Consider the following balanced equation:
2 Co(s) + 3 Br2(l) → 2 CoBr3(s)
How many moles of cobalt(III) bromide are obtained when 11.2 moles of bromine react with excess solid cobalt? Assume the reaction is 100% efficient.
Consider the following balanced equation: 2 Co(s) + 3 Br2(l) → 2 CoBr3(s) How many moles...
Titanium reacts with bromine gas according to the following balanced chemical equation: 2Ti(s)+3Br2(l)→2TiBr3(s) A: What mass of titanium(III) bromide is produced when 139.29 g titanium reacts with 553.73 g bromine liquid? in gTiBr3 B: What is the percent yield of titanium(III) bromide if 556.03 g of titanium(III) bromide is actually obtained?
Consider the following balanced chemical equation: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) a. How many moles of CO2 form when 1.53 moles of C2H5OH react? moles CO2 b. How many moles of H2O form from the reaction of 1.53 moles of C2H5OH? moles H2O c. How many moles of CO2 form when 1.53 moles of H2O form? moles CO2 d. How many molecules of CO2 form when 1.53 moles of H2O form? × 10(Click to select)21222324 molecules CO2
Consider the balanced equation for the following reaction: 2H3PO4(aq) + 3Ca(OH)2(s) → 6H2O(l) + Ca3(PO4)2(s) How much excess reactant remains in the reaction if 7.83 moles of H3PO4 reacts with 1.53 moles of Ca(OH)2? 7.83 moles 2.61 moles 0.510 moles 6.30 moles 6.81 moles
a For the following balanced chemical equation, calculate how many moles of products would be produced if 0.666 mol of the first reactant were to react completely CO (9) + 4H2(g) + CH (9) + 2H, 0(1) mol CH mol H2O b For the following balanced chemical equation, calculate how many moles of products would be produced if 0.441 mol of the first reactant were to react completely. BaCl, (aq) + 2AgNO, (aq) + 2ACI(8) + Ba(NO), (aq) mol AgCI...
Consider the balanced equation for the following reaction: 16HCl(aq) + 2KMnO4(aq) → 5Cl2(g) + 8H2O(l) + 2KCl(s) + 2MnCl2(aq) If 9.20 moles of HCl reacts with 3.57 moles of KMnO4, determine how much excess reactant remains in the reaction. Consider the following unbalanced equation: HCl(aq) + Al(s) → H2(g) + AlCl3(s) If 38.1 moles of HCl(aq) and 18.5 moles of Al(s) are allowed to react, what is the theoretical yield of AlCl3(s) in moles?
Thankyou! Consider the following balanced equation: 502(g) + C3H8(9) 3CO2(g) + 4H20(1) If 19.9 moles of O2(g) and 4.42 moles of CzHg(g) are allowed to react, what is the theoretical yield of CO2(g) in moles? 0 O OOOO 41.0 moles 94.3 moles 36.3 moles 35.3 moles 11.9 moles Consider the balanced equation for the following reaction: 6HCl(aq) + 2Al(s) + 3H2(g) + 2AlCl3(s) How much excess reactant remains in the reaction if 54.1 grams of HCl reacts with 85.8 grams...
A. Classify each of the following reactions as decomposition, combination, combustion, 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) 2KClO3(s)→2KCl(s)+3O2(g) S(s)+3F2(g)→SF6(g) CaO(s)+H2O(l)→Ca(OH)2(aq) 2Cu(NO3)2(s)→2CuO(s)+4NO2(g)+O2(g) B. Solid aluminum metal and diatomic chlorine gas react spontaneously to form a solid product. Give the balanced chemical equation (including phases) that describes this reaction. Indicate the phases using abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Express your answer as a chemical equation. C. When heated, solid copper(II) carbonate decomposes to solid copper(II) oxide and carbon dioxide gas. Give...
Consider the balanced equation for the following reaction: 3H2O(1) + Mg3N2(aq) + 3MgO(s) + 2NH3(g) If Mg3N2 is present in excess, how many moles of H20 are needed to form 4.72 moles of NH3? 05.41 moles O 0.787 moles 3.93 moles 07.08 moles 03.15 moles Calculate the grams of Naf required to form 422 g of sulfur tetrafluoride, according to the reaction? 3 SCl2 + 4 NaF SF4 + S2Cl2 + 4 NaCl 44.69 13109 656 g O 16909 1789...
Time Remaining:03:23 1. Consider the balanced equation for the following reaction: 3Fe2O3(s) + CO(g) + CO2(g) + 2Fe3O4(s) How much excess reactant remains in the reaction if 46.8 grams of Fe2O3 reacts with 22.4 grams of CO? 0.195 moles 0.702 moles 0.800 moles 0.267 moles 0.507 moles Use the slider to rate your confidence on this question 100 Not at all confident Very confident
Consider the following balanced chemical equation: 2H2S(g) + SO2(g) → 3S(s) + 2H2O(g) a. How many moles of H2S must react to form 4.18 moles of S? _ moles H2S b. How many moles of SO2 must react to form 4.18 moles of S? _ moles SO2 c. How many moles of H2S must react to form 4.18 moles of H2O? _ moles H2S d. How many moles of SO2 must react to form 4.18 moles of H2O? _ moles...