Butane, C4H10, is the gas burned in disposable lighters. How many moles of oxygen are needed to burn 5.0 mol of butane in a lighter to produce carbon dioxide and water?

Unbalanced equation:

C4H10 + O2 -> CO2 + H2O

28 mol

32 mol

13 mol

32 mol

Explanation:

Step 1: Write the balanced equation.

C₄H₁₀ + 6.5 O₂ → 4 CO₂ + 5 H₂O

Step 2: Establish the appropriate molar ratio.

The molar ratio of C₄H₁₀ to O₂ is 1:6.5

Step 3: Calculate the moles of oxygen needed to burn 5.0 mol of butane.

We use the molar ratio established in the previous step.

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation:

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.