Question 3 Lithium carbonate, Li2CO3, is commonly used to treat bipolar disorder. What is the percent by mass of lithium in this compound (to the nearest whole percent)? Mass % =( mass of elmt) x 100 mass of cpd 19% 7% 14% 9% 1275 points Which of the following has the highest boiling point? (Hint: consider the intermolecular forces involved.)

Trinity C. asked • 11/26/18 What is the net ionic equation for the reaction between Li2CO3(aq) and HCl(aq).

2016年2月16日 · Both of the compounds decompose but thermal stability increases as one moves down the group. The reason is that lithium is small size exhibit a stronger ionic charge than potassium, therefore bonding more covalently with the carbon atom in CO 3 - .

the balanced equation is 2LiOH+CO2>Li2CO3+H2O What mass of lithium carbonate will be formed by reacting 3.80kg of lithium hydroxide with excess carbon dioxide. This problem has been solved! You'll get a detailed solution from a subject matter expert that …

Question: 2LiOH(s) + CO2(g) -----> Li2CO3(s) +H2O (l) #1- Calculate the theoretical CO2 absorption capacity of 0.070 grams of lithium, assuming a complete reaction and absorption has occurred. #2- Calculate the experimental CO2 absorption capacity of 0.070 grams of LiOH, assuming the CO2 volume change measured was 23.0 mL.

Identify the molar mass of each component atom in the Li2CO3 molecule; the molar mass of lithium (Li) is approximately , carbon (C) is approximately , and oxygen (O) is approximately . Step 1 View the full answer

Calculate the molar mass for lithium carbonate, Li2CO3, used to treat bipolar disorder. 1) Obtain the molar the molar mass of each element. Li (in g/mol) , C (in g/mol) and O (in g/mol) b) Multiply each molar mass by the number of moles (subscript) in the formula. Grams from 2 moles of Li: Grams from 1 mole of C: Grams from 3 moles of O:

Which of the following submicroscopic representations best represents Li2CO3? Your solution’s ready to go! Our expert help has broken down your problem into an easy-to-learn solution you can count on.

2021年3月30日 · 90 moles of CO2 are captured in the reaction to form Li2CO3. The balanced equation says we'll get 1 mole Li2CO3 for every 1 mole of CO2 consumed. That means 90 moles of Li2CO3 will form over the two days. (90 moles LiCO3)*(75g/mole Li2CO3) = 6750 g LiCO3 formed. That's 6.75 kgof Li2CO3, under the 7.5kg limit, assuming the H2O can be expelled.

2 LiHCO3 (s) arrow Li2CO3 (s) +CO2 (g) +H2O (g) Part A) a mixture of LiHCO3 and sand weighing 8.41 g is heated. After cooling, the residue composed of Li2CO3 and sand weighs 6.80g. Assuming that the sand in the sample is unaffected by the heat, calculate the mass loss due to the escape of gaseous CO2 and H2O.