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Jr. Member

Joined: 16 Sep 2018
Posts: 5

# HELP!!! I need help with this question

A bottle with a volume of 0.85 L is filled up with CO2 at a pressure of 1.44 atm and temperature of 312 K. Upon adding LiOH into this bottle, it is found that the pressure of CO2 reduces to 0.56 atm because some of CO2 reacts with LiOH. Calculate the amount of Li2CO3 that is generated (Li = 7, C = 12,O = 16, H = 1)

CO2(g) + 2LiOH(aq) = Li2CO3(aq) + H2O(l) [/b]

Jr. Member

Joined: 16 Sep 2018
Posts: 5
 my results do not correspond to the result given by the teacher

Sr. Staff Member

Joined: 27 Sep 2017
Posts: 226
Location: Berlin, Germany
 Show your calculation first. Do you know ideal gas law? What are the constant values in this case. What is relation of mole and pressure.

Jr. Member

Joined: 16 Sep 2018
Posts: 5
 First i calculated the numbers of moles of CO2 using the first pressure given(1,44atm). n=PV/RT n=(1,44)x(0,85)/(0,08206)x(312) n=0,048 mol of CO2 After i did the same using the last pressure given (0,56 atm) using the same volume ,temperature, which give me 0,0189 moles, so i did the difference between the first and the last what give me 0,029 moles, what i supose is the moles of Li2CO3. Lastly i did the stoichiometry to find the mass. 0,029mol Li2C03 x (73,9g Li2CO3/1 mol Li2C03) =2,14 g of Li2CO3 The result given by the teacher is 1,628g.

Sr. Staff Member

Joined: 27 Sep 2017
Posts: 226
Location: Berlin, Germany
 Your calculation is correct. I got the same result. Maybe you can get the calculation from your teacher.

Jr. Member

Joined: 16 Sep 2018
Posts: 5
 Thank you.

Sr. Staff Member

Joined: 27 Sep 2017
Posts: 226
Location: Berlin, Germany
 Do you have the teachers calculation?

Jr. Member

Joined: 16 Sep 2018
Posts: 5
 Not yet, when I have it, I'll post it here.
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