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Consider the following reaction: 2H₂ + O₂ --> 2H₂O How many moles of water can be formed from 2.5 mole of H₂ and 2.7 moles of O₂? Your Answer: 2 Answer moles of v units

For the following reaction, 6.61 grams of benzene (C6H6) are mixed with excess oxygen gas. The reaction yields 18.6 grams of carbon dioxide.benzene (C6H6) (l) + oxygen (g) carbon dioxide (g) + water (g) What is the ideal yield of carbon dioxide?  grams What is the percent yield for this reaction?  %

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

2.80 g of ethene react with chlorine. 8.91 g of dichloroethane are formed. (Ar values: H = 1.0, C = 12.0, Cl= 35.5) Calculate: a the number of moles of ethene that were used b the number of moles of dichloroethane that were formed c the percentage yield d the number of grams of dichloroethane that would have formed if the percentage yield had been 80.0%.

Nitromethane Fuel CH3NO2 is burned with atmospheric air in a stoichiometric ratio. The total number of moles of the products is: Select one: O a. 7.3 O b. 5.82 O c. 10 O d. 4.3

Nitromethane Fuel CH3N02 is burned with atmospheric air in a stoichiometric ratio. The number of moles of air is: Select one: O a. 0.8 O b. 2.1 O c. 3.57 O d. 4.7

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Chem 1101: Elements of Chemistry -. Define the term limiting reactant. .. If 0.80 moles of acetic acid are allowed to react with 0.65 moles of sodium bicarbonate, what is the limiting reactant? How many moles of CO₂ can be produced? (Show your work) 0.8 moles Procedure Obtain five quart-sized Ziplock bags and carefully label them 1-5 with a Sharpie. Obtain five weigh boats and label them 1-5 with a Sharpie. 2 Experiment 11 3 4 JU 0.65 moles sodu 5 2. Place the following amounts of baking soda into the corresponding bag. Be sure to carefull- measure the baking soda by leveling off the measuring spoons with a knife.

In the acetylene torch, acetylene gas (C2H2)(C2H2) burns in oxygen to produce carbon dioxide, water, and energy: How many moles of O2O2 are needed to react with 3.00 molmol of C2H2C2H2? How many moles of CO2CO2 are produced when 4.8 molmol of C2H2C2H2 react? How many moles of C2H2C2H2 are required to produce 0.70 molmol of H2OH2O? How many moles of CO2CO2 are produced when 0.180 molmol of O2O2 reacts?

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 .

For the following reaction: > LIHCO3 Li₂CO3 + H₂O + CO₂ - O a. If 1.25g of Li₂CO3 is added to 0.5g of H₂O, what is the limiting reactant? Li₂CO3 b. H₂O O C. CO₂ O d. LiHCO3

9) Calculate the predicted values for the Final rows, for moles and grams. Complete the ICF table: Reactants Products Balanced CH4 + 202 CO2 + 2H20 Chemical Equation 0.0 0.0 moles 0.0 0.0 grams moles grams moles F grams

For the following reaction, 6.57 grams of potassium hydroxide are mixed with excess carbon dioxide. The reaction yields 7.27 grams of potassium carbonate. carbon dioxide (g) + potassium hydroxide (aq) potassium carbonate (aq) + water (1) What is the theoretical yield of potassium carbonate ? What is the percent yield of potassium carbonate ? grams %

Is the number of total molecules on the left side of a balanced equation always equal to the number or total molecules on the right side of the equation?

For the following reaction, 5.10 grams of aluminum oxide are mixed with excess sulfuric acid. The reaction yields 11.7 grams of aluminum sulfate. aluminum oxide (s) + sulfuric acid (aq) aluminum sulfate (aq) + water (1) What is the theoretical yield of aluminum sulfate ? What is the percent yield of aluminum sulfate? grams %

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

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CALCULATIONS: SHOW COMPLETE "SET-UPS" (and the rounding off) for all calculations on the bottom of this p a separate sheet. Use the correct number of significant figures and correct units. page or on A 1. Mass of PbCrO4 formed 2. Moles of PbCrO4 formed 3. Formula of Limiting Reagent 4. Moles of PbCrO4 predicted by calculation 5. % Difference in moles formed and predicted gnificant figures and correct units. B 44.1248 44.3198 44.2921 A 44.0432 44.3279 44.25979 th both reagents. Briefly, indicate the B

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For the following reaction, 3.66 grams of oxygen gas are mixed with excess propane (C3Hg). The reaction yields 2.34 grams of carbon dioxide. (1) What is the theoretical yield of carbon dioxide? (2) What is the percent yield for this reaction? Submit Answer C3H8 (g) +502 (g) Retry Entire Group % Cengage Learning Cengage Technical Support 3CO₂ (g) + 4H₂O (g) grams 3 more group attempts remaining Previous Email Instructor Next Save and Exit

For the following reaction, 4.59 grams of water are mixed with excess carbon monoxide. The reaction yields 8.28 grams of carbon dioxide. carbon monoxide (g) + water (1) carbon dioxide (g) + hydrogen (g) What is the theoretical yield of carbon dioxide ? grams What is the percent yield of carbon dioxide ?

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How many moles of C3H8 must react with excess O2 to produce 11 moles of CO2? How many moles of H2O are also formed? C3H8 + O2 → CO2 + H20 (unbalanced)