4. 2CH3OH + 302 --> 2002 + 4H20

When 6.40 g of CH3OH were mixed with 10.2 g of O2, 6.12 g of CO2 were made.

a. Calculate the theoretical yield of CO2-

b. Determine the percent yield of CO2.

See explanation

Explanation:

The balanced reaction equation is;

2CH3OH + 302 --> 2C02 + 4H20

Number of moles of of methanol = 6.40g/32.04 g/mol= 0.1998 moles

2 moles of methanol yields 2 moles of CO2

0.1998 moles of methanol also yields 0.1998 moles of CO2

Number of moles of oxygen = 10.2g/32g/mol = 0.3188 moles

3 moles of oxygen yields 2 moles of CO2

0.3188 moles of oxygen yields 0.3188 × 2/3= 0.2125 moles of CO2

Hence, methanol is the limiting reactant

Mass of CO2 produced = 0.1998 moles of CO2 × 44g/mol = 8.79g

Theoretical yield = 8.79g

%yield = actual yield/theoretical yield × 100

% yield = 6.12/8.79 × 100

%yield = 69.6%

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

no statements shown

the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl