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Chapter 3: Problem 45

The anticaking agent added to Morton salt is calcium silicate, CaSiO \(_{3}\). This compound can absorb up to 2.5 times its mass of water and still remain a free-flowing powder. Calculate the percent composition of \(\mathrm{CaSiO}_{3}\).

Short Answer

Expert verified
The percent composition of CaSiO\(_3\) is 34.50% Calcium (Ca), 24.18% Silicon (Si), and 41.32% Oxygen (O).

Step by step solution

01

Determine the Atomic Masses from the Periodic Table

The atomic masses of calcium (Ca), silicon (Si), and oxygen (O) are 40.08 g/mol, 28.09 g/mol, and 16.00 g/mol, respectively. Therefore, the molar mass of CaSiO\(_3\) is calculated by adding the atomic masses of all the atoms in the formula: (1 x 40.08) + (1 x 28.09) + (3 x 16.00) = 116.17 g/mol.
02

Calculate the Percent Composition of Each Element

Next, compute the percent composition of each element:- Percent composition of Ca = ((1 x 40.08) / 116.17) x 100% = 34.50%- Percent composition of Si = ((1 x 28.09) / 116.17) x 100% = 24.18%- Percent composition of O = ((3 x 16.00) / 116.17) x 100% = 41.32%
03

Summarize the Result

In the compound CaSiO\(_3\), the percent composition of Calcium (Ca) is 34.50%, Silicon (Si) is 24.18%, and Oxygen (O) is 41.32%.

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Most popular questions from this chapter

Octane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) is a component of gasoline. Complete combustion of octane yields \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CO}_{2} .\) Incomplete combustion produces \(\mathrm{H}_{2} \mathrm{O}\) and CO, which not only reduces the efficiency of the engine using the fuel but is also toxic. In a certain test run, 1.000 gal of octane is burned in an engine. The total mass of \(\mathrm{CO}, \mathrm{CO}_{2},\) and \(\mathrm{H}_{2} \mathrm{O}\) produced is \(11.53 \mathrm{~kg} .\) Calculate the efficiency of the process; that is, calculate the fraction of octane converted to \(\mathrm{CO}_{2}\). The density of octane is \(2.650 \mathrm{~kg} / \mathrm{gal}\)

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Calculate the percent composition by mass of all the elements in calcium phosphate \(\left[\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\right],\) a major component of bone.

When heated, lithium reacts with nitrogen to form lithium nitride: $$6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s)$$What is the theoretical yield of \(\mathrm{Li}_{3} \mathrm{~N}\) in grams when \(12.3 \mathrm{~g}\) of \(\mathrm{Li}\) are heated with \(33.6 \mathrm{~g}\) of \(\mathrm{N}_{2} ?\) If the actual yield of \(\mathrm{Li}_{3} \mathrm{~N}\) is \(5.89 \mathrm{~g},\) what is the percent yield of the reaction?

Silicon tetrachloride \(\left(\mathrm{SiCl}_{4}\right)\) can be prepared by heating \(\mathrm{Si}\) in chlorine gas:$$\mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SiCl}_{4}(l)$$In one reaction, 0.507 mole of \(\mathrm{SiCl}_{4}\) is produced. How many moles of molecular chlorine were used in the reaction?
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