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Chem chapter 6

QuestionAnswer
Given that the mass of one beryllium atom is 9.01 amu and that of one bromine atom is 79.90 amu, what is the mass ratio of beryllium to bromine? A) 9.01 / 79.90 B) 79.90 / 9.01 C) 9.01 x 79.90 D) 79.90 x 9.01 A
Atomic mass ratios of elements are applicable to A) units of grams. B) units of amu. C) any units of mass. D) any units of moles. C
Given the following atomic masses: O = 15.9994 g/mol and Fe = 55.847 g/mol, how many grams (to 3 significant figures) of oxygen are combined with 75.0 grams of iron to make the iron(II) oxide compound? A) 262 g B) 16.0 g C) 11.9 g D) 21.5 g D
Given the following atomic masses: O = 15.9994 g/mol and Fe = 55.847 g/mol, how many grams (to 3 significant figures) of iron are combined with 75.0 grams of oxygen to make the iron(II) oxide compound? A) 21.5 g B) 11.9 g C) 262 g D) 21.4 g C
What is the mass ratio for the elements in aluminum chloride (AlCl3)? [Al:Cl] A) 27:35.5 B) 27:106.5 C) 0.4:1.0 D) 3.9:1.0 B
If 23.6 g of Na and 23.6 g of I combine to form NaI, how much of which element will be leftover after the reaction? A) I – 130. g B) Na – 4.28 g C) Na – 19.3 g D) I – 106 g C
The value associated with a mole is based on which one of the following isotopes? A) 13C B) 16O C) 24Cr D) 12C D
Having one mole of carbon dioxide means that you have A) 1 g of CO2 B) 1 kg of CO2 C) 6.022x1023 molecules of CO2 D) 1 molecule of CO2 C
Having one mole of carbon dioxide means that you have A) 6.022x1023 moles of carbon B) 6.022x1023 atoms of oxygen C) 1 mole of carbon atoms D) 1 molecule of CO2 C
Which one of the following is not a good example to describe the concept of a mole? A) a herd of elephants B) a dozen eggs C) a 24-pack of soda D) a ream of paper A
Given the atomic mass of Zn = 65.39 g/mol, determine the number of moles in a 15.4-g sample of zinc. A) 0.2355 moles B) 0.236 moles C) 1007 moles D) 1.00x103 moles B
Given that Avagadro's Number is 6.022 x 1023 atoms/mol, if you have 3.33x10-6 moles Sr, then how many atoms of Sr do you have? A) 2.01x1018 atoms B) 1.76x1020 atoms C) 5.68x10-21 atoms D) 4.98x10-19 atoms A
How many moles are in 183.85 g of W? A) 183.85 moles B) 0.00544 moles C) 1.00 moles D) 6.022 x 1023 moles C
Given the atomic mass of Li = 6.941 g/mol, what is the mass of 0.50 moles of Li? A) 3.5g B) 14 g C) 0.072 g D) 7.0 g A
Given the Atomic Mass of Se is 78.96 g/mol, what is the mass of 4.3 moles of Se? A) 340 g B) 18 g C) 2.6 x 1024 g D) 7.1 x 10-24 g A
Given that Avagadro's Number is 6.022 x 1023 atoms/mol and that sample of plutonium is known to contain 4.50 x 1018 atoms. How many moles of plutonium are present? A) 1.08x1021 moles B) 9.30x10-22 moles C) 1.34x105 moles D) 7.47x10-6 moles D
Given that the Atomic Mass of Cobalt is 58.93320 g/mol, if a sample of cobalt is composed of 3.231 moles, what is its mass? A) 190.4 g B) 0.0548 g C) 196 g D) 1.95x1024 g A
What is the mass of one mole of chlorine? A) 35.45 g B) 70.90 g C) 17.72 g D) not enough information B
