Question

Consider the combustion reaction between 24.0 mL of liquid methanol (density=0.850g/mL) and 12.0 L of oxygen...

Consider the combustion reaction between 24.0 mL of liquid methanol (density=0.850g/mL) and 12.0 L of oxygen gas measured at STP. The products of the reaction are CO2(g) and H2O(g).

Calculate the volume of liquid H2O formed if the reaction goes to completion and you condense the water vapor.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the combustion reaction between 25.0mL of liquid methanol (density=0.850g/mL) and 12.5 L of oxygen gas...
Consider the combustion reaction between 25.0mL of liquid methanol (density=0.850g/mL) and 12.5 L of oxygen gas measured at STP. The products of the reaction are CO2(g) and H2O(g). Calculate the volume of liquid H2O (density= 1g/mL) formed if the reaction goes to completion and you condense the water vapor. *assume that oxygen is an ideal gas*
C2H5OH + 3O2 --> 2CO2 + 3 H2O If the combustion uses 55.8 mL of oxygen...
C2H5OH + 3O2 --> 2CO2 + 3 H2O If the combustion uses 55.8 mL of oxygen measured at 2.26 atm and 40 degrees Celsius, what volume of CO2 is produced when measured at STP?
(10) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s). Part A What...
(10) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s). Part A What volume of O2 gas (in L), measured at 778 mmHg and 19 ∘C, is required to completely react with 53.3 g of Al? Part B Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.0 L of methane gas (measured at a pressure of 732 torr and...
Consider the reaction between NO and NO to produce the dimer N2O2. It the reaction is...
Consider the reaction between NO and NO to produce the dimer N2O2. It the reaction is at equilbirium in a closed container, which way will the reaction proceed if the volume of the container is halved? 2NO(g)↔N2O2(g) A No change B Reaction will make more N2O2 C Reaction will make more NO The ΔH for vaporization of water at 25oC is 44.0. What change will occur to the equilibrium between vapor and liquid in a closed container when the temperature...
The next three questions are based on the combustion of propane gas (C3H8) with oxygen to...
The next three questions are based on the combustion of propane gas (C3H8) with oxygen to produce carbon dioxide and water vapor. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Stu Dent measures exactly 5.10 g of C3H8 and burns it with excess oxygen gas. What is his theoretical yield of carbon dioxide gas?  What is his theoretical yield of water vapor?  (Both answers should have 3 significant digits and units of g) Stu measures his experimental products. He finds...
1. Enthalpies and energies of reactions. Consider the combustion of methane, which involves the reaction of...
1. Enthalpies and energies of reactions. Consider the combustion of methane, which involves the reaction of 1 mol CH4(g) with 2 mol of O2(g) to form 1 mol CO2 (g) and 2 mol H2O (l): CH4(g) + 2 O2(g) → CO2(g)+ 2 H2O(l) (a) Using heats of formation from Table 2.6 in the text (or from the tables in the back of the book, or from webbook.nist.gov) calculate ∆Hr◦ for the reaction. (b) Calculate ∆Ur for the reaction by only...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 ∘C). The reaction produces 26.0 L of hydrogen gas measured at STP. What is the percent...
A high temperature reaction vessel is charged with 0.5860 mol of iron powder and 35.1 L...
A high temperature reaction vessel is charged with 0.5860 mol of iron powder and 35.1 L of oxygen gas at STP. 4Fe(s) + 3O2(g) yields 2Fe2O3(s) After the reaction vessel is cooled, and assuming reaction goes to completion, what volume of oxygen remains?
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 ∘C). The reaction produces 26.2 L of hydrogen gas measured at STP. What is the percent...
1. Consider the following chemical reaction: 2CH3OH(l) + 3O2 (g) → 2CO2 (g) + 4H2O(l) Calculate...
1. Consider the following chemical reaction: 2CH3OH(l) + 3O2 (g) → 2CO2 (g) + 4H2O(l) Calculate the number of moles of CO2 produced when 11.25 mL of methanol CH3OH reacted completely with O2 (g). The density of methanol is 0.79 g/mL.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT