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For this you need the atomic (molecular) mass of N2. Take the number of moles and multiply it by the Atomic Mass. Divide by one mole for units to cancel.
2.25 moles × 28.0 grams = 63.0 grams N2
What else can I help you with?
How many grams of H2 are needed to produce 13.14g of NH3?
To calculate the mass of H2 needed to produce 13.14g of NH3, you can use the molar ratio between H2 and NH3. From the balanced chemical equation for the reaction, you can see that 2 moles of NH3 are produced for every 3 moles of H2 consumed. First, calculate the number of moles of NH3 using its molar mass, then use the molar ratio to find the moles of H2 needed, and finally convert the moles of H2 into grams.
How many grams are in 3.26x10-1 mol NH3?
Assuming you are talking about production from the Haber process, and also assuming Hydrogen is not the limiting quantity and also assuming 100% conversion, then the answer is as follows: N2 + 3H2 ----> 2NH3 Then 1 mole of N2 produces 2 moles of ammonia. So 3.94 moles of N2 produces 7.92 moles of ammonia. Taking the molecular weight of ammonia to be 17 then 17 x 7.92 = 134.64 g of ammonia produced.
What is the formula for the sum of the series r(1/n2-1/n2)?
The formula for the sum of the series r(1/n2-1/n2) is r(1-1/n2).
How many ml is in 48 oz?
The only information you've given is you want to know moles and how many Liters there are. To calculate, you need to know what you are preparing(i.e., N2, AgNO3, etc.), and it's Molarity(M). Here's an example: How many moles of silver nitrate are needed to prepare 250mL of standard 0.100M silver nitrate solution? Note: M = moles of solute(stuff) / volume of solution(L) = # moles / L So, ?/250mL=.1M First we use dimensional analysis to convert mL to L. 250mL x 10-3 L / 1 mL = .25L Since we know M=moles/L, we can take the Molarity and put it in moles/L form. .10M = .10 mol/L Finally, .10 mol/L x .25L = .025 mol AgNO3 We can make a general assumption for your question and say the M is standard .100M. .10M = .10 mol/L .10 mol/L x 48L = 4.8 moles
What is the freezing point of a substance with a molecular weight of n2?
The freezing point of a substance with a molecular weight of N2 is -210.01 degrees Celsius.
How many moles of N are there in 0.189 grams of N20?
The answer is 0,0043 moles of N2.
How many grams of NH3 can be produced from 2.79 moles of N2?
The mass of ammonia will be 95,03 g.
How many grams of nitrogen are required to react with 2.79 g of hydrogen to produce ammonia?
In the reaction 3H2 + N2 --> 2NH3, the ratio of H2 to N2 is 3:1. To calculate the amount of N2 required, we need to first convert the mass of H2 to moles, then use the ratio to find the moles of N2 needed, and finally convert the moles of N2 to grams. After the calculation, we find that 2.79 g of H2 requires 3.31 g of N2 to react completely.
How many grams are in 0.713 moles of Ga?
For this you need the atomic (molecular) mass of N2. Take the number of moles and multiply it by the atomic mass. Divide by one mole for units to cancel..713 moles × (69.7 grams) = 49.7 grams Ga
How many moles of NH3 can be produced from 14 grams of N2?
The molecular mass of NH3 is the sum of the atomic mass of nitrogen and three times the atomic mass of hydrogen, or 14.007 + 3(1.008) = 17.031. Therefore, the number of moles of NH3 in 14.0 grams is 14.007/17.031 = 0.822. Since each molecule of N2 supplies two nitrogen atoms and each molecule of NH3 needs only one nitrogen atom, the number of moles of N2 needed is half the number of moles of NH3 formed = 0.411.
How many grams of NH3 can be produced from 2.08 grams of N2?
Ok, so I'm assuming that the chemical formula is written as - 3H2 + N2 ----> 2NH3 2.80 = moles of N2 17.03052 g/mol = Molar mass of NH3 (2.80 mol N2) x (2 NH3) / (1 N2) = 5.6 mol NH3 x (17.03052 g) / (1 mol NH3) = 95.4 g NH3
How many molecules of Nitrogen are in 3.5 grams of N2?
To find the number of molecules of N2 in 3.5 grams, first calculate the number of moles using the molar mass of N2 (28 g/mol). Then use Avogadro's number (6.022 x 10^23 molecules/mol) to convert the moles to molecules.
N2 plus 3H2 -- 2NH3 If you produce 55.5 grams of ammonia how many grams of nitrogen will you need?
You need the balanced chemical equation for N2 and H2 combining to form ammonia, NH3.N2 (g) + 3 H2 (g) -----> 2 NH3 (g)Moles NH3 = ( 55.5 g NH3 ) / ( 17.03 g/mol NH3 ) = 3.259 moles of NH3n N2 required = ( 3.259 mol NH3 ) ( 1 N2 mol / 2 NH3 mol ) = 1.629 moles N2m N2 required = ( 1.629 mol N2 ) ( 28.103 g N2 / mol N2 ) = 45.67 g N2 needed
What is the mass in grams of 2.4 moles of N2?
One look at a periodic table tells you the molar mass of sodium (Na) is 22.99 g/mol. So multiply your mol value by the g/mol value to get a value in grams! 2.0x10-3 x 22.99 = !!!
If 5.0 moles of NH3 are produce how many moles of N2 must have been used?
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
Find the mass in grams of 4.00x1023 molecules of N2?
1 mole N2 = 28.0134g 1 mole N2 = 6.022 x 1023 molecules N2 28.0134g N2 = 6.022 x 1023 molecules N2 (4.00 x 1023 molecules N2) x (28.0134g/6.022 x 1023 molecules) = 18.6g N2
How many moles of which reactant will remain if 1.39 moles of N and 3.44 moles of H will react to form ammonia find out how many grams of ammonia can be formed and how many moles of limiting reactant?
3,44 moles H2 react with 1,146 moles NH3. The limiting reactant is hydrogen. O,244 moles N2 remain. 19,5 g NH3 are obtained.
