I’ll you : )
what is the mass of co2 produced when 100. g of butane, c4h10, is burned with excess oxygen,
according to the following chemical equation? (molar mass of c4h10 is 58.12 g/mol, molar mass of
co2 is 44.01 g/mol)
2 c4h10 (g) + 13 o2 (g) → 8 co2 (g) + 10 h20 (l)

The answer to your question is: 303g of CO2

Explanation:

Data

mass CO2 = ?

mass C4H10 = 100 g

MW C4H10 = 58.12 g

MW CO2 = 44.01 g

Solve this problem using rules of three

Reaction

                    2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H20 (l)

                    2(58.12)       8(44.01)

                    100g              x

mass of CO2 produced = x = (100)(8)(44.01) / (2)(58.12)

                                          x = 35208 / 116.24

                                          x = 302.9 g ≈ 303 g of CO2

C₂H₆ + 2Cl₂ => C₂H₄Cl₂ + 2HCl

Or from left to right:

1, 2, 1, 2

Explanation:

To balance an equation, start by counting the number of atoms of each element on both sides.

C₂H₆ + Cl₂ => C₂H₄Cl₂ + HCl

C  2                 C  2

H  6                 H  5

Cl  2                Cl  3

We should increase the number of hydrogen atoms (H) on the right (products).

C₂H₆ + Cl₂ => C₂H₄Cl₂ + 2HCl

C  2                 C  2

H  6                 H  6

Cl  2                Cl  4

Increase the number of chlorine atoms (Cl) on the left (reactants).

C₂H₆ + 2Cl₂ => C₂H₄Cl₂ + 2HCl

C  2                  C  2

H  6                  H  6

Cl  4                 Cl  4

The equation is now balanced because there are the same number of atoms on each side.

C₂H₆ + 2Cl₂ => C₂H₄Cl₂ + 2HCl

or, if your drop down menus need you to write "1".

1C₂H₆ + 2Cl₂ => 1C₂H₄Cl₂ + 2HCl

The correct format is not to write the "1".