Ammonium perchlorate (NH,Clo,) is a powerful solid rocket fuel, used in the Space Shuttle boosters. It decomposes into nitrogen (N,) gas, chlorine (C1,) gas, oxygen (0,) gas and water vapor, releasing a great deal of energy. Calculate the moles of nitrogen produced by the reaction of 1.40 mol of ammonium perchlorate. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.

Ammonium perchlorate (NH,Clo,) is a powerful solid rocket fuel, used in the Space Shuttle boosters. It decomposes into nitrogen (N,) gas, chlorine (C1,) gas, oxygen (0,) gas and water vapor, releasing a great deal of energy. Calculate the moles of nitrogen produced by the reaction of 1.40 mol of ammonium perchlorate. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter1: The Atom In Modern Chemistry

Section: Chapter Questions

Problem 35P: Aluminum oxide (Al2O3) occurs in nature as a mineral called corundum, which is noted for its...

See similar textbooks

Similar questions

How many molec of Al(NO3)3 are in 0.072 mol of Al(NO3)3? Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Abbreviate units as follows: g, mol, molec, atom If molar mass is needed, be sure to use our periodic table and round to the proper number of decimal places. If Avogadro's number is needed, use it to 4 digits. Use the blanks to enter the number, exponent if needed, unit, and substance (in this order) that appears in the numerator of the conversion factor. × 10 Calculate the answer and use the first two blanks to report the value (scientific notation including proper s.f., and exponent), and the final two blanks to report units and substance (in this order). × 10
In 1961, scientists agreed that the atomic mass unit (amu)would be defined as the mass of an atom of 12C. Before then,it was defined as the average mass of an atom of naturally occurring oxygen (a mixture of 16O, 17O, and 18O). The current atomic mass of oxygen is 15.9994 amu. (a) Did Avogadro’snumber change after the definition of an amu changed and, if so,in what direction? (b) Did the definition of the mole change?(c) Did the mass of a mole of a substance change? (d) Before1961, was Avogadro’s number 6.021023(when considered tothree significant figures), as it is today?
Saccharin, a molecular model of which is shown below, is more than 300 times sweeter than sugar. It was first made in 1807, when it was common practice for chemists to record the taste of any new substances they synthesized. (a) Write the molecular formula for the compound, and draw its structural formula. (S atoms are yellow.) (b) If you ingest 125 mg of saccharin, what amount (moles) of saccharin have you ingested? (c) What mass of sulfur is contained in 125 mg of saccharin?
Suppose that the atomic mass of C-12 is taken to be 5.000 amu and that a mole is defined as the number of atoms in 5.000 kg of carbon-12. How many atoms would there be in one mole under these conditions? (Hint: There are 6.0221023 C atoms in 12.00 g of C-12.)
Aluminum oxide (Al2O3) occurs in nature as a mineral called corundum, which is noted for its hardness and resistance to attack by acids. Its density is 3.97gcm3 . Calculate the number of atoms of aluminum in 15.0cm3 corundum.
Assume that the ratio of moles of Cl to moles of Cu are 2.7. If we can represent the formula by CuClx, what is the value for x? Round your answer to the nearest whole number. Do NOT include units. So, if you think the formula is CuCl6, you enter the number 6.
How many g of Si3O5 are in 0.094 mol Si3O5? SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Abbreviate units as follows: g, mol, molec, atom. If molar mass is needed, be sure to use our periodic table and round to the proper number of decimal places. If Avogadro's number is needed, use it to 4 digits. Use the three blanks to enter the number, unit, and substance (in this order) that appears in the numerator of the conversion factor. Calculate the answer and use the first two blanks to report the value (scientific notation including proper s.f., and exponent), and the final two blanks to report units and substance (in this order). × 10
How many molecules of hydrogen fluoride (HF) are in (2.1x10^-2) moles of hydrogen fluoride (HF)? For Avogadro's number use: 6.022 x 1023 Round your answer to two significant figures. For the unit, use the word molecule. Note: Your answer is assumed to be reduced to the highest power possible.
Complete the following table. Formula Number of SO42−SO42− units Number of sulfur atoms Number of oxygen atoms Number of metal ions CaSO4CaSO4 _____ _____ _____ _____ Express your answers as integers separated by commas. NSO42−NSO42−, NSNS, NONO, NCaNCa =
In the air we breathe at 74.0 ∘F∘F and 1.09 atmatm pressure, how many molecules does a typical cubic centimeter contain, assuming that the air is all N2N2. N= ---------- molecules
The empirical formula for C6H13 is-
A given sample of a xenon fluoride compound contains molecules of a single type XeFn , where n is some whole number. Given that 8 x 1020 molecules of XeFn weigh 0.225g, calculate n.