Amount of NH3 = 10.0/17.0 = 0.588mol
The ratio of H to NH3 is 3:1.
Amount of H = 3 x 0.588 = 1.76mol
Mass of H = 1.0 x 1.76 = 1.76g
Ammonia is composed of one nitrogen atom and three hydrogen atoms. The molar mass of ammonia is 17.03 g/mol, with 3.04 g/mol from the hydrogen atoms. To find the grams of hydrogen in 10.0 g of ammonia, we need to calculate the proportion of hydrogen in the compound. This comes out to 3.04 g H x (10.0 g NH3 / 17.03 g NH3) = 1.79 g H.
The molar mass of ammonia (NH3) is 17.03 g/mol. Hydrogen's molar mass is 1.01 g/mol. The mass of hydrogen in ammonia is 3.03 g (3*1.01). To find the mass percentage of hydrogen in ammonia: (3.03 g / 17.03 g) * 100% ≈ 17.8%.
To find the percent yield, first calculate the theoretical yield of ammonia based on the given amounts of nitrogen and hydrogen. Then compare the actual yield (62g) with the theoretical yield to calculate the percent yield using the formula: (actual yield/theoretical yield) x 100%. The percent yield would be the actual mass of ammonia produced (62g) divided by the theoretical yield of ammonia.
lets see. H20 you have 2.016 grams of hydrogen here to 16.0 grams oxygen 2.016/16.0 X 100 = 12.6% hydrogen by mass H2O2 you have the same 2.016 grams hydrogen here, but you have 32.0 grams oxygen in this molecule 2.016/32.0 X 100 = 6.3% so H2O has the higher percent by mass of hydrogen
To determine the number of molecules in 100 grams of hydrogen chloride gas, you need to first calculate the number of moles present using its molar mass. The molar mass of HCl is about 36.5 g/mol. Then, you can use Avogadro's number (6.022 x 10^23) to convert moles to molecules.
100 micrograms is equal to 0.0001 grams.
For carbon 0.80 x 100 = 80 grams of carbon; and for hydrogen 0.20 x 100 = 20 grams of hydrogen
The molar mass of ammonia (NH3) is 17.03 g/mol. Hydrogen's molar mass is 1.01 g/mol. The mass of hydrogen in ammonia is 3.03 g (3*1.01). To find the mass percentage of hydrogen in ammonia: (3.03 g / 17.03 g) * 100% ≈ 17.8%.
For this you need the atomic (molecular) mass of NH3. Take the number of moles and multiply it by the atomic mass. Divide by one mole for units to cancel. NH3=16.0 grams100 grams NH3 / (16.0 grams) = 6.25 moles NH3
To find the percent yield, first calculate the theoretical yield of ammonia based on the given amounts of nitrogen and hydrogen. Then compare the actual yield (62g) with the theoretical yield to calculate the percent yield using the formula: (actual yield/theoretical yield) x 100%. The percent yield would be the actual mass of ammonia produced (62g) divided by the theoretical yield of ammonia.
Onions do not naturally contain ammonia. They contain sulfur compounds that can produce a pungent smell and flavor when the onion is chopped or crushed, but this is different from the smell of ammonia.
100 grams = 3.5 ounces.
For the reaction 2H₂ + O₂ → 2H₂O, we know that the molar ratio of H₂ to O₂ is 2:1. To produce 900 grams of water, we need 450 grams of hydrogen (900g / 2). Therefore, we need to add 450 grams of hydrogen to 800 grams of oxygen to produce 900 grams of water.
100 grams is 3.527 ounces.
.1 Kg = 100 grams
To find the mass of water containing 5.0 grams of hydrogen, we need to set up a proportion using the mass percentage of hydrogen in water. Since water is 11.2% hydrogen by mass, we can calculate the mass of water using the formula: (5.0 grams of hydrogen) / (11.2 grams of hydrogen per 100 grams of water) = x grams of water. Converting grams to kilograms, the mass of water containing 5.0 grams of hydrogen would be 5.0 g / 11.2% = 44.64 g. This figure converted to kilograms is 0.04464 kg.
