Hydrogen and oxygen react to produce water, according to the reaction

2 H2 (g) + O2 (g) → 2 H2O (l).

If 3 moles of hydrogen react with 2 moles of oxygen and the yield in the reaction is 80%, how many moles of water are obtained?

3 mol

Explanation:

Given data:

Moles of hydrogen = 3 mol

Moles of oxygen = 2 mol

Yield of reaction = 80%

Moles of water produced = ?

Solution:

Chemical equation:

2H₂ + O₂  →  2H₂O

Now we will compare the moles of water with both reactants.

                       H₂           :         H₂O

                        2            :            2

                          3          :             3

                          O₂        :           H₂O

                           1          :              2

                           2          :         2×2 =   4

Hydrogen produced less number of moles of water so it will limiting reactant.

So number of moles of water produced are = 3 mol

Let x = cost of one t-shirt

Let y = cost of one sweatshirt

Jayden: 9x + 3y = $420

Carson: x + 6y = $296. Multiply Jayden's equation by -2

Jayden: -18x - 6y = $-840

Carson: x + 6y = $296. Add the equations together to eliminate variable y.

New equation: -17x = $-544. Divide each side by -17.

x = $32. Plug this value into one of the original equations.

32 + 6y = $296. Subtract 32 from each side.

6y = 264. Divide each side by 6.

y = 44.

Plug both your x and y value into one of the equations to ensure they're correct.

9(32) + 3(44) = 420

420 = 420.

x = 32

y = 44.