denotation shockwave. explosion materials Find possible reactant and product of the following explosive materials. Calculate mass of mixture, total number of moles and molecular weight. Reactant Product a. TNT (Solid) b. TNT (liquid) S. PETN
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- A mixture containing KClO3, K2CO3, KHCO3, and KCl washeated, producing CO2, O2, and H2O gases according to thefollowing equations:2 KClO31s2¡2 KCl1s2 + 3 O21g22 KHCO31s2¡K2O1s2 + H2O1g2 + 2 CO21g2K2CO31s2¡K2O1s2 + CO21g2The KCl does not react under the conditions of the reaction. If100.0 g of the mixture produces 1.80 g of H2O, 13.20 g of CO2,and 4.00 g of O2, what was the composition of the originalmixture? (Assume complete decomposition of the mixture.)Why is there a danger of possible explosions in places like coal mines where there are large quantities of powdered, combustible materials?The following reaction was studied in the laboratory and the data shown in the table below was recorded at 25oC : A(g) + B(g)⟶C(g) + D(g) Trial A (mol/L) B (mol/L) Δ[C]/Δt (mol/L/s) 1 1.00 × 10−6 3.00 × 10−6 6.60 × 10−5 2 1.00 × 10−6 6.00 × 10−6 1.32 × 10−4 3 1.00 × 10−6 9.00 × 10−6 1.98 × 10−4 4 2.00 × 10−6 9.00 × 10−6 3.96 × 10−4 5 3.00 × 10−6 9.00 × 10−6 5.94 × 10−4 (a) Determine the order of reaction with respect to each reactant and the overall order. Show your working clearly. (b) Determine the value of the rate constant K. (c) Calculate the half-life of the reactant ‘A’ if initial concentration is 1 x 10-6 M. (d) Using this reaction as an example, explain the difference between stoichiometric coefficients, reaction order and molecularity.
- What about Part C? Additionally for part B I'm not really getting the bottom of the 2nd page where have the Chemical Reaction written. Wouldn't it be better to set9.15 + log((7.5mM - 1.25mM)/17.5)? So don't need to know equation?Plz do the 4 and 5 of level 2... for each one write the chemical reaction in symbols... highlight the coefficients...In Problems 23–28, use the procedures illustrated in Example 10to balance the given chemical equation.23. Na H2O S NaOH H224. KClO3 S KCl O225. Fe3O4 C S Fe CO26. C5H8 O2 S CO2 H2O27. Cu HNO3 S Cu(NO3)2 H2O NO28. Ca3(PO4)2 H3PO4 S Ca(H2PO4)2
- Plz do the 4 and 5 only ... for each one write the chemical reaction in symbols... highlight the coefficients...In any manufacturing process, reaction monitoring ensures that a chemical reaction proceeds as expected. Table 1 shows the monitoring data for the formation of chlorohexane, collected using a technique called gas chromatography. Note that the concentrations of the chlorohexane solutions are given in millimoles per litre (mmol l–1). The abbreviation mM (millimolar) is frequently used. Plot a graph of the data in Table 1. The graph should be drawn on graph paper or use fine grid if it’s drawn on Excel. Elapsed Time/Hours Concentration of Chlorohexane/mM 0 0 2 40 4 65 6 80 8 90 10 95 12 99Ozone can oxidize HSO3^1-(aq) as represented below: HS03^-1(aq)+03(aq)-->HS04^-(aq)+02(g) A solution is prepared in which the initial concentration of HSO3^1-(aq)(6.4x10^-4 M) is much larger than that of O3(aq)(1.0x10^-5 M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below: (see attached image) The data are consistent with the following rate law: Rate = k1[O3] i) Based on the graph, determine the half-life of the reaction ii) Determine the value of the rate constant k1 for the rate law. Include units
- 21. A flask is charged with 0.140 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) B(g) The following data are collected. times (s) 0 40 80 120 160 moles of A 0.140 0.072 0.042 0.033 0.020 (a) Calculate the number of moles of B at each time in the table.0 s _____mol40 s _____mol80 s ______mol120 s ______mol160 s ______mol(b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s.0 - 40 s ______mol/s40 - 80 s ______mol/s80 - 120 s_______ mol/s120 - 160 mol/s ______mol/sBalance the following chemical equations, making sure to apply the principle of the Law of Conservation of Mass.Per ruling, please answer equation #10. Thank you!Some ionic can include in their solid structures in specific proportions. For example anhydrous copperII sulfate form a hydrate according to the reaction equation below. Determine the number of water moléculas in the hydrate ( x in the equation) from the following information. A 1.000g sample of anhydrous CuSO4 adsorbed water and became completely hydrated. This sample then weighed 1.65g CuSO4+x H2O --> CuSO4 . x H2O