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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 = !!!
What else can I help you with?
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 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.
What is mass of N2 required to occupy 3.0 L at 100C and 700 mmHg?
To find the mass of N2, first calculate the moles of N2 using the ideal gas law: PV = nRT. Then use the molar mass of N2 to convert moles to grams. Given that the volume is 3.0 L, the temperature is 100°C (373 K), and the pressure is 700 mmHg (93.3 kPa), you can substitute these values into the ideal gas law to find the moles of N2.
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
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.
How many grams are in 2.25 moles of N2?
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
How many grams of NH3 can be produced from 2.79 moles of N2?
The mass of ammonia will be 95,03 g.
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 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 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 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.
What is mass of N2 required to occupy 3.0 L at 100C and 700 mmHg?
To find the mass of N2, first calculate the moles of N2 using the ideal gas law: PV = nRT. Then use the molar mass of N2 to convert moles to grams. Given that the volume is 3.0 L, the temperature is 100°C (373 K), and the pressure is 700 mmHg (93.3 kPa), you can substitute these values into the ideal gas law to find the moles of N2.
How many moles of N2 are in 50g of it?
To determine the number of moles of N2 in 50g, you first need to find the molar mass of N2 (28.02 g/mol). Then, you divide the given mass (50g) by the molar mass to get the number of moles. In this case, 50g / 28.02 g/mol ≈ 1.79 moles of N2.
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 2.08 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
If the total mass of N2 in the atmosphere is 3.87e21 grams or 2.901 moles based on the denitrification rate of 310e12 grams year what is the residence time of N2 in the atmosphere?
Residence time = 3.87E21/310E12 = 1.25E7 years
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