lets see. H20 you have 2.016 grams of hydrogen here to 16.0 grams oxygen 2.016/16.0 X 100 = 12.6% hydrogen by mass H2O2 you have the same 2.016 grams hydrogen here, but you have 32.0 grams oxygen in this molecule 2.016/32.0 X 100 = 6.3% so H2O has the higher percent by mass of hydrogen
It's a straight-forward stochiometric calculation. But first, we need to ask the question a bit more precisely. For example, how many Hydrogen atoms are in 100 milliliters (i.e. about 100 grams) of 10% ammonia in water (no soaps or surfactants). ACE hardware brand is about as pure a "cleaning" ammonia solutions as I can find in a retail store. However, it's not pure ammonia (NH3, NH4). Instead, the ammonia is in the compound Ammonia Hydroxide, NH4OH. Now, this molecular formula tells us that each *molecule* of Ammonia Hydroxide contains 5 hydrogen atoms, one nitrogen and one oxygen atom for a total of 7 atoms in the molecule. Now, we haven't really answered your question yet. We only know that we have 5 hydrogen atoms of in each molecule of ammonia hydroxide, and we have a 10% solution of ammonia hydroxide presumably in 100% pure water, H2O. To know how many hydrogen atoms are in a given amount of cleaning solution, we need to know how much these molecules weigh (i.e, their mass) and then do a bit of math to arrive at the number of hydrogen atoms. To do this, we need two very important tools: a periodic table of the elements to get each atoms atomic weight, and Avogadro's number. Avagadro's number (6.022 x 10^23, that's 10 to the 23rd power) is the unit of measure that defines how many atoms of stuff (any element) are in a *mole*, or "mol". What's a mole? It's a unit of measure. It's like a dozen of something. A dozen eggs is 12 eggs. A dozen donuts is 12 donuts is 12 donuts. Likewise, a mole of something is 6.022x10^23 of something. Why do we need these two measures? Because, scientists have measured and recorded the weight of each of the elements on the periodic table using these units of measure. If you look at a periodic table, Hydrogen, element number 1, has an atomic weight of 1.00794. That means 6.022 x 10^23 atoms of hydrogen, collected together and put on a scale weighs 1.00794 grams, on average (isotopes of an element can weight more or less). With this information, we can convert grams of cleaning solution into grams of ammonia hydroxide, and furthermore moles or numbers of atoms of each element, thereby answering your question. We do it this way because we don't buy ammonia cleaner at the store by how many moles of solution there are. We buy it by the ounce or milliliter. First, we need figure out the molecular weights of the two compounds in our solution: 1. ammonia hydroxide (NH40H), 2. water (H2O). For NH4OH, Here are the numbers of each atoms and their atomic weights added together: 1 x N (14.0067) = 14.0067 5 x H (1.00794) = 5.0397 1 x O (15.9994) = 15.9994 ------------------------- Total: 35.0458 grams / mole of NH40H or, written in terms of Avagadro's number, we can say the total weight is 35.0458 grams / 6.022x10^23 molecules of NH4oH. This is a conversion factor (fraction) that we'll use later to convert weights to molecules. For H2O, Here we do the same: 2 x H (1.00794) = 2.0159 1 x O (15.9994) = 15.9994 ------------------------- Total: 18.01528 grams/mole or, again, in terms of Avagadro's number, we say the total weight is 18.01528 grams / 6.022x10^23 molecules of H2O. Now, lets figure out hydrogen atoms in 100 milliliters (ml) of cleaning solution that's 10% ammonia by weight(see note below). We know that 1 ml of pure water weights 1 gram We do the math, using our conversion factors to get the number of hydrogen atoms present. Both the ammonia hydroxide and the water contain hydrogen atoms. We'll calculate them separately, then add them together for the total. First, the NH4OH atoms. Remember, each *molecule* has *5* hydrogen atoms: 100grams cleaner x (10% NH40H/grams cleaner) x (6.022x10^23 molecules NH40H / 35.0458 grams) x (5 atoms Hydrogen/molecule NH40H) = 8.5916 x 10^23 Hydrogen atoms in the ammonia hydroxide. Next, the H2O atoms. Each *molecule* of H2O has *2* hydrogen atoms: 100grams cleaner x (90% H2O/grams cleaner) x (6.022x10^23 molecules H2O / 18.01528 grams) x (2 atoms hydrogen/molecule H2O) = 60.1689 x 10^23 Hydrogen atoms in the water. If you add these numbers together, the total hydrogen atoms in both the ammonia hydroxide and the water are: ..8.5916 x 10^23 Hydrogen atoms in NH4OH +60.1689 x 10^23 Hydrogen atoms in H2O ---------------- 68.7605 x 10^23 Hydrogen atoms in 100 grams of cleaning solution from Ace hardware. Obviously, the majority of hydrogen atoms in the solution are in the water, as is expected. If someone cares to check to check my work, I didn't really spend a lot of time double checking my numbers. Hopefully, I got them right. And, there you have your answer. Note: While the percentage of ammonia hydroxide is most likely by *volume*, I'll calculate it as it were by *weight* or mass. Otherwise, I'd have to throw in some density conversions to get weights by volumes, which would just add to the calculations. We'll keep things simple to demonstrate the process of getting the answer. Also, we used the rough approximation that 1 ml of solution weighs 1 gram. While this works with water at standard temperature at sea level, ammonia is different. However, only 10% of our solution is ammonia,so an approximation is good enough to demonstrate how we do the calculations.