In an experiment, 8.50 g of methane, ch4, reacted with 15.9 g of oxygen gas, as shown in the following equation: ch4(g) + 2 o2(g) co2(g) + 2 h2o(g) determine the percent yield if 9.77 g of carbon dioxide was obtained

Percentage Yield  = 89.39 %

Explanation:

First thing's first, we have to write down the balanced chemical equation;

CH4(g) + 2 O2(g) --> CO2(g) + 2 H2O(g)

It is crucial we identify the limiting reactant before proceeding. The limiting reactant tells us which reactant is the reaction dependent on and how much of the product can be obtained. We calculate it using the following steps;

1. Calculate the number of moles of each reactant present

Methane - Number of moles = mass / molar mass = 8.50 / 16 =  0.53125 mol

Oxygen - Number of moles = mass / molar mass = 15.9 / 32 =  0.4969 mol

2. Divide the actual number of moles of each reactant by its stoichiometric coefficient in the balanced chemical equation:

Methane - 0.53125 / 1 = 0.53125

Oxygen - 0.4969 / 2 = 0.24845

3. The reactant with the smallest mole ratio is limiting. The limiting reactant is oxygen.

Since the product we are interested in is the Carbon dioxide, From the equation, we have;

2 mol of O2 reacts to produce 1 mol of CO2.

Expressing in terms of mass; Mass = Number of moles * Molar mass

64g ( 2 * 32) = 44g ( 1* 44)

15.9 g = x

Upon solving for x;

x = (15.9 * 44) / 64

x = 10.93

Theoretical Yield = 10.93g

Practical Yield = 9.77g

Percentage Yield = (Practical Yield / Theoretical Yield) * 100

Percentage Yield = ( 9.77 / 10.93 ) * 100

Percentage Yield = 89.39%

r just means there's a number of carbon in teh chain. for example rcooh means that after x number of carbon, the chain ends with cooh.

explanation:

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.