Given:

cac2 + n2 → cacn2 + c

in this chemical reaction, how many grams of n2 must be consumed to produce 265 grams of cacn2? express your answer to three significant figures.

the reaction requires how many grams of n2?

92.6 g.

Explanation:

CaC₂ + N₂ → CaCN₂ + C.

n = mass / molar mass = (265.0 g) / (80.102 g/mol) = 3.308 mol.

∵ 1.0 mole of N₂ produces → 1.0 mole of CaCN₂.

∴ 3.308 mole of N₂ produces → 3.308 mole of CaCN₂.

∴ The grams of N₂ = n x molar mass = (3.308 mole)(28.0 g/mol) = 92.63 g = 92.6 g.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.