For the reaction 4Cr (s) + 302 (g) → 2Cr₂O3 (s) calculate how many grams of the product form when 15.4 g of O₂ completely reacts. Assume that there is more than enough of the other reactant. 15. ΑΣΦ Submit ****** ? Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining 6.0 g

Consider the following balanced chemical equation: 2 Na(s) + Cl2 (3) →2 NaCl(s) If 4 moles of sodium chloride are produced, how many moles of chlorine gas are used up? 2.0 mol O 1.0 mol 0.5 mol more information is needed

MISSED THIS? Watch KCV.7.5. IWE 7 Read Section 7.5. You can click on the Review link to access the section in your Text Consider the following reaction: 2CH3OH(g) +30 (g) → 200; (g) + 4H₂O(g) Each of the following molecular diagrams represents an initial mixture of the reactants How many CO₂ molecules would be formed from the reaction mixture that produces the greatest amount of products? Express the number of molecules as an integer. ▸ View Available Hint(s) N-2 ΜΕ ΑΣΦ molecules Submit Each molecule represents a mole of available reactant. To simplify calculations and reporting, the units used in the problem will be molecule X Incorrect: Try Again; 3 attempts remaining First, identify the limiting reactant, which is the substance that is completely consumed during the reaction. You can then determine how much product is produced using the ratio of the limiting reactant to the desired product You may want to review Hint 1. How to approach the problem.

Consider a reaction in which two reactants make one product (for example, consider the unbalanced A + B → C). You know the following: 2.0 mol A (with an excess of B) can make a maximum of 4.0 mol C 3.0 mol B (with an excess of A) can make a maximum of 8.0 mol C If you react 2.0 mol A and 3.0 mol B, what is the maximum amount of C that can be produced?

For the reaction below, find the limiting reactant for each of the initial amounts of reactants. 2 Na(s) + Br2(g) ------> 2 NaBr(s)a. 2 mol Na, 2 mol Br2

how do I do this step by step?

Use only 1 decimal point for the atomic masses. Determine the yield (amount of product) of HCl if 32.5 g of NH4Cl decomposes by the following reaction: NH4Cl(s)-->NH3(g)+HCl(g)

A student heats a 2.8695g sample of a mixture that contains an unknown amount of potassium chlorate (KClO3). The KClO3in the mixture decomposes and releases its oxygen. The mass of the remaining sample residue was 2.0427g. KClO3(s) →KCl (s) + 3 O (g) a.How many grams of oxygen were in the KClO3sample? b.How many moles of oxygen atoms is this? c.How many moles of KClO3were in the original sample? d.How many grams of KClO3were in the original sample? e.What is the % of KClO3in the original sample?

For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants. 2 Na(s) + Br₂(g) → 2 NaBr(s) 2 mol Na, 2 mol Br₂ Express your answer as a chemical formula. Part B A chemical reaction does not occur for this question. Submit Request Answer 1.8 mol Na, 1.4 mol Brą Express your answer as a chemical formula. Submit ΑΣΦ Part C A chemical reaction does not occur for this question. Request Answer ΑΣΦ Submit [MD] 2.5 mol Na. 1 mol Brą Express your answer as a chemical formula. Part D ΑΣΦ A chemical reaction does not occur for this question. Request Answer 12.6 mol Na. 6.9 mol Brą Express your answer as a chemical formula. ΑΣΦ ? ? A chemical reaction does not occur for this question.

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s)