2. A mixture weighing 42.500 g contains 7.500 g NH4Cl, 19.650 g SiO2. With the remainder...

2. A mixture weighing 42.500 g contains 7.500 g NH4Cl, 19.650 g SiO2. With the remainder being NaCl. Find the percent by weight of each component. Show your calculations.

Expert Solution

Solution :-

mass of mixture = 42.500 g

mass of NH4Cl = 7.500 g

mass of SiO2 = 19.650 g

mass of NaCl = mass of mixture - [mass of NH4Cl + mass of SiO2]

= 42.500 g - [7.500 g +19.650 g]

= 15.350 g

now lets find the percent of the each

% NH4Cl =( mass of NH4Cl/mixture mass )*100%

=(7.500g/42.500g)*100%

= 17.647 %

% SiO2 = =( mass of SiO2 /mixture mass )*100%

=(19.650 g / 42.500g)*100%

= 46.235 %

%NaCl = =( mass of NaCl/mixture mass )*100%

=(15.35 g/42.500g)*100%

= 36.117 %

queen_honey_blossom answered 2 years ago

The separation of a mixture (NH4Cl, NaCl and SiO2) is accomplished by: (1) heating the mixture...

The separation of a mixture (NH4Cl, NaCl and SiO2) is accomplished by: (1) heating the mixture to sublime the NH4Cl, (2) extracting the NaCl with water, and (3) evaporating water from both the NaCl and SiO2, to yield the dry mixture. Could the separation of these three components be accomplished in any other order while using same techniques? Could the separation of these components be accomplished using other physical methods of separation besides these three? Could please explain this to...

What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250...

What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250 mL of 0.12 NH3? Is the final pH lower than the pH of the 0.12 M ammonia solution?

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water...

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water and an excess of is added, producing a precipitate of . The precipitate is filtered, dried, and weighed. The mass of the precipitate is 1.06 g. What is the mass percent of in the sample? %

A sample weighing 3.027 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3...

A sample weighing 3.027 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not react. If the sample residue (the solid species remaining after the reaction) weighs 2.889 g, what is the mass fraction of Fe2O3 in the original sample?

A sample weighing 3.082 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3...

A sample weighing 3.082 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not react. If the sample residue (the solid species remaining after the reaction) weighs 2.637 g, what is the mass fraction of Fe2O3 in the original sample?

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g...

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total pressure of the mixture is 3.05 atm, what is the partial pressure of each component?

A mixture of CaO(s) and BaO(s) weighing 5.14 g is added to a 1.50 L container...

A mixture of CaO(s) and BaO(s) weighing 5.14 g is added to a 1.50 L container containing carbon dioxide gas at 750.2 torr and 30.2ºC. The oxides react with CO2 to form the metal carbonate, and at the completion of the reaction, the pressure of CO2 is 230.7 torr. What was the mass of calcium oxide in the original mixture?

Question

2. A mixture weighing 42.500 g contains 7.500 g NH4Cl, 19.650 g SiO2. With the remainder...

Solutions

Expert Solution

Related Solutions