When 22.8 g of carbon were burned in the presence of 78. 9 g of oxygen 18.1 g of oxygen remained unreacted what mass of carbon dioxide was produced

Explanation:

We are given the masses of two reactants and asked to determine the mass of the product.

This looks like a limiting reactant problem.

1. Assemble the information

We will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.  

MM:           12.01        32.00   44.01

                    C      +      O₂ ⟶ CO₂  

Mass/g:     22.8          78.9  

2. Calculate the initial moles of C

We know that there is excess oxygen, so C is the limiting reactant.

3. Calculate the moles of CO₂ formed

4. Calculate the mass of CO₂

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.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer