For the reaction: NH2OH(aq) + Cr(s) --> N2H4(aq) + Cr(OH)3(s), pH = 10.0 balance the reaction
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For the reaction: NH2OH(aq) + Cr(s) --> N2H4(aq) + Cr(OH)3(s), pH = 10.0 balance the reaction
Balance the following redox reaction in basic solution. Cl (aq)+Cro (aq) - Cl2(g)+Cr(OH)3(s) Cl (aq) Cro (aq) C,(g) Cr(OH), (s)
Given the unbalanced equation, Cr(NO3)3(aq) + LiOH(aq) → LiNO3(aq) + Cr(OH)3(s), how many grams of Cr(OH)3 are produced from 0.56 g of Cr(NO3)3?
Balance each of the following in BASE: Show work A). CrO42-(aq) + Cu(s) Cr(OH)3(s) + Cu(OH)2(s) B). NO2(g) NO3-(aq) + NO2-(aq) D). Zn(s) + NO3-(aq) Zn(OH)42-(aq) + NH3(g) D). Br2(l) BrO3-(aq) + Br -(aq)
2. Consider the following unbalanced redox reaction: CIO2 (aq) Cr(OH)1(s)CI(aq) +Cr04(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients Enter coeffcients for one and zero. Blanks i be marked incorrect.) CIO2 (aq) + Submil Answer Tries 0/3 H20(I) + OH (aq) + Submi AnserTries 0/3 (b) Using the results from part (a), balance the full reaction in acidic conditions with the lowest possible whole number coefficients. (Enter coefficients for one and zero....
[References) Balance the following redox reaction, which takes place in basic solution. Fe(OH),(s) + Cr(s) + Fe(OH),(s) + Cr(OH),(6) (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Fe(OH),(s) + Cr(s) + Fe(OH),(s) + Cr(OH),(s) + Submit Answer Try Another Version 10 item attempts remaining
3. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): Cr0(aq) + U" (aq) → Cr" (aq) +UO; (aq) (b) (acid solution): Cr(s) + O2(g) → Cr* (aq) (C) (basic solution): P. (s) + OH' (aq) → PH; (g) + H2PO2 (aq)
Balance the redox reactions: basic: ClO-(aq)+Cr(OH)4-(aq)----> CrO42-(aq)+Cl-(aq) MnO4-(aq)+Br-(aq)--> MnO2(s)+BrO3-(aq) NO2-(aq)+Al(s)--->NH3(g)+AlO2- Aidic: ClO4-(aq)+Cr(OH)4---->ClO3-(aq)+Cl2(g)
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) MnO4-(aq) + Cl-(aq) Mn2+(aq) + Cl2(aq) MnO4- + Cl- + H+ + H2O Mn2+ + Cl2 + H+ + H2O (b) Cr2O72-(aq) + NO2-(aq) Cr3+(aq) + NO3-(aq) Cr2O72- + NO2- + H+ + H2O Cr3+ + NO3- + H+ + H2O (c) Tl2O3(s) + NH2OH(aq) TlOH(s) + N2(g) Tl2O3 + NH2OH + OH- + H2O TlOH(s) + N2 + OH- + H2O (d) CrO42-(aq) + C2O42-(aq) Cr(OH)3(s) + CO2(g) CrO42- + C2O42- + OH- + H2O Cr(OH)3 + CO2 + OH- + H2O
balance the following redox equation: Mg(s) + Cr^3+ (aq) -------> Mg^2+ (aq) + Cr(s)
Consider the reaction between Cr(OH)3(s) and H2SO4(aq). a) Write the balanced chemical equation. b) Write the net ionic equation with the products soluble in water. c) If one reacts 100.mL of 0.200M H2SO4 with 2.06g of Cr(OH)3(s), how many grams Cr2(SO4)3 will be formed after removal from the water solution?