Grignard worksheet-1 (1)

This is my data. Could you help me to find the theoretical yield of acetylsalicylic acid in moles and grams. Also Theoretical yield of dry product as well?

Scientifically, nitrogen and hydrogen at high temperature are converted to ammonia. When 350 grams of Hydrogen gas are added to an excess amount of Nitrogen gas, 80 grams of Ammonia are formed. Calculate the percent yield. * (10 Points) 3H2+ N2> 2NH3

The experimenter uses 3.25 mL of cyclohexanol (d=0.962 g/mL) and isolates 2.05 g of a clear liquid. Determine the yield for the reaction. (Integer only).

3,25

I. Procedure, Results and Observations: 1. Butane is typically used as fuel for cigarette lighters and portable stoves. A. What substance is required for the complete burning of butane? B. Balanced chemical equation for the combustion of butane: C. Calculation: If 74.3 g of butane is burned in 132 kg of oxygen a. Which is the limiting reagent? b. What is the mass of carbon dioxide obtained by heating butane? c. How much of the excess reagent remains unreacted?

7:27 O O @ X all 25% Submission Name: De Ocampo, Cyzvell N. Date: 11-30-21 Strand and Section: 12STEMA7 Teacher: Mr. Reynante S. Santos Homework 7.1| Stoichiometry in Chemical Reactions Directions: Use the balanced chemical equation to solve the following problems. 4Fe + 302 → 2FE203 1. How many moles of Fe,0z are produced when 7.27 grams of Fe is reacted? 1 mel Fe 2 mol Fe203 0.07 or 0.0650 mol Fe203 7.27 gFe 55.85 g Fe 4 mel Fe 2. How many moles of Fe,0, are produced when 19.0 grams of 0, is reacted? 1 mel02 2 Fe203 19:0 g02---- = 0.40 or 0.395 mol Fe203 32 g02 3 mele2 3. How many moles of 0, are needed to react with 25.9 grams of Fe? 1 met-Fe 3 mol 02 = 0.35 mol 02 25.9 Fe 55.85 g Fe 4 met Fe COMMENTS FILES (1) RUBRIC

5. The reaction of gaseous potassium superoxide, KO, is used in life-support systems to replace CO:(g) in expired air with O:(g). The unbalanoced chemical equation for the reaction is given below. KO:(s) + CO:(g) – K:CO:(s) + O:(g) How many moles of K:CO:(s) are produced per milligram of KO2(s) consumed?

Can you make sure the numbers are correctly labeled

12-13

6. You'll use a stoichiometry calculation to predict the mass of aspirin you should obtain if all of the salicylic acid is converted to product. Since you'll do that calculation in today's lab, you'll use a different reaction to demonstrate that you can work stoichiometry problems unassisted: the condensation of ethanoic acid and cyclohexanol (in Question 1). Determine the mass of the ester product that should form when 2.23 grams of ethanoic acid is completely converted to ester with an excess of cyclohexanol. Show all three steps of the stoichiometry calculation (with units), and express your answer with units and the appropriate number of significant figures. ethanoic acid + cyclohexanol 60.05 g/mole 100.16 g/mole ester product + water 142.19 g/mole

Q3.When the Organic Chemistry students carried out the experiment, they weighed out 5.037 g of p-aminophenol and mixed it with excess acetic anhydride. (Show ALL steps and mathematical equations involved in your calculations) Calculate the moles of p-aminophenol (Provide all answers to 4 decimal places)   Calculate the theoretical yield of Acetaminophen (Paracetamol) in moles (Provide all answers to 4 decimal places)    Calculate the theoretical yield of Acetaminophen (Paracetamol) in grams  (Provide all answers to 3 decimal places)

Balance the chemical equation by giving the appropriate coefficient for each molecule in the below chemical reaction. Use a “1” if necessary – do not leave any blanks.  (3 points)                                    _____NCl3 →    _____N2 + _____Cl2

The experimenter uses 3.25 mL of cyclohexanol (d=0.962 g/mL) and isolates 2.05 g of a clear liquid. Determine the yield for the reaction. (Integer only). the answer is NOT 65 or 66 or 67

please answer in the format seen above! ty:)

F any = www-awa.aleks.com/ O CHEMICAL REACTIONS Understanding theoretical, actual, and percent yield Black Forest Biologicals, a biotech startup, has a promising Alzheimer's drug candidate Compound SLT-88 entering Phase I trials this year. SLT-88 is the only product formed by the reaction of two precursor compounds A and B, both of which are quite expensive. The chief medicinal chemist of Black Forest is trying out different reaction conditions to minimize the cost of manufacturing SLT-88. Trial In the table below are listed the initial and final amounts of A and B used under two different trial conditions, and also the actual amount of SLT-88 recovered in each case. Complete the table by calculating the theoretical yield of SLT-88 and the percent yield of SLT-88. Round your amounts to the nearest milligram and your percentages to the nearest whole percent. 1 2 Explanation amount of A initial final 200. mg 0 mg 900. mg Check 0 mg amount of B initial 500. mg final 290. mg 700. mg 490.…

Need help asap! Thanks!!

In terms of % yield = (actual / theorietical ) X 100, explain what is meant by “theorietical”.

Calculate theroetical yield in BOTH grams and mols and percent yield (% by mass) please!

If the percent yield of the reaction below is 78%, how many grams of chlorine gas are needed to produce 315.0 g of PCI3 Show all work on a separate piece of paper and submit work in part B. Clearly label question # and answer. Failure to show work will result in a zero for this question. P4(s) + 6CI2 eDetA 4PCI3(1) Type your answer...

Calculate the theoretical yield of the following experiment. 3.42g of salicylic acid (C7H6O3) was dissolved in excess acetic anhydride (C4H6O3) to produce acetyl salicylic acid (aspirin) (C9H8O4). How many grams of aspirin should be produced in the reaction? Be sure to include proper units with your answer.C7H6O3 + C4H6O3 -> C9H8O4 + C2H4O2

9:55 ull LTE Question 4 of 15 Submit Determine the mass in grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C4H10(g) + 13 O2(g) → CO2(g) + 10 H20(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.0374 2 mol C4H10 1 mol CO2 8.70 44.01 g H20 2.18 4.35 g O2 18.02 208.00 g CH10 126 13 mol H20 10 6.022 x 1023 mol O2 58.14 g CO2 Tap here or pull up for additional resources

Consider the reaction. heat 2 Al(s) + Fe,0,(s) Al,03(s) + 2 Fe(1) If 11.5 kg Al reacts with an excess of Fe,O2, how many kilograms of Al,0, will be produced? mass of Al,0, produced: kg

of a certain Compound X , known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of  128./gmol , is burned completely in excess oxygen, and the mass of the products carefully measured:   product mass carbon dioxide 17.19g water 2.81g Use this information to find the molecular formula of X .

How do I calculate the percent yield for the Grignard reagent experiment? Starting reactants: magnesium and bromobenzene Grignard reagent: phenylmagnesium bromide + benzophenone Product: triphenylmethanol

For the reaction 2 H2O → 2 H2 + O2, how many moles of O2 are produced with 1.45 moles of H2? Your answer should have 2 decimal places. Your Answer: Answer units