2Mg(s) + O2 (g) → 2MgO(s)   The number of moles of oxygen gas needed to react with 4.00 mol of Mg is ________.         A) 1.00 mol       B) 2.00 mol         C) 3.00 mol         D) 4.00 mol

A student has an acid (A) and base (B) solution that they mix together. The acid solution has 10 ml of 2M HCl that has been diluted to a total volume of 40 ml.The base solution (B) is 40 ml of 3 M NaOH.How many moles of H2O will form when solution A and B are mixed together? Which reactant A or B is limiting?

Please help with question 2 G-I

Consider the reaction of ammonia as below: 2 NH3(g) + 5 F2(g) N2F4(g) + 6 HF(g) ----> How many moles of ammonia (NH3) are needed to completely react with 13.6 mol of F2? O 34.0 mol 2.27 mol O 6.80 mol O 5.44 mol

Consider the following unbalanced equation. How many molecules of hydrogen will be required to produce 1.60 mol of water?H2 + O2  H2O

Could someone please Help! No plagiarism Please! 1. Consider the following reaction:  2H₂O (l)    →    2H₂ (g)    +     O₂ (g)                                   Which of the following statements is/are true for this reaction?                     A. This is a synthesis reaction. B. This is a decomposition reaction. C. This is a combustion reaction. D.None of the above   2. The reaction below shows the equation for the combustion of methane gas. How does the chemical equation demonstrate the Law of Conservation of Matter?   A. There is one CH₄ molecule on the reactant side and one CO₂ molecule on the product side of the reaction. B. There are two O₂ molecules on the reactant side and two H₂O molecules on the product side in the reaction. C. There are four oxygen atoms, four hydrogen atoms and one carbon atom on both the reactant and product side of the reaction. D. The reaction does not satisfy the Law of Conservation of Matter.   3. Chemists use the activity…

Classify each equation as either decomposition, combination, or combustion.

Please don't provide handwritten solution .... Help me.

33. You can -Text A 62.5 mL sample of a 0.118 M potassium sulfate solution is mixed with 37.0 mL of a 0.128 M lead(II) acetate solution and the following precipitation reaction occurs: The solid PbSO, is collected, dried, and found to have a mass of 1.00 g - Determine the limiting reactant, the theoretical yield, and the percent yield. ▸ Part A Part B Determine the theoretical yield. mass of PbSO, K₂SO, (aq) +Pb(C₂H₂O₂) (aq) +2KC₂H₂O₂ (aq) + PbSO,(s) ΗΘΕΙ ΑΣΦ Submit Previous Answers Bequest Answer nin * Incorrect; Try Again; 5 attempts remaining ? K

12. Sulfuric acid can dissolve aluminum metal according to the following reaction. 2 Al(s) + 3 H₂SO4(aq) Al2(SO4)3(aq)+3 H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 29.0 g and you have 1.80 L of 1.00 M sulfuric acid available. a) Determine the limiting reactant. What is the theoretical yield of aluminum sulfate? 2/3/22 b) After the reaction is complete, you weigh the aluminum sulfate and it has a mass of 145 g. What is the percent yield of aluminum sulfate?