Mo Part B Part \'C Part D 49.575 41.5422 25.73g ,601 g 0 350 41.5.744 25.083a 50
ID: 561444 • Letter: M
Question
Mo Part B Part 'C Part D 49.575 41.5422 25.73g ,601 g 0 350 41.5.744 25.083a 50.537a 1. Mass of crucible and lid (g) 0. 48O 25.732 S 2. Mass of crucible, lid and sample (1.574 3. Mass of sample (g 4. Mass of crucible, lid and product Ist mass measurement () 2nd mass measurement (g) 3rd mass measurement (g) 41.5728, 25.073a 50,5383 4157B3 2573 50.52 0.035g 093 0953 257 50.533 5. Final mass of crucible, lid, and product ()41-577 6. Mass of product (g) 7. Part B. Combination Reaction of Magnesium and Oxygen a. Mass ratio of Mg and O b. Mole ratio of Mg and O c. Consensus empirical formula of magnesium oxide M 100 d. Percent by mass (%) 0 , 0 a 3 % Mig C. 0-1 % 8. Part C. Decomposition Reaction of a Pure Compound a. Mass ratio of CaO and CO2 b. Mole ratio of CaO and CO2 c. Consensus mole ratio of CaO and CO d, Percent by mass (%) % CaO; %CO2 Part D. Combination Reaction of Tin and OxygenExplanation / Answer
You must first be sure the equation is balanced, which it is. Then you must determine the limiting reactant, as that will determine the theoretical yield of calcium carbonate.
CaO(s) + CO2(g) CaCO3(s)
a. The molar mass of CaO(s)=56.077 g/mol. The molar mass of
CO2(g) = 44.099g/mol
Mass ratio of Cao and Co2 is = 56.077/44.099
b.The mole ratios of Cao and CO2 is 1:1.
CaCO3(s)CaO(s)+CO2(g)
This tells us that:
1 mole 1 mole + 1mole
Convert moles to grams
100g 56g + 44g
10g5.6g + 4.4g
This means that 12g of the impure sample must contain 10g of CaCO3 and 2g of impurity.
% impurity = 212×100=17
d. percentage of Mass ratio of Cao and Co2 is = 0.56077/0.44099
Part D;
Tin(II) oxide (stannous oxide) is a compound with the formula SnO. It is composed of tin and oxygen where tin has the oxidation state of +2. There are two forms, a stable blue-black form and a metastable red form.
Blue-black SnO can be produced by heating the tin(II) oxide hydrate, SnO·xH2O (x<1) precipitated when a tin(II) salt is reacted with an alkali hydroxide such as NaOH.
Metastable, red SnO can be prepared by gentle heating of the precipitate produced by the action of aqueous ammonia on a tin(II) salt.
SnO may be prepared as a pure substance in the laboratory, by controlled heating of tin(II) oxalate (stannous oxalate) in the absence of air or under a CO2 atmosphere. This method is also applied to the production of ferrous oxide and manganous oxide.
SnC2O4·2H2O SnO + CO2 + CO + 2 H2O
Tin(II) oxide burns in air with a dim green flame to form SnO2.
2 SnO + O2 2 SnO2
When heated in an inert atmosphere initially disproportionation occurs giving Sn metal and Sn3O4 which further reacts to give SnO2and Sn metal.
4SnO Sn3O4 + Sn
Sn3O4 2SnO2 + Sn
SnO is amphoteric, dissolving in strong acid to give tin(II) salts and in strong base to give stannites containing Sn(OH)3. It can be dissolved in strong acid solutions to give the ionic complexes Sn(OH2)32+ and Sn(OH)(OH2)2+, and in less acid solutions to give Sn3(OH)42+. Note that anhydrous stannites, e.g. K2Sn2O3, K2SnO2 are also known. SnO is a reducing agent and this appears to its role in the manufacture of so-called "copper ruby glass".