Which of the following reactions are redox reactions?
Check all that apply.
$$ \begin{array}{l} \mathrm{Mg}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{l}) \rightarrow \mathrm{MgBr}_{2}(\mathrm{~s}) \\ \mathrm{Al}(\mathrm{s})+3 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{Ag}(\mathrm{s}) \\ 4 \mathrm{~K}(\mathrm{~s})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{~K}_{2} \mathrm{O}(\mathrm{s}) \\ \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \end{array} $$
Which of the following reactions are redox reactions? Check all that apply. Check all that apply. Al(s)+3A g + (aq)→A l 3+ (aq)+3Ag(s) S O 3 (g)+ H 2 O(l)→ H 2 S O 4 (aq) Ba(s)+C l 2 (g)→BaC l 2 (s) Mg(s)+B r 2 (l)→MgB r 2 (s)
84. Which reactions are redox reactions? (a) Al(s) + 3 Ag+(aq) -> Al+(aq) + 3 Ag(s) (b) 4 K(s) + O2(g) → 2K2O(s) (c) SO3(g) + H2O(l) → H2SO4(aq) (d) Mg(s) + Brz(1) ► MgBrz(s)
Which of the following reactions are redox reactions? Check all that apply. Check all that apply . Al(s)+3Ag+(aq) = Al3+(aq)+3Ag(s) SO3(g)+H2O(l) = H2SO4(aq) Ba(s)+Cl2(g) = BaCl2(s) Mg(s)+Br2(l) = MgBr2(s)
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
Part A Which of the following reactions are redox reactions? Check all that apply. Check all that apply. Al(s)+3Ag+(aq)→Al3+(aq)+3Ag(s) SO3(g)+H2O(l)→H2SO4(aq) Ba(s)+Cl2(g)→BaCl2(s) Mg(s)+Br2(l)→MgBr2(s)
Classify the following reactions as either: combination, decomposition, combustion, precipitation (metathesis) or redox reactions. C(s) + 4 HNO_3 (aq) rightarrow 4 NO_2 (g) + 2 H_2 O (I) + CO_2 (g) HCI (aq) + NH_3 (aq) rightarrow NH_4 CI(aq) 2HI (g) rightarrow H_2 (g) + I_2 (g) Cu(NO_3)_2 9aq) + Na_2 S (aq) rightarrow CuS(s) + 2 NaNO_3 (aq) Zn(s) + 2 AgNO_3 (aq) rightarrow Zn(NO_3)_2 (aq) + 2 Ag(s) H_2 SO_3 (aq) + 2 KOH(aq) rightarrow K_2 SO_3 (aq)...
A sample of \(\mathrm{N}_{2} \mathrm{O}_{3}\) contains 1 moles of nitrogen. Use the following atomic masses: \(\mathrm{N}=14, \mathrm{O}=16\).$$ \begin{array}{|l|l|l|} \hline \text { The number of moles of } \mathrm{N}_{2} \mathrm{O}_{3} \text { present }= & \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{3} \\ \hline \text { The mass of the sample }= & \mathrm{g} \mathrm{N}_{2} \mathrm{O}_{3} \\ \hline \text { The number of moles of oxygen in the sample }= & & \mathrm{mol} \mathrm{O} \\ \hline \text { The mass of oxygen in the sample...
7. Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350K(a) \(\quad A g^{\prime}(a q)+M g(s) \leftrightharpoons A g(s)+M g^{2 *}(a q)\)(b) \(\mathrm{Cu}^{2 \cdot}(\mathrm{aq})+\mathrm{OH}(\mathrm{aq}) \div \mathrm{Cu}^{+1}(\mathrm{aq})+\mathrm{O}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(1)\)(c) \(\quad \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\mathrm{Fe}^{+1}(\mathrm{aq}) \leftrightarrows \mathrm{Fe}^{-2}(\mathrm{aq})+\mathrm{Mg}(\mathrm{s})+\mathrm{OH}^{-1}(\mathrm{aq})\)8. Complete the following table and comment on the spontancity each reaction.
Balance the following reactions and label the type of reaction. POST-LAB PROBLEMS Balance the following reactions and label the type of reaction. 1. Reaction Type Balance Chemical Reaction CaCO, CaO Co, a. Fe CuSO,(n Cu b. FeSO, 4 (a) Al O2 AlO, C. Na SO BaC NaCl d. BaSO, + 4() CH CO, H,O е. + 2 (g) HCI NaOH (aq) но, f. NaCl KNO, РЫ, * _Pb(NO) KI (ag) 2 (a) 3 (ag) 2 (ag) K,SO H,O H_SO КОН...
23. How many molecules of \(\mathrm{HCl}\) are formed when \(80.0 \mathrm{~g}\) of water reacts according to the following balanced reaction? Assume excess ICl_3.$$ \mathrm{ICl}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{ICl}+\mathrm{HIO}_{3}+\mathrm{HCl} $$A) \(4.46 \times 10^{24}\) molecules \(\mathrm{HCl}\)B) \(2.68 \times 10^{24}\) molecules \(\mathrm{HCl}\)C) \(8.04 \times 1024\) molecules \(\mathrm{HCl}\).D) \(5.36 \times 10^{24}\) molecules \(\mathrm{HCl}\)E) \(4.46 \times 1025\) molecules \(\mathrm{HCl}\)24. Determine the oxidation state of \(\mathrm{P}\) in \(\mathrm{PO}_{3}^{3-}\)A) \(+3\)B) \(+6\)C) \(+2\)D) 0E) - 325. Give the complete ionic equation for the reaction (if any) that occurs when...