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Since you need 46.01 g of nitrogen dioxide in order to have one mole of the compound, it follows that 114.95 g will contain. 114.95g ⋅ 1 mole NO2 46.01g = 2.49837 moles NO2. Rounded to four sig figs, the number of sig figs you have for the molar mass of the compound, the answer will be. nN O2 = 2.498 moles. Answer link.
This means that you can use the number of moles of nitrogen dioxide that react to determine how many moles of nitric acid would be produced. So, use nitrogen dioxide's molar mass to determine how many moles react #80cancel("g") * ("1 mole "NO_2)/(46.006cancel("g")) = "1.74 moles"# #NO_2# That many moles of nitrogen dioxide would produce
"12.65 g NO"_2" can be produced. Start with a balanced equation. "Cu(s) + 4HNO"_3("aq")"rarr"Cu(NO"_3)_2("aq") + "2NO"_2("g") + "2H"_2"O(l)" Calculate mol "Cu" by dividing its given mass by its molar mass ("63.546 g/mol"). Do this by multiplying by the inverse of its molar mass (mol/g). Then multiply by the mol ratio between "Cu" and "NO"_2" in the balanced equation, with "NO"_2" in the ...
The molar mass of nitrogen (N) is approximately 14.01 grams per mole of nitrogen atoms. Molar mass is the quantity of an element in grams for every one mole of atoms of that element. Numerically, it's the same as the element's atomic mass in units of amu (atomic mass units). A mole, or mol for short, is a quantity of any given thing that is equal to 6.02214 * 10^23 particles. This number, 6. ...
40.7 L of "NO"_2 will be produced at STP. > There are four steps involved in this stoichiometry problem: Step 1. Write the balanced chemical equation. "4NH"_3 + "7O"_2 → "4NO"_2 + "6H"_2"O" 2. Convert grams of "NH"_3 to moles of "NH"_3 The molar mass of "NH"_3 is 17.03 g/mol. ∴ "moles of NH"_3 = 30.5 color(red)(cancel(color(black)("g NH"_3))) × ("1 mol NH"_3)/(17.03 color(red)(cancel ...
By using the period table and knowing that hydrogen peroxide of dihydrogen dioxide have 2 hydrogen atoms and 2 oxyagen atoms, we can calculate the molar mass. [2 ⋅ (1.01(g mol))] + [2(16.00(g mol))] = 34.02(g mol) Note: Some tables differ slightly by the atomic mass average. Answer link. Add up the atomic weights of each constituent atom.
What is the mass in grams of 67.2 L of nitrogen dioxide, #NO_2#? Chemistry Measurement Unit Conversions. 1 Answer
4.52 * 10^(23) Your strategy here will be to use the molar mass of nitric oxide, "NO", to determine how many moles you get in that sample. Once you know that, you can use Avogadro's number as a conversion factor to help you determine how many molecules would be present in that many moles. So, nitric oxide has a molar mass of "30.01 g mol"^(-1), which means that one mole of nitric oxide has a ...
The actual number of moles is. nN O2 = V V molar = 99.02L 22.4L = 4.42 moles, which means. mN O2 = n ⋅ molarmass = 4.42moles ⋅ 46 g mole = 203g. Notice the similarity between the estimate and the actual result... The answer is 203g. At STP - Standard Temperature and Pressure (273.15K, 1 atm) - an ideal gas' molar volume is equal to 22.4L ...
Percent composition in chemistry typically refers to the percent each element is of the compound's total mass. The basic equation = mass of element / mass of compound X 100%. For instance, if you had a 80.0 g sample of a compound that was 20.0 g element X and 60.0 g element y then the percent composition of each element would be: