## I'm sorry but the answer that you got was incorrect.

Let’s go through the steps together to help you understand.

Since the balanced equation is 2Na + 2H2O --> 2NaOH + H2, the ratio is going to be 2:2.

Na: H2O:

Na: 1x23 = 23 GFW H: (2x1 = 2) + O: (1x16 = 16) = 18 GFW

The number of grams for Na is 61.0g. To find the number of moles you are going to divide 61.0g by 23 GFW. This equals 2.65 moles.

The number of grams for H2O is 26.9g. To find the number of moles you are going to divide 26.9g by 18 GFW. This equals 1.49 moles.

Since the ratio that we have is a 2:2 ratio, we can divide both sides by 2 to make it a 1:1 ratio, Na to H2O.

Since you have a 1:1 ratio the number of moles of H2O and Na should be the same. Since you have 1.49 moles of H2O and 2.65 moles of Na, you do not have the sufficient amount of H2O makes it the limiting reagent.

**Question:**For the balanced equation 2Na + 2H2O --> 2NaOH + H2, if 61.0 grams of Na is reacted with 26.9 grams of H2O, and produce an 88.3% yield of H2, how many grams of H2 would be produced?**Step One:**Find the the limiting reagent.__Here are the steps to finding the limiting reagent__**Step One**: Based on the coefficients of the reactants (the two compounds) find the ratio.Since the balanced equation is 2Na + 2H2O --> 2NaOH + H2, the ratio is going to be 2:2.

**: Find the GFW of each compound (do not combine them).**

Step TwoStep Two

Na: H2O:

Na: 1x23 = 23 GFW H: (2x1 = 2) + O: (1x16 = 16) = 18 GFW

**Step Three:**Find the number of moles for each compound. You can do this by dividing the number of grams for one of the compounds by its GFW (do this for both compounds, separately).__Na:__The number of grams for Na is 61.0g. To find the number of moles you are going to divide 61.0g by 23 GFW. This equals 2.65 moles.

__H2O:__The number of grams for H2O is 26.9g. To find the number of moles you are going to divide 26.9g by 18 GFW. This equals 1.49 moles.

**Step Four:**Take the ratio and rewrite it so that it’s a one to something ratio (1:?). This is done by dividing both numbers in the ratio by the smaller number in the ratio.Since the ratio that we have is a 2:2 ratio, we can divide both sides by 2 to make it a 1:1 ratio, Na to H2O.

**Step Five:**Whichever compound is the “one part” of the ratio, multiply its number of moles by the other number in the ratio. If the product is greater than the number of moles in the second compound, the second compound is the limiting reagent. If the product is less than the number of moles in the second compound, the first compound is the limiting reagent.Since you have a 1:1 ratio the number of moles of H2O and Na should be the same. Since you have 1.49 moles of H2O and 2.65 moles of Na, you do not have the sufficient amount of H2O makes it the limiting reagent.

**Step Two:**Find the theoretical yield

__Here are the steps to finding the theoretical yield__**Step One:**Use the limiting reagent and see what the ratio is between that and the compound in the product (this is what you are trying to figure out). Make this ratio 1:? or ?:1

Since the limiting reagent is H2O and the balanced equation is 2Na + 2H2O --> 2NaOH + H2, the ratio between H2O and H2 is a 2:1 ratio.

**Step Two:**Using the ratio between the limiting reagent and the compound in the product, find the number of moles in the product's compound by multiplying/diving the limiting reagent by the non-one number in the ratio (1:

**?**).

For every 1.49 moles of H2O (^number of moles of H2O that we have^) we need half as many moles of H2, as shown in the ratio, therefore, we divide the number of moles of H2O by 2 to get 0.745 moles of H2.

**Step Three:**Once you know how many moles of the compound in the product you have, turn the moles back into grams. This allows you to answer the question of how much of ___ compound is able to be produced.

To turn the moles back into grams we used the equation grams=(moles)(GFW).

GFW of H2: (2x1)= 2 GFW grams=(0.745moles)(2GFW) ---> grams=1.49g

**Step Three:**Find the Actual Yield by plug in known information into equation shown below

Percentage Yield = (Actual Yield/Theoretical Yield) x 100%

88.3% = (Actual Yield/1.49grams) x 100%

Actual Yield = 1.316 grams

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