Limiting Reactant Lab Report

Macmillan Learning Combining 0.244 mol Fe₂O, with excess carbon produced 11.1 g Fe. Fe₂O3+3C 2Fe + 3 CO What is the actual yield of iron in moles? actual yield: 1988 What is the theoretical yield of iron in moles? theoretical yield: What is the percen percent yield: TOOLS x10⁰ mol mol

21) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:2NaN3 (s) → 2Na (s) + 3N2 (g)How many moles of N2 are produced by the decomposition of 1.75 mol of sodium azide? 21) ______A) 5.25 B) 0.583 C) 1.17 D) 2.63 E) 0.875

T-Mobile 12:20 PM 65% Question 44 of 59 Submit How many moles of MnO3 are produced when 4.30 kg of oxygen gas completely reacts according to the balanced chemical reaction: 2 Mn(s) + 3 O2(g) → MnO3(s) х STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.001 0.0896 g Mn g MnO3 2 4.30 89.6 mol Mn mol MnO3 3 54.94 9.22 x 103 g O2 022 х 1023 32.00 kg O2 1000 102.94 mol O2

Macmillan Learning Combining 0.205 mol Fe₂O3 with excess carbon produced 19.4 g Fe. Fe₂O3 + 3C →2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: What is the theoretical yield of iron in moles? theoretical yield: What is the percent yield? percent yield: mol mol %

4. Provide the complete balanced chemical equation for the reaction carried out in lab. Calculate the molar mass (molecular weight) of all the chemicals. H₂N + H₂O OH + но OH

Kiley wants to balance the equation H2 + N2 NH3. Which would be her first step in balancing an equation? multiplying the subscripts in the atoms of the reactants together adding the coefficient 3 in front of H2 and the coeffiçient 2 in front of NH3 changing the subscripts so they match for the total number of atoms creating a chart that shows the number of atoms in the reactants and products Submit Next Save and Exit Mark this and return

Based on the mole ratios of the substances in a chemical reaction shown, which is the correct equation for the chemical reaction? Substances Mole ratio A:B 1:2 A:C 1:3 B:C 2:3 A+2B 3C O 3A+2B → C O A+B →C O 6A+ 6B – 20 99+ PrtSc Insert Dele C F5 F6 F7 F8 F9 F10 F11 F12 F4 $4 & * Back 5 6 7 8. 9. Y U G J K Il + ト の

MISSED THIS? Watch KCV: Limiting Reactant, Theoretical Yield, and Percent Yield, IWE: Limiting Reactant and Theoretical Yield; Read Section 4.4. You can click on the Review link to access the section in your eText. For the reaction Mn(s) + O₂(g) → MnO₂ (s) compute the theoretical yield of product (in moles) for each of the following initial amounts of reactants. Part B 5 mol Mn and 7 mol O2 Express your answer using one significant figure. ( Templates Symbols undo redo 2/ Submit Previous Answers Request Answer Part C rese X Incorrect; Try Again; 4 attempts remaining keyboard shortcuts help 26.5 mol Mn and 44.8 mol O₂ Express your answer using three significant figures. Submit ( Templates Symbols undo redo reset keyboard shortcuts help 2/ Request Answer mol mol

Raw Materials: 500 g of Calcium polysulphide (CaSs) 1 500 g of Hydrochloric acid (HCI) Balanced Equation: Cass + 2 HCI → CaCl, + 4 S+ H,S Question: 1) Determine the Limiting Reagent 2) Determine the Excess Reagent

I need help finding the therotical yield and the percent yield by finding the limiting reagent based on the data i need the step by step calculations  benzaldehyde 1.0 ml 20% NAOH 10 ml  95% ethanol 7.6 ml

ZnXqofPk5LcfGlcd5XLvhZQfZRQ8mZaOkAA5mqj9618/edit apidldentity A Classes BELL GoogleDocs DOutlook Limiting Reactants Note Sheet and Practice Problems ☆ D O Saved to Drive Help Last edit was seconds ago BIUA E E E = E 12 21 3 4 3. How many molecules of hydrogen gas will have been produced when the reaction runs out between 4.32 g of aluminum metal and 17.65 g of hydrochloric acid? How much of the excess reactant will remain unreacted? T !!! II

Fill in the Blanks Type your answers in all of the blanks and submit X, X According to the balanced chemical reaction below, calculate the amount of each compound involved if 11 moles of Na3PO₁ reacted completely. 2Na₂PO4 +3MgCl₂ → 6NaCl + Mg3 (PO4)2 The reaction will require The reaction will produce moles of Mg3(PO4)2 Type your answer here Type your answer here Please type your answer to submit Looking for a specific section within the page" moles of MgCl₂ to fully react all of the Na3 PO4 moles of NaCl and Type your answer here Please type your answer to submit There are 2 errors to address before submitting e 4. Resubmit

19)Consider the unbalanced chemical equation below. How many grams of CO2 can you produce from 5.33 x 1025 HCl particles? (assume excess NazCO3) NazCO3 + HCl → CO2 + NaCI + H2O а. 44.3 g b. 1.95 x 103 g с. 1.10 g d. 3.90 x 103 g е. 5.33 х 1024 g

Question 1 of 8 Submit Calculate the theoretical yield in grams All: from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: Al(s) + :(s) – 2 All:(s) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 3 138 1 18.3 0.678 1.47 407.7 277 26.98 mol Alls g/mol Alls mol Al g/mol Al g Alls g Al 2.

WS3 – Percent Yield Date: Name: Period: 1. Explain what % yield is. Use an everyday example. 2. LIOH + KCI -> LICI Кон a) I began this reaction with 20 grams of lithium hydroxide & excess KCI. How much lithium chloride will be produced (in grams)? D) Tactually produced 6 grams of lithium chloride. What is my percent yield? 3. C3H8 5 O2 → 3 CO2 4 H2O a) If I start with 5 grams of C3H8 and excess oxygen gas, how much water would be produced (in grams)? b) I got a percent yield of 75%. How many grams of water did I make? 4. Be + 2 HCI → BeCl2 + H2 My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5 grams, what was my percent yield?

The following diagram represents the reaction of A (red spheres) with B (blue spheres) Y Part A Balance the equation for the reaction, and identity the limiting reactant. Match the items in the left column to the appropriate blanks on the right. Submit 1 2 3 4 5 A₂ B₂ Previous Answers Request Answer A₂+ AB₂ The limiting reactant is Reset Help B₂ →

In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 120 g 240 g 38.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.