Q: Calculate the mass of 2.5 moles of ammonia.
A:
Q: Determine the number of oxygen atoms present in25.0 g of carbon dioxide.
A: From given data Mass of carbon dioxide (CO2) = 25 g Also, Molar mass of carbon dioxide = 44…
Q: A sample of silicon having a mass of 3.43 g combined with oxygen to form a compound with a mass of…
A:
Q: The molar mass for this compound is 208.2 g/mol. The molecular formula for this compound is
A: Given :- Percent by mass of P = 14.88 % Percent by mass of Cl = 85.13% Molar mass of compound =…
Q: Determine the number of atoms in 30.0 g of Ne.
A: One mole of any species contains avagadro number of atoms, molecules and ions.
Q: A sample contains 10.0 g C, 2.5 g H, and 5.0 g of O. Calculate the mass percent composition of…
A: Given: Mass of carbon in the sample = 10.0 g Mass of hydrogen in the sample = 2.5 g Mass of oxygen…
Q: Calculate the mass % of O in beryllium perchlorate.
A: We have to calculate the oxygen % in beryllium perchlorate.
Q: what mass of cobalt contains the same amount of atoms as 57.0 g of flourine
A:
Q: Use the average atomic mass in grams present in 0.432 mol of lithium
A: Number of moles = MassAverage atomic/molar mass
Q: Calculate the mass (in grams) found in 0.805 mol sulfur.
A: Since mass = moles X molar mass Since the formula for sulphur is not given So assuming its natural…
Q: Determine the atoms of O in 5.0 moles of Mg(CIO4)2
A: Given, 5.0 moles of Mg(ClO4)2 and we are asked to determine the number of oxygen atoms in 5.0 moles…
Q: How many atoms of vanadium are in 1.28 grams of vanadium
A: One mole of any chemical substance has Avogadro’s constant or Avogadro’s number of atoms.…
Q: Determine the percentage by mass of an element in "salt"
A: Chemical Formula of Table Salt = NaCl Molar Mass of NaCl = 58.44 g/mol Mass of Element Na = 22.99…
Q: Determine the number of atoms in 30.0 g of S.
A: The given mass of S is 30.0 g The molar mass of S is 32 g The conversion of mass to moles can be…
Q: Calculate the number of oxygen atoms in 24 g of carbon dioxide
A: Molecular weight of CO2 = 12+(16*2) = 44g/mol Molecular weight of oxygen = 16g/mol Molecular weight…
Q: A 1.115-g sample of cobalt was heated with excess sulfur to give 1.722 g of cobalt sulfide. What is…
A: Mass of Co = 1.115 g Mass of S = mass of cobalt sulfide - mass of cobalt = 1.722 -…
Q: Calculate the total number of oxygen ATOMS in 1.926 g of magnesium perchlorate.
A: The total number of atoms available in the molecules of any particular substance is referred to as…
Q: Determine the number of atoms in 30.0 g of Zn.
A: Given that: Mass of zinc = 30.0 g Number of atoms of Zn = ?
Q: Determine the number of atoms in a 48.3-g sample of zinc.
A: Mole is the amount of the substance that contains the same number of particles or atoms or…
Q: Calculate the number of nitrogen atoms in a 150.0 g sample of dinitrogen tetroxide
A:
Q: Calculate the number of moles in 9.364 x 1018 atoms of Ca
A:
Q: Calculate the number of moles of helium that contains 2.79×1021 atoms.
A: Given,Number of helium atoms = 2.79 × 1021
Q: Determine the empirical formula of a compound containing 2.76 g of silicon and 13.9 g of chlorine.
A: Given, mass of Si=2.76 g, molar mass=28 g mol-1 mass of Cl=13.9 g, ,molar mass=13.9 g , molar…
Q: determine the number of atoms of 47.56g of Pa
A:
Q: How many GRAMS of nitrogen are present in 1.62 moles of nitrogen dioxide
A: A mole is expressed as the quantitative amount of a given substance that would contain 6.023 x 1023…
Q: Calculate the mass percentage of each element in vanadium (III) acetate.
A: Given :- name of compound = vanadium (III) acetate To calculate :- mass percentage of each element
Q: Calculate the mass percent composition of bromine in each compound.
A: The mass percent composition of bromine in Br2O =90.89967%
Q: How many oxygen atoms are in 1.70 g of quartz?
A: The chemical formula of quartz is SiO2. The formula mass of SiO2 is 60.08 g. The number of moles (n)…
Q: Calculate the mass of 3.57 mol of vanadium.
A:
Q: Determine the mass in grams of 4.38 × 10²¹ atoms of chromium. (The mass of one mole of chromium is…
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Q: Calculate the mass in grams of 14 atoms of Ca.
A:
Q: determine the number of cations in 0.125 moles of potassium carbonate
A: 1 mole = 6.022 X 1023 Chemical Formula of Potassium Carbonate= K2CO3
Q: Determine the mass, in grams, of 0.575 moles of I (1 mol of I has a mass of 126.90 g).
A: Molar mass of I = 126.9 g
Q: Calculate the mass of 8.65 mole of lithium flouride.
A: A question based on mole concept that is to be accomplished.
Q: 0.933 g sample of Nickle metal is heated in the presence of nitrogne gas forming 1.081 grams of a…
A: Mass of Sample = 0.933 gMass of Nickel Nitride = 1.081 gmoles of Nickel in sample = To be determined…
Q: how many atoms of Fe are in 26.9 g Fe?
A: Given, the mass of iron Fe =26.9 gramwe are asked to calculate the number of atoms of iron Fe in the…
Q: How many moles of magnesium phosphate are present in 4.77 grams of this compound?
A:
Q: Calculate the number of moles of He atoms present in 6.33 g of He.
A: Weight of He = 6.33 gm
Q: Calculate the mass % of O in lithium permanganate.
A: Mass percentage is the term used to calculate the concentration of any element in the given…
Q: Calculate the mass in grams of 422 atoms of potassium K
A:
Q: Determine the number of sodium atoms in 49.78 g of the element.
A: Given: Mass of sodium i.e. Na = 49.78 g.
Q: What is the empirical formula of a molecule containing four sulfur atoms and four fluorine atoms?
A: Note: Since you have posted multiple independent questions in the same request, we will solve the…
Q: Determine the number of moles of Zn atoms in 3.15 g of zinc metal.
A:
Q: Calculate the average mass of 500. atoms of iron (Fe).
A: Atomic mass of one iron atom = 55.845 u molar mass = 55.845 gm/mol Use Avogadro's number to divide…
Q: Calculate the number of grams of lead(Pb) in 46.3 moles of lead
A: Since the relationship between moles and mass of an element is given by Moles = mass / molar mass
Q: Use the average atomic mass to calculate the mass in grams present in 2.56x10^-3 mol of lead
A: Moles of lead = 2.56 × 10-3 moleAverage Atomic mass of lead =207.2 g/mole
Q: Calculate the number of nitrogen atoms in 240. g of ammonium nitrate.
A: The molecular formula of ammonium nitrate is: To calculate the number of moles of ammonium nitrate…
Q: 0.353 g of phosphorus combined with 1.08 g o Empirical formula:
A: Given: 0.353 g of phosphorus combined with 1.08 g of fluorine. To find: empirical formula of the…
Q: How many atoms of Lithium are in 1.00g?
A: The detailed calculation to calculate number of atoms of lithium in 1 gram of Li is provided in a…
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- You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?Assume that the radius of Earth is 6400 km, the crust is 50. km thick, the density of the crust is 3.5 g/cm3, and 25.7% of the crust is silicon by mass. Calculate the total mass of silicon in the crust of Earth.
- A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 ratio and a sample of water vapor? Explain.89 A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluoride gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 K. A mixture of 0.0600 g of Xe and 0.0304 g of F2 is sealed into a 100.0-mL bulb. (The bulb is heated, and the reaction goes to completion. Then the sealed bulb is cooled back to 20.0°C. What will be the final pressure in the bulb, expressed in torr?
- When corn is allowed to ferment, the fructose in the corn is converted to ethyl alcohol according to the following reaction C6H12O6(aq)2C2H5OH(l)+2CO2(g)(a) What volume of ethyl alcohol (d=0.789g/mL) is produced from one pound of fructose? (b) Gasohol can be a mixture of 10 mL ethyl alcohol and 90 mL of gasoline. How many grams of fructose are required to produce the ethyl alcohol in one gallon of gasohol?When calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO3(s)CaO(s)+CO2(g) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?Estimating the radius of a lead atom. (a) You are given a cube of lead that is 1.000 cm on each side. The density of lead is 11.35 g/ cm3. How many atoms of lead are in the sample? (b) Atoms are spherical; therefore, the lead atoms in this sample cannot fill all the available space As an approximation, assume that 60% of the space of the cube is filled with spherical lead atoms. Calculate the volume of one lead atom from this information. From the calculated volume (V) and the formula (4/3) 3 for the volume of a sphere, estimate the radius (r) of a lead atom.
- Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of magnesium ribbon are added to 10 mL of the acid. The volume of the hydrogen gas obtained is a measure of the number of moles of hydrogen produced by the reaction. Various measurements are given in the table below. (a) Draw a graph of the results by plotting the mass of Mg versus the volume of the hydrogen gas. (b) What is the limiting reactant in experiment 1? (c) What is the limiting reactant in experiment 3? (d) What is the limiting reactant in experiment 6? (e) Which experiment uses stoichiometric amounts of each reactant? (f) What volume of gas would be obtained if 0.300 g of Mg ribbon were used? If 0.010 g were used?Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?