Consider the following chemical reaction: Cl2 (g) + 2 NaBr (s) ––> 2 NaCl (s) + Br2 (l)
What substance is oxidized in this reaction? (Hint: The substance that is oxidized will contain an element that undergoes an increase in oxidation number during the course of the reaction.)
Consider the following chemical reaction: Cl2 (g) + 2 NaBr (s) ––> 2 NaCl (s) +...
What is the coefficient for NaBr in the balanced version of the following chemical equation: Cl2+NaBr→NaCl+Br2
Match Each reaction to its reaction type: 2 NaBr + Cl2 → 2 NaCl + Br2 Na2SO4 + CaCl2 → CaSO4 + 2 NaCl CH4 + 2 O2 → CO2 + 2 H2O CaCO3 → CaO + CO2 MgO + H2O → Mg(OH)2 HCl + NaOH → NaCl + H2O A. Decomposition B. Double Replacement C. Combustion D. Acid/Base E. Explosion F. Combination G. Single Replacement
Fill in the Blanks Consider the already balanced chemical reaction shown below: KCLO2(s)KCl(s) + O2(g) The oxidation state of K in KCLO2(s) = The oxidation state of Cl in KCLO2(s) = The oxidation state of O in KCLO2(s) = The oxidation state of K in KCl (s) = The oxidation state of Cl in Kcl(s) = The oxidation state of O in O2(g) = The element being oxidized is (K, CI, O) The element being reduced is (K, CI, O)
Consider the following UNBALANCED equation: Na(s) + Cl2(g) -> NaCl(s). a.) Calculate the limiting reagent when 55.0 g of react with 67.2 g of Cl2. (Show all work, and clearly state which is the limiting reagent.) b.) What is the theoretical yield, in grams, of NaCl? c.) If 105g of NaCl is produced from the reaction, what is the percent yield of NaCl?
Consider the following chemical reaction: CH4 (g) + Cl2(g) + CCl4 (1) + CCl4 (I) + HCl (g) Identify the type of chemical reaction that this is classified as: oxidation-reduction (redox) O precipitation + acid-base precipitation + redox precipitation acid-base
Consider the following reaction, 2AB (g) ⇌ A2 (g) + B2 (g) K = 1.50x10−2 At some point in the reaction, Q = 5.30. Which of the following statements is correct concerning the equilibrium? 0.60 mol of Br2 and 0.60 mol of Cl2 are placed in a 1.00 L flask and allowed to reach equilibrium. After reaching equilibrium, the flask is found to contain 0.28 mol of BrCl. What is the value of Kc for this reaction? Br2 (g) + Cl2 (g)...
3. (a) Balance the following equation and then (b) write the half-reaction for the reduction and the half reaction for the oxidation that are taking place in this reaction (hint: NaBr and NaCl are both ionic compounds. The element Na does not change its oxidation state in the reaction but could be included as an ion in half reactions to balance charge and elements): a. NaBr + Cl2 NaCl + Br2b. Reduction half reaction: Oxidation half reaction:
Consider the following reaction:2Na + Cl2(g) → 2NaCl ΔH = -821.8 kJ(a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an enthalpy change of 16.5 kJ? (d) How many kilojoules of heat are absorbed when 44.1 g of NaCl is decomposed into Na and Cl2 at constant pressure?
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow N O 2 ( g ) + C l 2 ( g ) → C l N O 2 ( g ) + C l ( g ) S l o w NO2(g)+Cl(g)→ClNO2(g)Fast a)What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. b)Identify the intermediates in the mechanism. Check all that apply. Check all that apply. NO2(g), ClNO2(g), Cl2(g) ,Cl(g)...
Consider the balanced chemical reaction: Naz S (s)+2 HCI (aq) 2 NaCl (aq) + H,S (g) Part A Complete the change in moles row of the table below. H2Slg) 2 NaCl(aq) Na2S(s) Change 2 HCl(aq) [Select ] in [Select] [Select [Select] moles (An) Part B [Select The moles of H2S produced are equal to the 2 NaCl (aq) + H2 Na2S (s) +2 HCl (aq) Part A Complete the change in moles row of the table below. 2 HCl(aq) Na2S(s)...