Consider the reaction: C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (l) ΔH = -1.37 x 103 kJ When a 21.1 g sample of ethyl alcohol (molar mass = 46.07 g/mol) is burned, how much energy is released as heat?
The Old Thermodynamist says:Unfortunately, your stoichiometric equation is incorrect, because the combustion reaction produces H2O(g) not H2O(l). Consequently, your value for ΔH is incorrect.The answer to your question is: 21.1g/46.07g/mol = 0.458mol, so the combustion reaction is0.458C2H5OH(l) + 1.374O2(g) = 0.916CO2(g) + 1.374H2O(g) T = 2700CChange in Enthalpy: ΔH(2700C) = -3302kJ (negative, so the reaction is exothermic)So, 3302kJ of heat energy are released by this reaction.NOTE: if this combustion reaction were to have occurred in air instead of oxygen, it would have taken place at 2080C instead of 2700C. In that case, ΔH = -1815.9kJHope this helps!P.S. Whoever told you that the reaction produced liquid water didn’t know much about the flame temperature of ethanol in oxygen — or in air!
Consider the following unbalanced equation C2H5OH(g) + O2(g) CO2(g) + H2O(l)?
Consider the following unbalanced equation C2H5OH(g) + O2(g) CO2(g) + H2O(l) If 2.11 g of ethanol reacts with 10.0 g of oxygen. What is the total volume of gas present (in L) after the reaction is complete, assuming the reaction takes place at 1.00 atm and 25°C? A. 0.547 L B. 9.88 L C. 5.60 L D. 6.52 L E. 2.24 L
Consider the following unbalanced equation?
1) Balanced equation: C2H5OH(g) + 3 O2(g) = 2 CO2(g) + 3 H2O(l) 1mol C2H5OH reacts with 3mol O2 and produces 2 mol CO2 Molar mass C2H5OH = 46.1g/mol 1.1g = 1.1/46.1 = 0.0239 mol C2H5OH This will react with0.0239*3 = 0.0716 mol O2 Molar mass O2 = 32g/mol 14.7g O2 = 14.7/32 = 0.45 You have excess O2. Mol of CO2 is determined from mol of C2H5OH You have 0.0239mol C2H2OH This will produce 0.0239*2 = 0.048 mol CO2 Answer 2) Ba;anced equation: Na2SiF6 + 4 Na = Si + 6 NaF 1mol Na2SiF6 reacts with 4 mol Na 0.313mol Na2SiF6 will react with: 0.313*4 = 1.252 mol Na Molar mass Na = 23g/mol 1.252mol = 1.252*23 = 28.8g Na Answer E) 28.8g Na 3) 2mol A react with 1mol B 3.04mol A will react with 1.52mol B You have excess B, A is the limiting reactant 2mol A produce 3 mol C 3.04mol A will produce 3.04*3/2 =4.56 molC But you produced 4.00mol C % yield = 4.00/4.56*100 = 87.7% your answer is correct.
C2H5OH(l) + PBr3(l) C2H5Br(l) + H3PO3(l) Consider the unbalanced equation above.?
First, balance the equation 3C2H5OH(l) + PBr3(l) -----> 3C2H5Br(l) + H3PO3(l) Now, determine the limiting reagent. To do this, work out how much C2H5Br you would get from the amount of each reagent provided seperately. The one that produces the least C2H5Br is the limiting reagent. 26.0 g of C2H5OH moles C2H5OH = mass / molar mass = 26.0 g / 46.068 g/mol = 0.564383 mol 3 moles of C2HOH react to produce 3 moles of C2H5Br, a 1:1 ratio So moles C2H5Br possible = moles C2H5OH = 0.564383 mol 16.2 g PBr3 moles PBr3 = 16.2 g / 270.67 g/mol = 0.0598515 mol 1 mole PBr3 reacts to produce 3 moles C2H5Br So moles C2H5Br possible = 3 x moles PBr3 = 0.1795544 mol The amount of PBr3 provided yields the least C2H5Br, therefore it is the limiting reagent The theoretical yield of a reaction is the maximum amount of product that can possibly form from the amounts of reagents provided. It occurs if all the limiting reagent is completely used up. We just worked out above that if all the PBr3 were completely consumed we would get 0.1795544 moles of C2H5Br, so this is the theoretical yiled (in moles) mass = molar mass x moles mass C2H5Br = 108.96 g/mol x 0.1795544 mol = 19.5642 g = 19.6 g (3 sig figs) the theoretical yield of C2H5Br is 19.6 g
Reaction enthalpy?
consider the reaction C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l); change in H = -1.37 x 103 kJ Consider the following propositions: I. The reaction is endothermic. II. The reaction is exothermic. III. The enthalpy term would be different if the water formed was gaseous. Which of these propositions is (are) true?
Chemical reactions. ten points will be given?
10. Double replacement (also sometimes called ion combination or metathesis). The Al replaces the Ca and the Ca replaces the Al. In other words, Al and Ca trade partners. 11. a. Single replacement (or oxidation-reduction). Cl replaces the Br. b. Combination. The Fe and S combine to form a single product. c. Combustion (also oxidation-reduction). The reaction with oxygen to produce CO2 and H2O is called combustion.
Chemistry: How do you write a balanced equation for the combustion of ethanol?
Since it is unclear whether complete or incomplete combustion, I'll write down both.Complete combustion:[math]\text{C}_2\text{H}_5\text{OH} +6\text{O}_2 \rightarrow \text{2CO}_2+3\text{H}_2\text{O}[/math]Incomplete combustion:[math]\text{C}_2\text{H}_5\text{OH} +4\text{O}_2 \rightarrow \text{2CO}+3\text{H}_2\text{O}[/math][math]\text{C}_2\text{H}_5\text{OH} +2\text{O}_2 \rightarrow \text{2C}+3\text{H}_2\text{O}[/math]
What is the total volume of gas present (L) after the reaction is complete, assuming the reaction takes place at 1.00 atm and 25oC?
unbalanced equation: C2H5OH(g) + O2(g) CO2(g) + H2O(l) 1.58 g of ethanol reacts with 10.0 g of oxygen. What is the total volume of gas present (in L) after the reaction is complete, assuming the reaction takes place at 1.00 atm and 25oC?