8. Balance the following chemical equations and identify the type of reaction: a. ___Si, Na(s)→ __...
Balance the following chemical reaction equations. a. __Na2S(aq) + __CaCl2(g) → _Cas(s) + _NaCl(aq) _C6H180(g) + _ O2(g) → __CO2(g) + c. __C4H2OH() + O2(g) __CO2(g) + d. -_Ca(OH)2(s) + __H3PO4(aq) → TO + H2O(1) NaHCO3(s) + _H2SO4(aq) → H2SO4(aq) → (aq) + __ (g) + ___ H2O(1) _Cd(s) +_ H3PO4(aq) → - _(aq) + _H2(g) 1. Identify each of the following as a salt, acid, base, or hydrocarbon. a. Ammonium hydroxide d. HC2H302 b. CaC204 e. C2H60_ c. Ba(ClO4)2....
an " H" Type: 2. _ Type: Type: 1 13 wuler cr has Balance the following equations and indicate which type of reaction occurred. 1. ___ N2 + __02 _ NO2 Mg + __HCI → __MgCl+__H2 3. __A1+ _02 → ____ A120 F2 + _SnCl2 → _SnF2 +_ Cl2 BaCl2 +_ Na2SO4 → ___ BaSO4 +_ NaCl 6. __H2SO4 +_ NaOH → __Na2SO4+_ _H20 KCIO; → __KCI + ___02 C:His +_02 → __CO2+ _H2O Type: Type: Type: Type: Type:
Choose Question 2 1. Balance the following chemical equations and 2. Classify the type of reaction (acid-base neutralization, combination, decomposition, double-replacement, single replacement. a. Ll(s) + N2(8) LIN(s) b. (NH4)2Cr2O;(s) + N2(g) + Cr2O3(s) + H2O(g) C. SIO2 (s) + C(s) + Si(s) + COG) d. Al(SO4)3 + Na PO, AIPO, + Na, SO e. HF + Ba(OH)2 - BaF+H2O Upload Choose a Fe Question 3 Write the molecular couation, complete ionicouation nettonic equation and endly the samestor roton 1....
Due: Tuesday, November 12 SHOW ALL OF YOUR WORK. 1. Balance each of the following equations. (If the coefficient of a compound is 1, leave the space blank.) A. H3PO4(aq) + Ba(OH)2(aq) → Ba3(PO4)2(s) + H2O(1) B. Al(s) +_ CO(NO3)2(aq) → A(NO3)3(aq) + __Co(s) C. CH3OH(1) + O2(g) → __H2O(l) + __CO2(g) D.__K2MnO4 + __CO2 +_ _H2O → __KMnO4 + __KHCO3 + __MnO2
1 of 1 1) Balance the following redox reaction: Al + Zn → A1 + Zn 2. Balance the follwoing unbalanced chemical equations. Then, write an ionic equation, and a net ionic equation for each equation. Identify the spectator ions a) CaCl(aq) + K3PO(aq) - KClaq) + CaPO(S) LiOH(aq) + H2SO4(aq) → H01) + LigSO4(s) 3. In the reactions a) Pb(s) + 2Ag (aq) - P** (aq) + 2Ag(s) b) FeO3(s) + 3C0(g) 3Fe(s) + 3C0 g) Which species are...
POST-LAB QUESTIONS 1. Balance the following equations and indicate the type of chemical reaction that each represents: a. ___ NH.CI() → ___ NH3(g) + __HCl(g) Type: b. __C(s, graphite). __Ha(e) → _CH(8) Type: c. _ Zn(s) + - FeCl(aq) → ___ ZnCl2(aq) + __Fe(s) Type: d. __C.He(s) - 02(g) → _CO2(g) + __ H2O(1) Type: e. AICI: (aq) + __Hz () Al (s) + HCl(aq) →_ Type: 1. Write balanced chemical equations for each of the following: a. Sodium sulfate...
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
Classify each chemical reaction: Reaction Type Na CO2 (s) → Na20(s) + CO2(8) choose one AgNO3(aq) + NaCl(aq) → NaNO3(aq) + AgCl(s) choose one 2 Mg(s) + 02 (8) ► 2Mgo(s) choose one x 6 ?
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers to each, and write balanced net ionic equations. a) Cu(s) Cu2+(aq) + 2e- b) Cl2(aq) + 2e- Cl-(aq) c) Cu(s) + Cl2(aq) Cu2+(aq) + 2Cl-(aq) d) 4CuO(s) + CH4(g) 4Cu(s) + CO2(g) + 2H2O(l) e) 2CuSO4(aq) + 4KI(aq) 2CuI (aq) + 2K2SO4(aq) + I2(aq) f) Cu2O(s) + Fe(SO4)3 (aq) + H2SO4(aq) 2CuSO4(aq) + 2FeSO4(aq) + H2O(l)
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Half-reaction Identification F2(g) + 2e- 2F-(aq) _________oxidationreduction Al(s) Al3+(aq) + 3e- _________oxidationreduction (2) Write a balanced equation for the overall redox reaction. (Use smallest possible integer coefficients.) (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g)