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A chemical reaction is a process one or more substances are transformed into another substances. Physical change - color change - solid formation (precipitation) - gas release (evolution of a gas - heat exchange (evolution or absorption of heat) chemical equation is an expression of a chemical reaction by using symbols and formulas. In a reaction the starting substances are called reactants reactants products the substances formed in a reaction , are called products. reactant1 + reactant2 product(s) (g)= gas (I)= liquid (s)= solid (aq)= aqueous (water) solution Balancing Chemical Reaction Because atoms are neither created nor destroyed in any reaction, a chemical equation must have equal number of atoms of each elements on each side of the arrow. Stoichiometric balancing of a chemical reaction means adjusting the coefficients for the reactants and products in equation. CH4 + O2 CO2 + H2O Stoichiometric coefficients are the numbers placed in front of formulas in a chemical equation. Left side contains Right side contains 1C 1C 4H 2H 2O 3O The balanced reaction is, CH4 + 2 O2 CO2 + 2 H2O. 2 H2 (g) 2 molecules H2 two moles of H2 4 grams of H2 reacts with + O2 (g) 2 H2O (s) 1molecules O2 2 molecules H2O one mole O2 and reacts with 32 g O2 and two moles H2O is produced. 36 g H2O is produced. how many moles and grams of H2O are produced by burning 2.72 moles H2 a) in an excess of O2 b) with 1 mol O2 Ballance the following reactions N2H4 + N2O4 NaOH + CO2 CaO + P4O10 N2 + H2O Na2CO3 + H2O Ca3(PO4)2 limiting reactant In a chemical reaction one reactant is completely consumed while some amount of the other reactant/s) remains. The amount of products is limited by that reactant consumed. The reactant that is completely consumed in a chemical reaction limits the amounts of products formed, is called limiting reactant or limiting reagent. • Determine the limiting reactant and the mass of product when 1.20mol of Sb and 2.40mol I2 mixed? Sb + I2 SbI3 Sb:243 I:127.0 what mass of AgBr is formed when a solution containing 3.45 g of KBr is mixed with a solution containing 7.28 g AgNO3? KBr + AgNO3 AgBr + K+ + NO3- Consider the following reaction: Na3PO4 (aq) + Ba(NO3)2(aq) Ba3(PO4)2(s) + NaNO3 (aq) Suppose that a solution containing 3.50 grams of Na3PO4 is mixed with a solution containing 6.40 grams of Ba(NO3)2. How many grams of Ba3(PO4)2 can be formed? Yields of chemical reactions theoretical yield. actual yield. The percent yields The quantity of product that is calculated to form when all of the limiting reactant is consumed in a reaction is called the theoretical yield. The amount of product actually obtained is called the actual yield. The percent yields is the ratio actual yield to the theoretical yield times 100% Soru: Fe + O2 Fe2O3 Reaksiyonunda 11.2g Fe yeteri kadar oksijenle reaksiyona girdiğinde 10.0g Fe2O3 oluşuyor. Reaksiyonun teorik verimi, gerçek verimi ve yüzde verimini hesaplayınız. Fe :56 O:16 Methyl tert-butyl ether (MTBE, ), a substance used as an octane booster in gasoline, can be made by reaction of isobutylene with methanol. What is the percent yield of the reaction if 32.8 g of methyl tert-butyl ether is obtained from reaction of 26.3 g of isobutylene with sufficient methanol? Na3PO4 (aq) + Ba(NO3)2(aq) Ba3(PO4)2(k) + NaNO3 (aq) When 3.50 Na3PO4 reacts ewith 6.40 gram Ba(NO3)2 how many grams of Ba3(PO4)2 will produce? • Soru: 3,00g etilenamin CH3NH2, 0,100g H+ ile reaksiyona girdiğinde 2,60g CH3NH3+ oluştuğuna göre reaksiyonun gerçek verimi ve yüzde verimini hesaplayınız. • CH3NH2, + H+ • → CH 3NH3 CH3NH2, : 31,06 CH3NH3 :32,07 Reactions in Aqueous Solution Precipitation Reactions Acids, Bases, and Neutralization Reactions Oxidation–Reduction (Redox) Reactions Çözelti: Homogeneous mixtures are called solutions solvent solute nonelectrolyte Substances such as sucrose or ethyl alcohol, which