and K2CrO4. The x-axis should plot the volume of AgNO3 reading Irom lef to right (or the volume of K2CrO4 reading from right to left.) Draw two best fit lincs, one for the "up" slope and one for the "down" slope... see example to the right of the data. (Also consult your graphing skills handout if you have not yet drawn a graph) trial mL AgNO3 mL K2CrO mass of precipitate (g) 45 35 25 20 15 10 shape of graph 15 25 30 35 40 45 5.0 4 10.0 9.9 6.6 3.3 a) Use the intersection of best fit lines to find the theoretical maximum amount of product. b) Use the x-values to find the stoichiometric volume ratio c) Use the answer from b) and given molarities to find the stoichiornetric mole ratio d) How many values were used to plot your "up" line? How many values were used to plot your "down" line? 2. What single temperature change should be recorded if 10 mL of solution A at 20°C is mixed with 10 mL of 3. What single temperature change should be recorded if 10 mL of solution A at 20°C is mixed with 30 mL of 4. List four dependent variables that are often used for the method of continuous variations. Are these enough values to plot a good line? solution B at 24.0°C and the final temperature reaches 28.0°C? solution B at 24.0°C and the final temperature reaches 28.0°C?
