# Consider this balanced equation 3H2+CO -> CH4+H2O. how many moles of CH4 can be obtained by reached 2.0mol of H2 with 2.0molCO according to this equation?

<<Consider this balanced equation
3H2 + CO -> CH4+H2O.
How many moles of CH4 can be obtained by reacting 2.0 mol of H2 with 2.0 mol CO according to this equation?>>
You need three times as many moles of H2, as CO. Since there are equal moles of H2 and CO available, you will run out of H2 after consuming 2.0 moles of it, which will consume 2/3 mole of CO and make 2/3 mole of CH4.

## According to the balanced equation, the molar ratio between H2 and CH4 is 3:1. This means that for every 3 moles of H2, 1 mole of CH4 is produced.

Since you have 2.0 moles of H2, you can use the ratio to calculate the moles of CH4 produced:

2.0 moles H2 x (1 mole CH4 / 3 moles H2) = 0.67 moles CH4

Therefore, you can obtain 0.67 moles of CH4 by reacting 2.0 moles of H2 with 2.0 moles of CO according to this equation.

## To determine the number of moles of CH4 that can be obtained from 2.0 moles of H2 and 2.0 moles of CO, you can use the balanced equation as a conversion factor.

According to the balanced equation:
3H2 + CO -> CH4 + H2O

We can see that the ratio between H2 and CH4 is 3:1. This means that for every 3 moles of H2, we can obtain 1 mole of CH4.

Since we have 2.0 moles of H2, we can calculate the moles of CH4 using the following proportion:

2.0 mol H2 / 3 mol H2 = x mol CH4 / 1 mol CH4

Cross-multiplying the equation, we have:

2.0 mol H2 * 1 mol CH4 = 3 mol H2 * x mol CH4

Simplifying, we get:

2.0 mol CH4 = 3 mol H2 * x mol CH4

Dividing both sides of the equation by 3 mol H2, we get:

(2.0 mol CH4) / (3 mol H2) = (3 mol H2 * x mol CH4) / (3 mol H2)

Simplifying further, we have:

0.66667 mol CH4 = x mol CH4

Therefore, based on the balanced equation, you can obtain approximately 0.66667 moles of CH4 by reacting 2.0 moles of H2 with 2.0 moles of CO.