do not produce ions in aqueous solution, are called nonelectrolytes. electrolytes Substances such as NaCl or KBr, which dissolve in water to produce conducting solutions of ions, are called electrolytes. strong electrolytes, weak electrolytes. Compounds that dissociate to a large extent (~100%) into ions when dissolved in water are said to be strong electrolytes, compounds that dissociate to only a small extent are weak electrolytes. Mol number m n = --------MA Molarity n M= ------V mol/L m d = ---------V gr/mL density Diluting Concentrated Solutions Minitial x Vinitial = mol number = Mfinal x Vfinal Minitial x Vinitial = Mfinal x Vfinal Find the molarity of a solution that 23.4g of Na2SO4 was dissolved in water and diluted to 250.0ml Na2SO4: 142 calculate the molarity of H2SO4 solution when we dilute 50.0 mL of a solution of 2.00 M H2SO4 to a volume of 200.0 mL. Q1 How can you prepare 500ml 0.10 M H2SO4 solution from 3.0M H2SO4? Q2 How would you prepare 500.0 mL of 0.2500 M NaOH solution starting from a concentration of 1.000 M? What is the final concentration if 75.0 mL of a 3.50 M glucose solution is diluted to a volume of 400.0 mL? Q3 Reactions in Aqueous Solution Precipitation reactions Are the reactions, an insoluble solid is formed, the solid product is called as a precipitate. Ag+(aq) + Cl-(aq) → AgCl(s) solubility rules Soluble salts salts of 1A groups (Na, K, Li,) and NH4+ are soluble all nitrates, acetates and perchlorates are soluble NO3 (Nitrat), CHCOO- (asetat) ,ClO4 (perklorat) all chlorides (halogens) are soluble except (AgCl, Hg2Cl2, PbCl2) most sulfates (SO42+ ) are soluble except (Sr SO4, Ca SO4 , Ba SO4 , Pb SO4 ) Cl-, Br-, I- SO42Li+, Na+, K+, Rb+, Cs+ NH4+ NO3- ClO4- CH3CO2- solubility rules Slightly soluble all OH- hydroxides are insoluble except those of 1A group (Na, K, Li,) and NH4+ all sulfides S2- are insoluble except those of 1A group (Na, K, Li,) and NH4+ all carbonates are insoluble except those of 1A group (Na, K, Li,) and NH4+ All PO43- are insoluble except those of 1A group (Na, K, Li,) and NH4+ CO32-, PO43- OH-, S2- • What will happen if Na2CO3 and CaCl2 solutions are mixed ? • What will happen if CuSO4 and NaNO3 solutions are mixed ? Acids and Bases Asit Baz Have a sour taste, -Have a bitter taste, dissolve metals such as zinc and carbonate minerals -Have a slippery feel -change color of litmus to blue, change color of litmus to red -React with dissolved metal to form prepiciate Asit ve Bazlar Asit- Baz Tanımları Arrhenius Acid-Base Definition (1884) An acid is a substance that contains hydrogen and dissociates to produce Hydrogen ion in water : H+ HCl(aq) H+(aq) + Cl-(aq) A base is a substance that contains the hydroxyl group and dissociates to produce Hydroxide ion : OH – NaOH (aq) Na+ (aq) + OH -(aq) Neutralization is the reaction of an H+ ion from the ion from the base to form water, H2O H+(aq) + OH-(aq) <=> H2O(l) acid and the OH - Asit ve Bazlar Asit- Baz Tanımları Brønsted-Lowry Acid-Base Definition (1923) An acid is a species having a tendency to donate an H+ ion. HCl + H2 O Cl– + H3 O + A base is a species having tendency to accept an H+ ion. NH3 + H2O NH4+ + OHIn the Brønsted-Lowry perspective, one species donates a proton and another species accepts it: an acid-base reaction is a proton transfer process. Asit ve Bazlar The Lewis acid-base definition : A base is any species that donates an electron pair An acid is any species that accepts an electron pair. B + H+ B - H+ Asit ve bazların Kuvvetliliği Kuvvetli Asit Zayıf Asitler Strong Acids; An acid that completely ionized in water, is called as a strong acid Weak acid is an acid that partly ionized in water. HCl H+ + Cl- CH3COOH +H2O CH3COO- + H3O+ HCl, HBr, ve HI HNO3, H2SO4, HClO4 gibi Oksiasitler HF . HCN , H2S HClO, HNO2, ve H3PO4 Organik asitler (RCOOH), CH3COOH C6H5COOH Asit ve bazların Kuvvetliliği Kuvvetli baz Zayıf baz A base that