What mass of carbon dioxide can be produced from 3.60 g butane and 2.30 g of oxygen in the unbalanced reaction c4h10 + o2 -> co2 + h2o?

Mass = 2.64 g

Explanation:

Given data;

Mass of butane = 3.60 g

Mass of oxygen = 2.30 g

Mass of carbon dioxide produced = ?

Solution:

Chemical equation:

O₂ + C₄H₁₀  →  CO₂ + H₂O

Number of moles of BUTANE:

Number of moles = mass/ molar mass

Number of moles = 3.60 g / 58.12 g/mol

Number of moles = 0.06 mol

Number of moles of oxygen:

Number of moles = mass/ molar mass

Number of moles = 2.30 g / 32 g/mol

Number of moles = 0.07 mol

Now we compare the moles ammonia with hydrogen and nitrogen

                              O₂                :             CO₂

                               1                  :               1

                               0.07            :              0.07 mol                                 

                                C₄H₁₀         :              CO₂

                                  1              :                1

                                 0.06            :            0.06 mol

The number of moles of carbondioxide produced by butane are less so it will limiting reactant.

Theoretical yield:

Mass = number of moles × molar mass

Mass =0.06 mol × 44 g/mol

Mass = 2.64 g

explanation:

crosscutting concepts have application across all domains of science. as such, they are a way of linking the different domains of science. they include patterns; cause and effect; scale, proportion, and quantity; systems and system models; energy and matter; structure and function; and stability and change.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890