How many grams of CO2 are produced from 51 g of CH4?

140.25g of CO2

Explanation:

First, let us write a balanced equation showing how CO2 is produced from CH4. This is illustrated below:

When CH4 undergoes combustion it produces CO2 and H2O according to the balanced equation below:

CH4 + 2O2 —> CO2 + 2H2O

Next, let us calculate the mass of the CH4 that reacted and the mass of CO2 produced from the balanced equation. This is shown below:

Molar Mass of CH4 = 12 + (4x1) = 12 + 4 = 16g/mol

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

From the balanced equation above,

16g of CH4 produced 44g of CO2.

Therefore, 51g of CH4 will produce = (51 x 44)/16 = 140.25g of CO2.

From the calculations made above, we can see that 51g of CH4 produced 140.25g of CO2

139.91 g CO2 to the nearest hundredth.

Explanation:

CH4 +  2O2 >  CO2 +  2H2O

Using the molar masses of the chemicals:

 (12.011 + 4*1.008) g CH4 produces  (12,011 + 32) g CO2

So 51 g of CH4 produces   [51 * (12,011 + 32] /  [ (12.011 + 4*1.008) ]

=  139.91 g CO2.

indium, and thallium have three electrons i think