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Give detailed Solution with explanation needed..please explain..give all possible reagents to making following product.
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- The given are SlGMATROPlC REACTlONS. Show the arrøw pushing then find their products.A+B➡️P t=0 :C(A)=C(B) t=500sec 20% of react t=? Sec 60% of complSpecies So NH3 111.3 O2 205.0 CH4 186.1 HCN 201.7 H2O 70.0 Calculate the ΔSo for the reaction: 2 NH3 + 3 O2 + 2 CH4 ⟶ 2 HCN + 6 H2O T = 25o CExpress the answer to 1 decimal point.
- Explain why scientists do not use a standard set of steps for everyinvestigation they conduct.Rate = k[acetone]1[I2]0[H+]1 rate = 0.001M/ 332.26s = 3.01 x 10-6 my question is what is the S.I unit of this answer? 3.01 x 10-6 = k[0.80M]1 [0.001M]0 [0.20]1 k= (3.01 x 10-6)/ (0.16) k = 1.88 x 10-5 also S.I unit of this answer with clear explanation and stepsWhat is the microscopic explanation for the macroscopic behaviour illustrated in Figure 11.15?
- Jj.53.Why do you multipy the # of H2S mols by 4, when 4 corresponds to the reactory amount of O2?The logic there is somewhat confusing to me.I understand how/why you found out the mols of the equation but dividing the sample's MM by the equation confuses me.C. Purification of Water 1.For this part of the experiment, watch the video on the link(s) below: a. Flocculation: https://www.youtube.com/watch?v=5uuQ77vAV_U&t=82s Question: Observation before flocculation. Observation after Flocculation
- Which of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)(NH4)2Cr2O7 (s) --> Cr2O3 (s) + 4 H2O (g) + N2 (g) The compound Ammonium Dichromate, (NH4)2Cr2O7, will decompose into Cr2O3, H2O, and N2, when it is heated vigorously. However, it is almost impossible to acquire a pure sample of (NH4)2Cr2O7 , instead (NH4)2Cr2O7 is usually contaminated with some Cr2O3 in its container. To determine how much Cr2O3 is in the container, a student heats a sample of the mixture, and collects the water vapor using a drying agent. The following table shows the data the student recorded during the heating of a sample of the mixture. Mass of Empty Test Tube 14.66 g Mass of Test Tube and Mixture before Heating 16.92 g Mass of Drying Agent Before Reaction 2.26 g Mass of Drying Agent and Water After Reaction 2.65 g a) Calculate the grams of (NH4)2Cr2O7 present in the mixture in the test tube before the mixture was heated. b) Determine the mass percent of (NH4)2Cr2O7 in the mixture. c) If the student spilled some of the mixture out of the test tube…Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.