Concept explainers
(a)
Interpretation:To calculate the mass percent composition in CaCl2.
Concept Introduction :
Mass percent composition can be easily calculated by using the below formula:
Let’s say we have a molecule A3B2. Then,
(b)
Interpretation:To calculate the mass percent composition in Na2Cr2O7.
Concept Introduction :
Mass percent composition can be easily calculated by using the below formula:
Let’s say we have a molecule A3B2. Then,
(c)
Interpretation:To calculate the mass percent composition in C2H3Cl3.
Concept Introduction :
Mass percent composition can be easily calculated by using the below formula:
Let’s say we have a molecule A3B2. Then,
(d)
Interpretation:To calculate the mass percent composition in Ca3(PO4)2.
Concept Introduction :
Mass percent composition can be easily calculated by using the below formula:
Let’s say we have a molecule A3B2. Then,
(e)
Interpretation:To calculate the mass percent composition in C18H36O2.
Concept Introduction :
Mass percent composition can be easily calculated by using the below formula:
Let’s say we have a molecule A3B2. Then,
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Basic Chemistry
- An Alka-Seltzer tablet contains 324 mg of aspirin (C.9H8O4,), 1904 mg of NaHCO3, and 1000. mg of citric add (H3C6H5O7). (The last two compounds react with each other to provide the "fizz," bubbles of CO2, when the tablet is put into water.) (a) Calculate the amount (moles) of each substance in the tablet. (b) If you take one tablet, how many molecules of aspirin are you consuming?arrow_forwardA major textile dye manufacturer developed a new yellow dye. The dye has a percent composition of 75.95% C, 17.72% N, and 6.33% H by mass with a molar mass of about 240 g/mol. Determine the molecular formula of the dye.arrow_forwardBauxite, the principal ore used in the production of aluminum, has a molecular formula of Al2O3 2H2O. The H2O in the formula are called waters of hydration. Each formula unit of the compound contains two water molecules. a.What is the molar mass of bauxite? b.What is the mass of aluminum in 0.58 mole of bauxite? c.How many atoms of aluminum are in 0.58 mole of bauxite? d.What is the mass of 2.1 1024 formula units of bauxite?arrow_forward
- Dioxathion, a pesticide, contains carbon, hydrogen, oxygen, phosphorus, and sulfur. The compound has this mass percent composition: 31.57% C; 5.74% H; 21.03% O. The mass percent sulfur is 2.07 times that of phosphorus. Dioxathion has a molar mass of 456.64 g/mol. (a) Determine the empirical formula of dioxathion. (b) Determine the molecular formula of dioxathion. (c) A 57.50 mg dose of this pesticide is administered in a laboratory test. Calculate the amount of dioxathion in this dose. (d) Calculate the number of molecules of dioxathion in the dose.arrow_forwardThe formula mass of an unknown compound containing only C and H is 70.1 amu. What is its molecular formula?arrow_forwardCalculate the mass in grams of each of the following samples. l type="a"> 0.994 mole of benzene, C6H6 i>4.21 moles of calcium hydride 1.79104 moles of hydrogen peroxide, H2O2 i>1.22 rnmol of glucose, C6H12O6(1mmol=11000mole) i>10.6 moles of tin 0.000301 moIe of strontium fluoridearrow_forward
- Uranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. This question considers some uranium chemistry. (a) A small sample of uranium metal (0.169 g) is heated to between 800 and 900 C in air to give 0.199 g of a dark green oxide, UxOy How many moles of uranium metal were used? What is the empirical formula of the oxide, UxOy? What is the name of the oxide? How many moles of UxOy must have been obtained? (b) The naturally occurring isotopes of uranium are 234U, 235U, and 238U. Knowing that uraniums atomic weight is 238.02 g/mol, which isotope must be the most abundant? (c) If the hydrated compound UO2(NO3)2 z H2O is heated gently, the water of hydration is lost. If you have 0.865 g of the hydrated compound and obtain 0.679 g of UO2(NO3)2 on heating, how many waters of hydration are in each formula unit of the original compound? (The oxide Ux, Oy is obtained if the hydrate is heated to temperatures over 800C in the air.)arrow_forwardUranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. This question considers some uranium chemistry. A small sample of uranium metal (0.169 g) is heated to 900 °C in air to give 0.199 g of a dark green oxide, UxOy. How many moles of uranium metal were used? What is the empirical formula of the oxide UxOy? What is the name of the oxide? How many moles of UxOy, must have been obtained? The oxide UxOy is obtained if UO2NO3 · n H2O is heated to temperatures greater than 800 °C in air. However, if you heat it gently, only the water of hydration is lost. If you have 0.865 g UO2NO3 · n H2O and obtain 0.679 g UO2NO3 on heating, how many molecules of water of hydration were there in each formula unit of the original compound?arrow_forward
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