**Reaction Rate Analysis****Consider the reaction:**\[ 2\text{H}_3\text{PO}_4 \rightarrow \text{P}_2\text{O}_5 + 3\text{H}_2\text{O} \]**Objective:** Using the data in the table below, calculate the average rate of formation of \(\text{P}_2\text{O}_5\) between 10.0 and 40.0 seconds.| Time (s) | [\(\text{P}_2\text{O}_5\)] (M) ||----------|--------------------|| 0 | \(0\) || 10.0 | \(1.00 \times 10^{-3}\) || 20.0 | \(4.00 \times 10^{-3}\) || 30.0 | \(5.80 \times 10^{-3}\) || 40.0 | \(7.00 \times 10^{-3}\) || 50.0 | \(7.60 \times 10^{-3}\) |**Instructions:** Express your answer with the appropriate units.**Explanation of the Data:**The table provides concentration measurements of \(\text{P}_2\text{O}_5\) at various times during the course of the reaction. The concentration is expressed in molarity (M), and time is measured in seconds (s). To determine the average rate of formation of \(\text{P}_2\text{O}_5\), you will need to apply the formula for rate of reaction, focusing on the time interval from 10.0 to 40.0 seconds.

Rate of reaction :- The decrease in concentration of reactants with time or increase in…

Consider the reaction 2H3PO4→P205 + 3H2O Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s. Time (s) 0 10.0 20.0 30.0 40.0 50.0 P2O5] (M) 0 1.00×10-3 4.00×10-3 5.80×10-3 7.00×10-3 |7.60×10-3 Express your answer with the appropriate units.

Consider the reaction 2H3PO4→P205 + 3H2O Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s. Time (s) 0 10.0 20.0 30.0 40.0 50.0 P2O5] (M) 0 1.00×10-3 4.00×10-3 5.80×10-3 7.00×10-3 |7.60×10-3 Express your answer with the appropriate units.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
Consider the reaction and the information in the table provided. Calculate the average rate of formation of P2O5 between 20.0s and 40.0s. 2H3PO4 → P2O5 + 3H2O Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 Conc P2O5 (M) 0 0.00120 0.00420 0.00600 0.00720 0.00780
Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. The table: Time (s) [A] (M) 0.00 0.600 1.50 0.325 3.00 0.178 4.50 0.095 6.00 0.050 7.50 0.028 9.00 0.015
6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179
2N2O5(g) → 4NO2(g) + O2(g) Rate constants for the decomposition of gases dinitrogen pentoxide are 4.222 x 10s1 at 25 °C and 2.111 x 10 3 s1 at 80 °C. What is the activation energy for this reaction kJ/mol?(Hint R constant 8.314 J/K x mol) 60.55 kJ/mol 69.08 kJ/mol O -68.00 kJ/mol O -62.27 kJ/mol
Consider the reaction: 2NO(g) + O₂(g) 2 NO₂ (g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of -0.054 M S
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] 3.4 3.4 1.223775 0.294118 25 2.28 0.824175 0.438596 2.822 + 50 1.53 0.425268 0.653595 2.244 + 75 1.02 0.019803 0.980392 1.666 - 1.088 - 0.51 - 15 30 45 60 75 t y=-0.03156 x + 3.241000 2= 0.971 Add Row 10 total rows What is the reaction order? O 1 Calculate the concentration of A after 127 s. [A]127 s = M [V)
Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]
please see attached for the following equation: