A student calculates a theoretical yield of 10.15 grams of her product. After running her experiment, she weighs her product, which is 8.89 grams. What is her percent yield? % (Omit the units) *SHOW YOUR WORK
Q: Suppose theoretical yield of aspirin is 2.742 g, and the actual experimental yield is 2.180 g. What…
A: Theoretical yield is maximum amount of product that can formed from given amount of reactants. This…
Q: E. Yield Calculation Calculate the unknown in the given problems. Show your solution. Round off your…
A: 1. Calculating the percent yield of MgO: Given,
Q: Part A If the student collected 3.40 g of acetone and the theoretical yield is 3.67 g. what is the…
A: Percentage yield can be calculated through the ratio of actual yield to the theoretical yield of a…
Q: Liquid hexane (CH, (CH,),CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: How many grams O in 283.0 g Fe(OH)3? Molar mass of Fe(OH)3 is 106.867 Hint: 1 mole Fe(OH), has 3 mol…
A: We know that, Number of moles = Given mass / Molar mass Mass = Number of moles x Molar mass Number…
Q: A pharmaceutical company produced a batch of acetaminophen weighing 1,817 kilograms. The…
A:
Q: A clock maker has 16 clock faces. Each clock requires one face and two hands. Part A If the clock…
A: The number of faces clockmaker has is = 16 One clock requires one face and 2 hands.
Q: Liquid hexane (CH, (CH,) CH, reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: Liquid octane (CH, (CH,),CH;) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: Gaseous ethane (CH,CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,)…
A: Ethane reacts with oxygen to form carbon dioxide and water. The equation for the balanced chemical…
Q: Using the following equation: 2 NaOH + H2SO4 --> 2 H2O + Na,SO4 How many grams of sodium sulfate…
A: Given information: Mass of NaOH = 117.2 g
Q: If 1.50 grams of copper (Cu) is reacted with 9.54 grams of silver nitrate (AgNO3) to produce silver…
A: Identifying limiting reactant :
Q: Gaseous ethane (CH,CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,)…
A: Ethane reacts with oxygen to form carbon dioxide and water. The equation for the balanced chemical…
Q: In a lab, a scientist calculated that he should produce 12.3 grams of product in his experiment.…
A: % yield = {theoretical mass/actual mass}×100
Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (o,) to produce gaseous carbon dioxide (co.)…
A:
Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (o,) to produce gaseous carbon dioxide (Co,)…
A: Given, Mass of methane is 0.48g Mass of o2 is 3.3g Actual yield of carbon di oxide is 0.632g
Q: A student measures out exactly 0.101 g of salicylic acid and runs the experiment as dictated in the…
A:
Q: ulfur and Fluorine react in a combination reaction to produce sulfur and hexafluoride. In a…
A: The balanced equation for the given reaction is,
Q: Gaseous butane (CH,(CH,),CH;) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (Co,)…
A:
Q: Gaseous ethane (CH, CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (Co,)…
A:
Q: Platinum is a precious metal that is used as a catalyst for many important industrial reactions.…
A:
Q: 1. The density of vinegar is 1.05 g/mL. The molecular weight of acetic acid is 60.1 g/mol. Using…
A: To determine average percentage of acetic acid in Vinegar
Q: Gaseous butane (CH;(CH,) CH;) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A: Percent Yield is the ratio of actual yield to theoretical yield , multiplied by 100. In this…
Q: Gaseous methane (CH, reacts with gaseous oxygen gas (o,) to produce gaseous carbon dioxide (CO,) and…
A: Recall the reaction that will occur between gaseous methane and gaseous oxygen as follows…
Q: Mr. Ragusa asks Hannah to make copper crystals from the following reaction. Cu(NO3)2 + 2Na -->…
A: Here we are required to find the percent yield of the experiment
Q: In your experiment today will the percent yield of calcium carbonate be higher, lower or unchanged…
A: Each of the experiment will be analysed and the percent yield of calcium carbonate be higher, lower…
Q: Gaseous ethane (CH, CH,) reacts with gaseous oxygen gas (O,) to produce gaseous carbon dioxide (CO,)…
A:
Q: If a student performed part A of this experiment and recorded a 122% yield, what could have been…
A: Please find your solution below : Percentage yield is defined as the percent ratio of actual yield…
Q: 2.Based on your calculations, the experiment should ideally produce 70.22 grams of the product. If…
A:
Q: Gaseous butane (CH, (CH,), CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon…
A: Convert all substantce into mole from mass by dividing molar mass respectively.
Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,)…
A: Given, CH4(g) + O2(g) → CO2(g) + H2O(g) Balancing the above chemical equation: CH4(g) + 2O2(g) →…
Q: (CH,(CH;),CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and…
A:
Q: If the percentage yield is below 100%, what does that mean for your experiment? What possible errors…
A: Stoichiometry word comes from Greek word stoikehein which means element and metron which means…
Q: Gaseous butane (CH;(CH,), CH; reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A: Given Mass of gaseous butane = 1.7 g Molar mass of gaseous butane = 58.12 g/ mole Moles of…
Q: Calculate the %Yield of the 4 fractions based on the following numbers. Compare these numbers with…
A: Since you have asked a question with multiple sub-parts, as per our company guidelines we will solve…
Q: If an experiment theoretically yields 4.65 grams of X but actually yields 7.54 grams of X, what is…
A: While performing experiments including synthesis, Percentage yield helps to calculate and compare…
Q: The actual yield is always greater than the theoretical yield. TRUE FALSE
A: Percentage yield of chemical reaction is defined as the actual yield divided by the theoretical…
Q: 1. In an experiment, the actual yield was 3.26 grams and the theoretical yield was 3.42 grams. What…
A: Only question 1 is being asked. Solution :
Q: In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he…
A: Given that, Theoretical yield= 12.3 g Actual yield=10.1 g % yield =?
Q: Gaseous butane (CH;(CH,), CH;) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: Gaseous methane (CH) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (Co,) and…
A:
Q: Liquid octane (CH,(CH,) CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A: Given: Mass of octane=4.57 g Mass of oxygen gas=12.0 g Mass of water produced (Obtained yield) =2.38…
Q: Liquid octane (CH, (CH .),CH.) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Q: Why might a student obtain a percent yield more than 100% in an experiment? (No human error)
A: Percentage yield: It is one of the measures to find the efficiency of the reaction. It is the…
Q: An amount (in grams) of nitrogen gas is reacted with excess hydrogen, according to the balanced…
A: Ammonia gas is produced from the reaction of nitrogen and hydrogen. Balanced Reaction N2 (g) + 3 H2…
Q: LiOH + KCl ===> LiCl + KOH A scientist began this reaction with 20. grams of lithium hydroxide…
A: To solve this problem we will use the given balanced chemical equations . First we will find the…
Q: A student prepares aspirin using 3.985 grams of salicylic acid (MW = 138 g/mol) and 5.78 mL of…
A:
Q: Liquid octane (CH; (CH,),CH;) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…
A:
Step by step
Solved in 2 steps with 1 images
- 2.Based on your calculations, the experiment should ideally produce 70.22 grams of the product. If you only produced 63.79 grams, what is the percent yield of your product? Record your answer in two decimal places.Naphthalene, a common organic compound, was synthesized during a lab exercise. The theoretical yield was calculated to be 9.3740 g. After the synthesized naphthalene was purified and dried, its mass was taken. The mass of the empty weigh boat used was 0.1055 g and the mass of the weigh boat plus naphthalene was 5.5110 g. What is the percent yield of naphthalene? (Express your answer as a percentage to two decimal places).Platinum is a precious metal that is used as a catalyst for many important industrial reactions. Platinum can be purified by reacting platinum(IV) bromide solution with aluminium metal. To test this purification process, a student reacted 15.0 kg of aluminium metal with excess platinum(IV) bromide solution. After the reaction was complete, the student had extracted 75.4 kg of platinum metal. From this data, calculate the percent error of this experiment.Hint: Write a balanced chemical reaction equation and calculate the theoretical yield of platinum first.Record only your final answer with the correct number of significant digits and the proper units.
- Consider the chemical reaction : 2 Na3PO4 + 3 CaCl2 → Ca3(PO4)2 + 6 NaCl, if the theoretical yield for a reaction is 5.7 grams and the percent yield is 51, what is the actual yield? Round and report your answer to the first decimal place without unit.calcium metal reacts with lead(IV) nitrate in a single displacement reaction. 2.00 g of calcium metal reacts with 9.00 g of lead(IV) nitrate solution. a) Predict of mass of lead metal that should be formed rounding to the correct number of significant digits. b) When you perform the lab, the experiment produces only 3.7 g of lead metal. Determine the percentage yield of the reaction. Round to the correct number of significant digits.Prove that the statement is correct, give the solution and formula of the problem In a lab, a scientist calculated that he can produce 12.3 grams of product in his experiment, after doing so he collected that the product wieghs 10.1 grams therefore his percent yield is 82.1%
- Mr. Ragusa asks Hannah to make copper crystals from the following reaction. Cu(NO3)2 + 2Na --> 2NaNO3 + Cu Mr. Ragusa gives Hannah 86 g of sodium to conduct the experiment. Hannah gives Mr. Ragusa 52 g of copper crystals. What was Hannah's percent yield for her experiment? Please round your answer to 2 decimal places and do not include a unit for your answer.Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s)+3CO(g) → 2Fe(s)+3CO2(g)Fe2O3(s)+3CO(g) → 2Fe(s)+3CO2(g) The reaction of 182 gg of Fe2O3Fe2O3 with 85.8 gg of COCO produces 70.6 gg of FeFe. Calculate the theoretical yield of solid iron. Express the mass in grams to three significant figures. SEE PIC.A reaction for the reduction of copper is shown below (as an unbalanced reaction - that's how I will almost always give you reactions. ALWAYS check to see if a reaction is balanced before you use it. You balanced it in the last question; make sure you have that right before you start calculating!), you are given 3.000 tonnes (3.000x103 kg) of copper oxide. You check and find that you have 404.9 kg of ammonia gas available to you. What mass (in kilograms) of copper(II) oxide will remain unreacted after all the ammonia has been consumed and the reaction stops? CuO(s) + NH3(g) → Cu(s) + H2O(g) + N2(g)
- Could you help me this calculation part? Mass of empty, dry crucible (g): 0.5gMass of crucible with sodium bicarbonate (g): 0.5gMass after first heating (g): 0.5gMass after second heating (g): XgMass after third heating (if needed) (g): YgC a l c u l a t i o n s : Show calculations and include all units. Circle your final answers, and include them in the data section as needed. 1. Calculate the mass of sodium bicarbonate sample used: 2. Calculate the theoretical yield of sodium carbonate based on your starting mass of sodium bicarbonate: 3. Calculate the mass of sodium carbonate obtained (this is your experimental yield): 4. Calculate the percent yield for sodium carbonate: Experimental x 100 = TheoreticalAn amount (in grams) of nitrogen gas is reacted with excess hydrogen, according to the balanced reaction shown below. If 104 g of NH3 is recovered, giving a percent yield of 42%, what was the mass of the nitrogen (in grams) that reacted? N2 (g) + 3 H2 (g) --> 2 NH3 (g) Report your answer as an integer, that is as a number with zero decimal places, and with no units. Do NOT use scientific notation.If the percentage yield is below 100%, what does that mean for your experiment? What possible errors couldhave occurred that resulted in a percentage yield below 100%?