reaction that has a theoretical yield of 10. In the reaction below, identify the reactants. CaCl2...
Thankyou! Consider the following unbalanced equation: O2(g) + C2H6(9) + CO2(g) + H20(1) If 24.7 moles of O2(g) reacts with an excess of C2H6(9), what is the theoretical yield of CO2(g) in moles? O 97.2 moles 14.1 moles 37.7 moles 88.6 moles O 26.8 moles A 1.80 g sample of barium chloride hydrate, BaCl2 mass of 1.72 g. Calculate the value of x. XH2O is treated with excess sulfuric acid, forming a BaSO4 precipitate which has a i ooooo When...
In the combustion of ethanol according to the UNBALANCED reaction below, find the theoretical yield of CO2 in grams if we begin with 100g of C2H5OH C2H5OH(1) + O2(g) --> CO2(g) + H2O(1) give your answer to 2 decimal places Useful information: H = 1.01 g/mol C = 12.01 g/mol O = 16.00 g/mol hint: balance the reaction first!
In the combustion of ethanol according to the UNBALANCED reaction below, find the theoretical yield of CO2 in grams if we begin with 1000g of C2H5OH C2H5OH(I) + O2(g) --> CO2(g) + H2O(1) give your answer to 2 decimal places Useful information: H= 1.01 g/mol C = 12.01 g/mol O = 16.00 g/mol hint: balance the reaction first! 1 pts
Consider the following reaction Ca(s) + 2HCl(aq) --> CaCl2(aq) + H2(g) If the theoretical yield of CaCl2 is 0.736 g and the actual yield is 0.720 g, what is the percent yield? A.)53.0% b.)32.6% c.)95.5% d.)97.8% e.)102%
Suppose the theoretical yield in a reaction is 11.8 g and the percent yield is 58.2 %. What is the 36. actual yield of product obtained? A) 687 g B) 6.87 g C) 20.3 g D) 0.203 g Consider the oxidation of sodium metal to sodium oxide described by the balanced equation: 37. 4 Na+ O2 2 Na:O. What is the theoretical vield of Na:O in grams from 9.0 mol of O? 210 g of Na;O 18 g of Na...
Answer the following for the reaction: CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) What is the molarity of a HCl solution if the reaction of 215. mL of the HCl solution with excess CaCO3 produces 10.7 LL of CO2 gas at 725 mmHg and 18∘C?
QUESTION 1 Consider the following reaction: 4FeCr2O4(s) + 8K2CO3(aq) + 7020) 2Fe2O3(s) + 8K2CrO4(aq) + CO2(g) . 4.0 g of FeCr204 and 6.0 g of K2CO3 were reacted in excess O2. What was the limiting reagent? CO2 o K2CO4 0 02 K2CO3 FeCr204 Fe2O3 QUESTION 2 Consider the following reaction: 4FeCr2O4(s) + 8K2CO3(aq) + 702(g) — 2Fe2O3(s) + 8K2Cro4(aq) + CO2(g) 3.8 g of FeCr204 and 2.8 g of K2CO3 were reacted in excess O2 What was the theoretical yield...
please help fill in this chart using this reaction Na2CO3(aq) + CaCl2*2H2O(aq) -> CaCO3(s)+2NaCl(aq)+2H2O (aq) Given information 1 - CaCl2•2H2O Calcium chloride, dihydrate - 2.5 g 1 - Filter paper, 12.5 cm 1 - Na2CO3 - Sodium carbonate - 2 g 1 - Weighing boat, plastic Initial: CaCl2•2H2O (g) (1 gram) Initial: CaCl2•2H2O (moles) Initial: CaCl2 (moles) Initial: Na2CO3 (moles) Initial: Na2CO3 (g) Theoretical: CaCO3 (g) Mass of Filter paper (g) Mass of Filter Paper + CaCO3 (g) Actual: CaCO3...
What is the theoretical yield (in moles) of MgO that can be formed if you react 3.2 mol of O2 with an excess of magnesium? 2Mg(s) + O2(g) → 2MgO(s)
Question text A limiting reagent is Choose...consumed completelyleft over in excess during a chemical reaction, and it Choose...decreasesincreases the possible amount of product that can be formed. Question 2 Not yet answered Points out of 1 Flag question Question text A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The reaction is: K2CO3(aq) + CaCl2(aq) = CaCO3(s) + 2KCl(aq). Based on the masses of the two reactants given, the limiting reagent is Choose...CaCl2K2CO3 ....