A 23.056-gram sample containing impure calcium nitrite tetrahydrate (Ca(NO2)2· 4H2O, 204.164 g/mol) was heated. The sample...
A 23.056-gram sample containing impure calcium nitrite tetrahydrate (Ca(NO2)2· 4H2O, 204.164 g/mol) was heated. The sample mass after heating to drive off the water was 18.639 grams. What was the mass percent of calcium nitrite tetrahydrate in the original sample?)
*The answer is 54.27%, but I need work shown to get this answer.
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A 23.056-gram sample containing impure calcium nitrite
tetrahydrate (Ca(NO2)2· 4H2O, 204.164 g/mol) was heated. The sample...
What is the molarity of a solution prepared by dissolving 5.90 grams of calcium nitrite [Ca(NO2)2,...
What is the molarity of a solution prepared by dissolving 5.90 grams of calcium nitrite [Ca(NO2)2, molar mass=132.10 g/mol] in enough water to make a 106.0 mL soln?
A 0.5 gram sample of calcium chloride dihydrate (CaCl2 • 2H2O) is heated driving off the...
A 0.5 gram sample of calcium chloride dihydrate (CaCl2 • 2H2O) is heated driving off the water. The dehydrated calcium chloride (CaCl2) weighs 0.38 grams. What was the % H2O by mass? Hint: Just use grams, there is absolutely no need for moles this time. It is not a trick question.
1. After a 6.387 g sample of impure SnCl4.2H2O (Mn=296.7 g/mol) was throughly heated, 5.690 g remained b) How many g...
1. After a 6.387 g sample of impure SnCl4.2H2O
(Mn=296.7 g/mol) was throughly heated, 5.690 g remained
b) How many grams of the hydrate were present in the
sample?
c) What is the % m/m of the hydrate in the sample?
02 IR 4. After a 6.387 g sample of impure Snc.4.2H20 (Mm = 296.7 g/mol) was thoroughly heated, 5.690 g remained a) How many grams of water were present in the sample? SHOW WORK (3 pts) 5.692 g H2O...
A sample of calcium nitrate, Ca(NO3)2, with a formula weight of 164 g/mol. The atomic weight of...
A sample of calcium nitrate, Ca(NO3)2, with a formula weight of 164 g/mol. The atomic weight of Ca is 40.078 g/mol. How many grams of Ca are present in a 100 g sample of Ca(NO3)2?
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol) and CsCl (MW = 168.36...
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol) and CsCl (MW = 168.36 g/mol) originally weighs 1.9715 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl2·6H2O, leaving the anhydrous SrCl2. After cooling the sample in a desiccator, it has a mass of 1.6811 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 1) wt% Sr 2) wt% Cs 3) wt% Cl
11. At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8685-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. Th...
11. At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8685-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 51.2 mL at a temperature of 25°C and a pressure of 731 torr. Calculate the mass percent of NaClO3 in the original sample. (At 25°C the vapor pressure of water is 23.8 torr.)
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of...
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 44.82 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel Mn2+5 Fe34 H20 + 5 Fe2+ MnO8 H concentration g Fe/g steel A 1.969 g...
A student is given a sample of a calcium sulfate hydrate. He places the sample in...
A student is given a sample of a calcium sulfate hydrate. He places the sample in a dry, covered crucible and weighs it. The total mass (crucible, cover, and hydrate) is 19.39219.392 g. The crucible and cover together had previously weighed 17.98717.987 g. He then heats the crucible to redness for 10 minutes with the cover slightly ajar. After the crucible cools, he weighs the crucible and its contents; the mass is now 19.09819.098 g, due to the loss of...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 2.00 L. The salt decomposes when heated, the unbalanced equation for the decomposition reaction is shown below: Pb(NO3)2(s) → PbO(s) + NO2(g) + O2(g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 303 K? Assume the PbO(s) takes up negligible volume.
7A) Butane has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of...
7A) Butane has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of butane is burned in a bomb calorimeter containing 2.610 kg of water initially at 20.13 degrees C, find the final water temperature. 7B) A sample of ethanol (CH3CH2OH) increases the temperature of the bomb calorimeter in Question 7A by 4.71 degrees C. If the heat of combustion of ethanol is -1407 kJ/mol, what was the mass of the ethanol sample? I only need the...
1. After a 6.387 g sample of impure SnCl4.2H2O
(Mn=296.7 g/mol) was throughly heated, 5.690 g remained
b) How many grams of the hydrate were present in the
sample?
c) What is the % m/m of the hydrate in the sample?
02 IR 4. After a 6.387 g sample of impure Snc.4.2H20 (Mm = 296.7 g/mol) was thoroughly heated, 5.690 g remained a) How many grams of water were present in the sample? SHOW WORK (3 pts) 5.692 g H2O...
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 44.82 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel Mn2+5 Fe34 H20 + 5 Fe2+ MnO8 H concentration g Fe/g steel A 1.969 g...
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