logistic_guy
Full Member
- Joined
- Apr 17, 2024
- Messages
- 424
here is the question
One of the best-selling light, or low-calorie, beers is \(\displaystyle 4.2\%\) alcohol by volume and a \(\displaystyle 12\)-oz serving contains \(\displaystyle 110\) Calories; remember: \(\displaystyle 1\) Calorie \(\displaystyle = 1000\) cal \(\displaystyle = 1\) kcal. To estimate the percentage of Calories that comes from the alcohol, consider the following questions. (a) Write a balanced chemical equation for the reaction of ethanol, \(\displaystyle C_2H_5OH\), with oxygen to make carbon dioxide and water. (b) Use enthalpies of formation in Appendix \(\displaystyle C\) to determine \(\displaystyle ΔH\) for this reaction. (c) If \(\displaystyle 4.2\%\) of the total volume is ethanol and the density of ethanol is \(\displaystyle 0.789\) g/mL, what mass of ethanol does a \(\displaystyle 12\)-oz serving of light beer contain? (d) How many Calories are released by the metabolism of ethanol, the reaction from part (a)? (e) What percentage of the \(\displaystyle 110\) Calories comes from the ethanol?
my attemb
i understand when we burn the ethanol the carbon atom turn into carbon dioxide \(\displaystyle CO_2\) and the hydrogen atom turn into water \(\displaystyle H_2O\) so i need \(\displaystyle 2\) carbon dioxide and \(\displaystyle 3\) water.
\(\displaystyle C_2H_5OH + \cdots \to 2CO_2 + 3H_2O\)
this will balance the right side of the equation. still the left side missing \(\displaystyle 6\) oxygen atoms since i've \(\displaystyle 7\) so i need \(\displaystyle 3\) molecular oxygen. this will give me \(\displaystyle 6\) atoms. the balance chemical equation
\(\displaystyle C_2H_5OH + 3O_2 \to 2CO_2 + 3H_2O\)
reaction is my game, but i'm stuck to solve the rest. appendix \(\displaystyle C\) say
\(\displaystyle ΔH = \sum nΔH_f(products) - \sum mΔH_f(reactants)\)
i know this question is basic, but i'm confused
what's the idea of this summation?
One of the best-selling light, or low-calorie, beers is \(\displaystyle 4.2\%\) alcohol by volume and a \(\displaystyle 12\)-oz serving contains \(\displaystyle 110\) Calories; remember: \(\displaystyle 1\) Calorie \(\displaystyle = 1000\) cal \(\displaystyle = 1\) kcal. To estimate the percentage of Calories that comes from the alcohol, consider the following questions. (a) Write a balanced chemical equation for the reaction of ethanol, \(\displaystyle C_2H_5OH\), with oxygen to make carbon dioxide and water. (b) Use enthalpies of formation in Appendix \(\displaystyle C\) to determine \(\displaystyle ΔH\) for this reaction. (c) If \(\displaystyle 4.2\%\) of the total volume is ethanol and the density of ethanol is \(\displaystyle 0.789\) g/mL, what mass of ethanol does a \(\displaystyle 12\)-oz serving of light beer contain? (d) How many Calories are released by the metabolism of ethanol, the reaction from part (a)? (e) What percentage of the \(\displaystyle 110\) Calories comes from the ethanol?
my attemb
i understand when we burn the ethanol the carbon atom turn into carbon dioxide \(\displaystyle CO_2\) and the hydrogen atom turn into water \(\displaystyle H_2O\) so i need \(\displaystyle 2\) carbon dioxide and \(\displaystyle 3\) water.
\(\displaystyle C_2H_5OH + \cdots \to 2CO_2 + 3H_2O\)
this will balance the right side of the equation. still the left side missing \(\displaystyle 6\) oxygen atoms since i've \(\displaystyle 7\) so i need \(\displaystyle 3\) molecular oxygen. this will give me \(\displaystyle 6\) atoms. the balance chemical equation
\(\displaystyle C_2H_5OH + 3O_2 \to 2CO_2 + 3H_2O\)
reaction is my game, but i'm stuck to solve the rest. appendix \(\displaystyle C\) say
\(\displaystyle ΔH = \sum nΔH_f(products) - \sum mΔH_f(reactants)\)
i know this question is basic, but i'm confused
what's the idea of this summation?