# daniaridha

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May 2015
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• ### Dotti22

I would REALLY appreciate some full explanation for this question. The thermal decomposition of sodium hydrogen carbonate, NaHCo3, results in a 73.8% yield of sodium carbonate, Na2Co3. 2NaHCo3=Na2Co3+H2O+Co2 If a 1.68 g sample of sodium hydrogen carbonate is heated, calculate the mass, in g, of sodium carbonate produced.

I would REALLY appreciate some full explanation for this question. The thermal decomposition of sodium hydrogen carbonate, NaHCo3, results in a 73.8% yield of sodium carbonate, Na2Co3. 2NaHCo3=Na2Co3+H2O+Co2 If a 1.68 g sample of sodium hydrogen carbonate is heated, calculate the mass, in g, of sodium carbonate produced.
3. ## HL/SL Chemistry Question

Hi, I would really appreciate a full explanation of the process of the following question Chlorine gas is produced by the reaction hydrochloric acid, and the oxidizing agent manganese (IV) oxide, MnO2: MnO2+ 4HCl = MnCl2 + Cl2 + 2H2O At 273.15 K and 100 Pa, 58.34 g of HCl reacts with 0.35 mol of MnO2 to produce 7.056 dm^-3 of chlorine gas. Deduce the limiting reagent, and calculate the theoretical yield of chlorine.
4. ## Stochiometry Question

A solution of 155 g of potassium iodide, KI is added to a solution of 175 g of nitric acid, HNO3. The acid acts as an oxidizing agent. 6KI + 8HNO3= 6KNO3+2NO+3I2+4H2O A) Deduce which reagent is in excess. B) Determine how many grams of this reactant will remain unreacted. C) Determine how many grams of nitrogen monoxide, NO will be produced.

Hi everyone, if someone could please explain the following question's process to solving the answer it would be highly appreciated 1. Potassium superoxide, KO2, reacts with carbon dioxide, CO2, to produce oxygen and potassium carbonate, K2CO3. Write the balanced equation for this reaction (I already did this- 4KO2+2CO2=3O2+2K2CO3). 28.44 g of KO2 reacts with 22.00 g of CO2. Deduce the limiting reagent, calculate the mass of K2CO3 produced as well as the mass of O2 produced.

Hi everyone, I am trying to revise for my test Monday and I am in need of a little help. Could one please explain the full process of receiving the answer to the following question? It would be GREATLY appreciated

Hi, I would really appreciate some clarification on whether or not I executed the correct process for the following question: Ethyne, C2H2, reacts with oxygen according to 2C2H2+5O2=4CO2+2H2O. What volume of oxygen, in dm3, reacts with 0.40 dm3 of C2H2? Initially, I recognized the ratio of ethyne to oxygen to be 2:5. Then, I cross multiplied 2/5=0.40/x. I received the answer as 1 dm3. Is this correct?

Hi everyone, I would really appreciate some help in solving the following question. I did the process but I wanted to ensure that I achieved the correct answer. Thank you Two aqueous solutions, one containing 5.3 g of sodium carbonate and the other 7.0 g of calcium chloride, are mixed together. A precipitation reaction occurs: Na2CO3+CaCl2=2NaCl+CaCO3 Determine the limiting reagent and the mass, in g, of precipitate formed (theoretical yield).
9. ## Biology HL/SL Help!

Hi everyone, if anyone could please explain how to calculate the magnification of a scale bar that would be highly appreciated. For instance, if you are given a scale bar represented by a 2 micrometre value, and when I measured the scale bar itself it came to 1.8 cm, and the answer is X 8500, how would would actually achieve that answer? Thanks!
10. ## SL/HL Biology Question

If someone could please explain the process of how to calculate magnification given scale bars, that would be greatly appreciated! For instance, the length of a scale bar given is 2 micrometres. When I actually measure the length of the bar, it comes to 1.8 cm. The answer is X 8500. How would I receive this answer?

If you could please help explain the process of how to solve this question, that would be greatly appreciated 1. Butane lighters work by the release and combustion of pressurized butane. 2C4H10+13O2=8CO2+10H2O Determine the limiting reagent in the following reaction. a) 20 molecules of C4H10 and 100 molecules of O2.