Balance the following chemical equations using the smallest whole number coefficients. Note: You must enter all coefficients, even if the value of the coefficient is 1. For example: _2_ H2(g) + _1_ O2(g) → _2_ H2O(l)     K3PO4(aq) +   BaCl2(aq)→   KCl(aq) +   Ba3(PO4)2(s)   NO2(g) +   H2O(l)→   HNO3(aq) +   NO(g)   Al(s) +   H2SO4(aq)→   Al2(SO4)3(aq) +   H2(g)   Zn(s) +   HCl(aq)→   ZnCl2(aq) +   H2(g)   KOH(aq) +   H2SO4(aq)→   K2SO4(aq) +   H2O(l)

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

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From the list of reactions below, pick out the combustion reactions?        1) 2C2H6(g) + 7O2 (g) →  4CO2(g) + 6H2Ol)           2) MgO(s) + CO2 (g) → MgCO3(s)           3) ZnCO3(s) →  ZnO (s) + CO2 (g)           4) 2CH3OH(l) + 3O2 (g) →  2CO2(g) + 4H2O(l)     a 1, 2, 3, and 4   b 3 and 4   c 2, 3, and 4   d 1, 3, and 4   e 1 and 4

Consider the following chemical reaction: CaO(s) + H2O(l) ----------> Ca(OH)2 (aq) if 1.00 g calcium oxide is mixed with 2.00 g water, calculate grams of the product. CaO = 56.08 g/mole,  H2O = 18.02 g/mole,  Ca(OH)2 = 74.10 g/ mole

6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles

Balance the following equations in which ethane, C2H6, burns in oxygen.    C2H6(g) + O2(g) --> C(s) + H2O(g)    C2H6(g) + O2(g) --> CO(g) + H2O(g)    C2H6(g) + O2(g) --> CO2(g) + H2O(g) d.   Explain why the coefficients for oxygen vary, depending on whether C, CO, or CO2 is formed.

For the reaction C + 2H₂ → CH4, how many moles of hydrogen are needed to make 170.6 grams of methane, CH4 ? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Element Molar Mass Hydrogen 1 Carbon 12

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Balance the chemical equation.