1. 0349 5.2mL 6.5159 3,8479 2²1,7819 20.4989 Weight of Watch Glass, Filter Paper and CuCI Precipitate 26.875 Weight of Copper Volume of Added Nitric Acid Total Weight of Added Sodium Carbonate Weight of Watch Glass and Filter Paper Experimental Yield of CuCl Theoretical Yield of CuCl

D M [Review Topics] [References] Use the References to access important values if needed for this question. For the following reaction, 5.54 grams of oxygen gas are mixed with excess carbon monoxide. The reaction yields 12.1 grams of carbon dioxide. 2CO(g) + O2(g) → 2CO2(g) a. What is the theoretical yield of carbon dioxide? g b. What is the percent yield for this reaction? % Submit Answer Retry Entire Group 6 more group attempts remaining Cengage Learning | Cengage Technical Support Previous Next> Save and Exit

Gaseous methane (CH4) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). What is the theoretical yield of carbon dioxide formed from the reaction of 0.80 g of methane and 2.1 g of oxygen gas? Round your answer to 2 significant figures. THED X 5 ? Explanation Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DII DD J 4) F1 F8 F9 F10 F12 T 0 esc ! 1 @ 2 Check F2 #3 80 F3 S4 $ 000 000 F4 % 5 F5 MacBook Air F6 A 6 & 7 44 F7 * 00 8 ( 9 - F11 + 11 A alo Ar 00 dele

Consider the following chemical reaction HCl (aq)  + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3     Determine the excess reactant   The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction   Determine the type of this chemical reaction

Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 0.689g of water is produced from the reaction of 1.1g of octane and 2.1g of oxygen gas, calculate the percent yield of water.  Round your answer to 2 significant figures.

A 4.86 g quantity of solid rubidiummetal is combined with 3.44 g of magnesium chloride crystals according to this chemical reaction: 2 Rb (s) + 1 MgCl2 (s) 1Mg (s) +2 RbCI (s) What quantity of magnesium metal will be produced? _g Mg round your answer using appropriate sig figs The following molar masses may or may not be needed, but are provided to save you time: • molar mass: Rb = 85.47 g/mol • molar mass: MgCl2= 95.21 g/mol • molar mass: Mg = 24.31 g/mol Hiint: Start with the number of grams of Rubidium

The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.

(0)       Mass of FeCl2 (g) Volume of KMnO4(mL) Molarity of KMnO4 Trial 1 1.9986 33.81 0.0185 Trial 2 2.0237 32.33 0.0185 Trial 3 2.002 33.58 0.0185 The molecular weight of FeCl2 is 151.91 g/mol.   In this assignment, you will determine the mass % of an unknown sample of ferrous chloride (FeCl2) by titrating it with a KMnO4 solution of known concentration. 11. What is the average % iron in the unknown sample using your best three answers?

The theoritical yeild of a certain compound according to a chemical reaction is 127 g. The percent yield is 82.0%. When the reaction is carried out, what is the actual yeild?

1) The Law of Conservation of Mass states that the total mass, in an open system, does not change as the result of reactions between its parts.   True   False   2) The deviation from the theoretical yield to the actual yield is called the percent yield.     True   False