Could someone please help me with these chemical reaction balance equations? 1. (combustion) C3H8 + O2 ---> 2. (combustion) C2H6 + 02(g) ---> 3. (combustion) C2H6O + O2(g) -->
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Could someone please help me with these
1. (combustion) C3H8 + O2 --->
2. (combustion) C2H6 + 02(g) --->
3. (combustion) C2H6O + O2(g) -->
Step by step
Solved in 4 steps
- 会 云 + 1 1 < co T LL Car note CAU EMAIL CANVAS Pirate Ship MYJSC Vacančies | A... Birmingham Néw C....e Measures [Review Topics] [References] Complete and balance the following equations. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank.) a. I2 (aq) + Cl¯(ag) → b. Cl2 (aq) +I¯(aq) → c. Br2 (aq) +I (aq) → d. Br2 (aq) + CI¯ (aq) → Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Save and Exit L AON 14 étv MacBook Air 000 000 DD F7 F5 F4 F12 2$ 4. delete 8. 6. 7. } ] { [3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)3. When the reaction MnOc(aq) + (aq)-1(s)-MaOs) is balanced so that the smallest possible integers appear as stoichiometric coefficiens, the coefficient for OH is: 28060 23345
- 1. During the degradation of ethyl acetate (C4H3O2) with dichromate reactions occur as given below; balance the reactions: Total reaction: C4H3O2 + Cr20,2-+ H* Cr3* + CO2 + H2O(ii) H3CO H 1. excess CH3OH, [H+] 2. LDA, THF 3. H3C- 4. LiAlH4 5. H* workup 6. H3O+ e2. The formation of insoluble MgNH,PO,-6H,0, which is ignited to Mg.P.O, for weighing, can be used for the determination of Mg, N, or P. Write appropriate gravimetric factor that would apply to each determination.
- 1. Copper is found as the mineral covellite (CuS). The first step in extracting the copper is to dissolve the mineral in nitric acid (HNO3), which oxidizes sulfide to sufate and reduces nitric acid to NO: CuS) + HNO3(aq) → NO(g) + CuSO4 -> Balance this equation using the half- reaction method CHEM GINEE RST YEAR FRANE 6 hraIdentify the reaction that produced a blue precipitate (Exp 5). CưO + H;SO: → CuSO;+ H;C Cu + HNO3 → Cu(NO32+ NO, + H;C O Cu NOg2 + 2NaOH → Cu(OH)½ + 2NANO3 O CuSO + Mg –→ Cu + MgSO O CUOH)2→ CuO + H½C Quiz O 染+ F5 F6 F7 F8 F9 F10 F11 F12 & 國 立5. -4 Use the reaction below to complete the following problem. +2+6-8 8 Na CO4 + KMnO4 + H2SO4 --> MnSO4 + CD2 +13-2 (+246-2 14/2 + +2-8 +176-2 +2 + Na₂SO4 + K2SO4 + H₂O +462 +16-2 +1-2 0.221 g sample of sodium oxalate is dissolved in 100.00 mL distilled H2O and 20.00 mL of 3.0 M sulfuric acid. The solution is titrated to an endpoint with 37.14 mL of an unknown concentration of permanganate solution. Determine the equivalent weight of sodium oxalate. .2219 1349/mol - g/eq 00165 mol Calculate the equivalents of the oxalate used. eq Calculate the normality of the permanganate solution. eq/L 6 Given the foll
- 3. Complete the following reactions. (If the reaction doesn t occur, ple _H.SO, (aq) + _NAOH (aq) _C.H: (g) +_0: (g) KCI (aq) + AGNO: (ag) Zn (s) + CuSO, (aq)- _HBr (aq) +_N2OH (ag) CH12O6 (aq) +_O: (g) CuSO, (aq) +_K.CrO, (aq) _Mg (s) +_0: eA solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture