consider the equation for the following questions

2C2H6(g) + 7o2(g) 4 CO2(g) +6H2O(g)

How many grams of CO2 are produced when 2.00moles of C2H6 react with sufficient oxygen?

Just follow the steps from this example.

http://www.jiskha.com/science/chemistry/stoichiometry.html

To find the number of grams of CO2 produced when 2.00 moles of C2H6 react with sufficient oxygen, you need to use the balanced equation and the molar mass of CO2.

The balanced equation given is:
2C2H6(g) + 7O2(g) -> 4CO2(g) + 6H2O(g)

From the equation, you can see that 2 moles of C2H6 produce 4 moles of CO2. This means that the mole ratio between C2H6 and CO2 is 2:4, or simply 1:2.

Given that you have 2.00 moles of C2H6, you can convert this to moles of CO2 using the mole ratio. Since the ratio is 1:2, you multiply the number of moles of C2H6 by 2 to get the moles of CO2.

2.00 moles C2H6 x 2 moles CO2 / 1 mole C2H6 = 4.00 moles CO2

Now that you have the number of moles of CO2 produced, you can calculate the mass of CO2 using its molar mass. The molar mass of CO2 is approximately 44.01 g/mol.

4.00 moles CO2 x 44.01 g/mol = 176.04 grams CO2

Therefore, when 2.00 moles of C2H6 react with sufficient oxygen, 176.04 grams of CO2 are produced.