2.00−g sample of a metal x (that is known to form x2+ ions) was added to 0.100 l of 0.500 m h2so4. after all the metal had reacted, the remaining acid required 0.0637 l of 0.500 m naoh solution for neutralization. calculate the molar mass of the metal and identify the elemen

the molar mass is 40 and the metal is Calcium

Explanation:

X + H2SO4=X2SO4 + H2

The mole ratio is 1:1

no of mole of H2SO4= conc(M) × Vol(L)

=0.1×0.5

=0.05 mol

from the balanced chemical equation of the reaction

no of mole of 'X' = no of mole of H2SO4

thus no of mole of X=0.05 mol

Also, no of mole=mass/molar mass

molar mass of 'X'=mol/mass

=2/0.05

=40

hey your not cool]      

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.