completely ionized in water, is called as a strong base A weak base is a base that partly ionized in water. NaOH Na+ + OH - NH3 +H20 NH4+ + OH - M2O or MOH, M= 1A(1) metalleri (Li, Na, K, Rb, Cs) MO or M(OH)2, M = Group 2A metalleri (Ca, Sr, Ba) [MgO and Mg(OH)2 Amonyak (:NH3) Aminler (RNH2, R2NH, R3N), CH3CH2NH2, (CH3)2NH, (C3H7)3N, C5H5N • pH The pH is defined as the negative logarithm in base 10, of the hydronium ion concentration pH = - log[H3O+] • The pOH is defined as the negative logarithm in base 10, of the hydroxyl ion concentration pOH = - log[OH-] • pH of a neutral solution = 7.00 • pH of an acidic solution < 7.00 • pH of a basic solution > 7.00 Oxidation reduction reactions • Chemical reactions which involve involve electron transfers from one atom to another, are called oxidation-reduction or redox reactions. • • • • Oxidation is the process in which the oxidation number of atoms increase, Reduction is the process in which the oxidation number of atoms is decreased Oxidation is the loss of electrons by an atom reduction is the gain of electrons D Fe2O3(k) + 3 CO(g) → 2 Fe(k) + 3 CO2(g) Fe3+ --- metallic iron CO(g)---- Carbon diokside Fe3+ + Cu+ → Fe2+ + Cu2+ Fe3+ + e- → Fe2+ Cu+ → Cu2+ + e- Oxidation states • • • • • • • • Oxidation states (oxidation numbers) reflect, in general way, how electros are involved in compound formation. the oxidation state(O.S) of an atom in the pure (uncombined) element is 0. The total (sum) of the oxidation state of all the atoms in a molecule or formula unit is 0. For an ion total of the oxidation state is equal to the charge on the ion. In their compounds the alkali metals (1a groups Li, Na, K, Rb, Cs, Fr) have an +1 oxidation number. 2A group metals +2. In its compounds, the oxidation state of hydrogen is +1. but in NaH BeH2 it has OS of -1 O.S. of fluorine is –1. halogens have generally O.S of -1 when they combine with H and metals. In its compounds oxygen has an oxidation state of –2. Balancing Redox reactions 1- Split the equation into two half equation 2- Balance the two half equation same number of electrons must appears in each half equation • balance the atoms of element being oxidized or reduced • balanve oxidation number by adding electrons • balance charge in acidic solutions add H+ add OH in basic solutions • balance hydrogen by adding H2O 3- combine the two half equation eliminate electrons • Soru: Fe2+ + MnO4- → • Soru: Cl2 Fe 3+ + Mn2+ balance in acidic medium + Cr(OH)3 → Cl- + CrO42- balance in basic medium • Soru: C2H5OH + Ce4+ → CO2 + Ce3+ balance in acidic medium Titrasyon • Titration is a procedure for determining the concentration of a solution by allowing a carefully measured volume to react with a standard solution of another substance, whose concentration is known. By finding the volume of the standard solution that reacts with the measured volume of the first solution, the oncentration of the first solution can be calculated. • equivalent point The point that all reactants are consumed, Stoichiometric mol numbers of both reactants are equal. • an indicator a compound that change its color around equivalent point. such as phenolphthalein, is colorless in acidic solution but turns pink in basic solution. • Soru: antiasit ilaç tabletlerinin anabileşeni CaCO3 tür. 0.542 gr olarak tartılan bir tablet HCl ile titre edildiğinde, reaksiyonun tamamlanması için 38.5 ml 0.200M HCl harcandığına göre tablet içindeki CaCO3 yüzdesi nedir? CaCO3 + HCl → Ca2+ + CO2 + Cl- + H2O • Konsantrasyou bilinmeyen bir permanganat çözeltisinin 28,97ml si 0,1058g okzalik asit ile tamamen reaksiyona girdiğine göre permanganat çözeltisinin konsantrasyonunu hesaplayınız. • MnO4- + H2C2O4 → Mn2+ + CO2 2 MnO4- + 5 H2C2O4 6 H+→ 2 Mn2+ + 10 CO2 + 8H2O A 25.0 mL sample of vinegar (dilute acetic acid, ) is titrated and found to react with 94.7 mL of 0.200 M NaOH. What is the molarity of the acetic acid solution?