Monoclinic sulfur (S8) is used in the vulcanization of rubber and in the making of gunpowder. How many moles of sulfur are there in 17.62 g of S8? A) 244.3 mol B) 14.56 mol C) 0.06869 mol D) 0.550 C
Used in the manufacture of rat poisons, white phosphorus exists as cubic crystals containing P4 molecules. What is the mass of 6.431 x 10-3 mol of P4? A) 0.1992 g B) 2.077 x 10-4 g C) 0.04979 g D) 0.7968 g D
A sample of nitrogen gas has a mass of 23.3 g. How many moles of nitrogen are in this sample? A) 1.66 mol B) 326 mol C) 0.832 mol D) 653 mol C
Given the following atomic masses: Fe = 55.847 g/mol and O = 15.994 g/mol, what is the formula weight for iron(III) oxide to 4 significant figures? A) 183.6 amu B) 199.6 amu C) 143.7 amu D) 159.7 amu D
What is the formula weight for barium phosphate, Ba3(PO4)2 to 4 significant figures? A) 232.3 amu B) 507.0 amu C) 601.9 amu D) 559.6 amu C
What is the molar mass for capsaicin (C18H27NO3), which is responsible for the heat of a chili pepper to 4 significant figures? A) 291.4 amu B) 305.4 amu C) 49.0 amu D) 367.0 amu B
Determine the formula weight for cobalt(II) chloride hexahydrate (CoCl2 . 6H2O) to 4 significant figures. A) 112.4 amu B) 237.9 amu C) 147.8 amu D) 202.5 amu B
A sample of N2O5 is known to contain 4.3x1024 molecules. How many nitrogen atoms are in this sample? A) 4.3x1024 atoms B) 8.6x1024 atoms C) 4.3x1048 atoms D) 2.2x1025 atoms B
A sample of N2O5 is known to contain 4.3x1024 atoms of nitrogen. How many oxygen atoms are in this sample? A) 4.3x1024 atoms B) 1.1x1025 atoms C) 1.7x1024 atoms D) 7.1 atoms B
A sample of N2O5 is known to contain 4.3x1024 molecules. What is the mass of this sample? A) 770 g B) 0.066 g C) 2.8x1050 g D) 210 g A
When converting from moles of nitrate ion to moles of aluminum in aluminum nitrate, which of the below mole ratios should be utilized? A) 1 mole of Al/3 mole NO3- B) 3 mole NO3-/1 mole of Al C) 2 mole of Al /3 mole NO3- D) 3 mole of Al /2 mole NO3- A
What is the mass of 0.00322 moles of Na2SO4? A) 0.229 g B) 0.457 g C) 4.41x104 g D) 0.395 g B
The following mole ratio is used to convert from moles of barium to moles of oxygen, (6 mole O/1 mole Ba). For which chemical compound is this ratio applicable? A) Ba(NO3)2 B) BaO C) BaSO3 D) Ba(ClO4)2 A
A sample of dinitrogen tetraoxide has a mass of 1.5 g. How many moles of oxygen are present in this sample? A) 0.016 mol B) 0.326 mol C) 0.023 mol D) 0.065 mol D
A sample of dinitrogen trioxide contains 0.25 moles of oxygen. How many moles of compound are present? A) 0.25 mol B) 0.75 mol C) 0.083 mol D) 0.50 mol C
Given that Avagadro's Number is 6.022 x 1023 atoms/mol and that a sample of Fe2O3 (MM = 159.69 g/mol) contains 5.4x1021 atoms of oxygen. What is its mass? A) 1.4 g B) 0.48 g C) 2.2 g D) 0.96 g B
Given the following atomic masses: Ba = 137.327 g/mol, Cl = 35.4527 g/mol, O = 15.9994 g/mol, what is the percent composition of chlorine in the compound Ba(ClO3)2 to 3 significant figures? A) 23.3% B) 11.7% C) 18.8% D) 16.1% A
The simplest whole-numbered ratio of atoms in a compound is known as the A) molecular formula. B) chemical formula. C) molecular equation. D) empirical formula. D
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