Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product: First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02×10236.02×1023 particles per mole) to convert number of particles to moles. Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2+O2→2H2O2H2+O2→2H2Othe coefficients tell us that 2 molmol of H2H2 reacts with 1 molmol of O2O2 to produce 2 molmol of H2OH2O. Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2H2, reacts with nitrogen gas, N2N2, to form ammonia gas, NH3NH3, according to the equation 3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. Part A How many moles of NH3NH3 can be produced from 16.5 mol of H2 and excess N2? Express your answer numerically in moles.
Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product: First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02×10236.02×1023 particles per mole) to convert number of particles to moles. Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2+O2→2H2O2H2+O2→2H2Othe coefficients tell us that 2 molmol of H2H2 reacts with 1 molmol of O2O2 to produce 2 molmol of H2OH2O. Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2H2, reacts with nitrogen gas, N2N2, to form ammonia gas, NH3NH3, according to the equation 3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. Part A How many moles of NH3NH3 can be produced from 16.5 mol of H2 and excess N2? Express your answer numerically in moles.
Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product: First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02×10236.02×1023 particles per mole) to convert number of particles to moles. Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2+O2→2H2O2H2+O2→2H2Othe coefficients tell us that 2 molmol of H2H2 reacts with 1 molmol of O2O2 to produce 2 molmol of H2OH2O. Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2H2, reacts with nitrogen gas, N2N2, to form ammonia gas, NH3NH3, according to the equation 3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. Part A How many moles of NH3NH3 can be produced from 16.5 mol of H2 and excess N2? Express your answer numerically in moles.
To convert from a given quantity of one reactant or product to the quantity of another reactant or product:
First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02×10236.02×1023 particles per mole) to convert number of particles to moles.
Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2+O2→2H2O2H2+O2→2H2Othe coefficients tell us that 2 molmol of H2H2 reacts with 1 molmol of O2O2 to produce 2 molmol of H2OH2O.
Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles.
Reaction of hydrogen and nitrogen to form ammonia
Hydrogen gas, H2H2, reacts with nitrogen gas, N2N2, to form ammonia gas, NH3NH3, according to the equation
3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g)
NOTE: Throughout this tutorial use molar masses expressed to five significant figures.
Part A
How many moles of NH3NH3 can be produced from 16.5 mol of H2 and excess N2?
Express your answer numerically in moles.
Definition Definition Number of atoms/molecules present in one mole of any substance. Avogadro's number is a constant. Its value is 6.02214076 × 10 23 per mole.
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