4 pts Question 5
Directions:
Solve the following problem on a separate sheet of paper.
Submit a photo (or scan) to receive credit. File type must be .pdf.
Problem:
Consider the balanced reaction: 4Ga(s) + 302(g) → 2Ga2O3(s)
When gallium metal reacts with 13.0 g of oxygen gas how many grams of gallium oxide will be
produced?
Upload
Choose a File

First we need to find the number of moles that 43.9g of gallium metal is. We can do this by finding the molar weight of gallium and cross-multiplying to cancel out units:

So we are dealing with 0.63 moles of gallium metal.

We can take from the balanced equation that 4 moles of gallium metal will react completely with 3 moles of oxygen gas. We can take this ratio and make a proportion to find the amount of oxygen gas, in moles, that will react completely with 0.63 moles of gallium metal:

Cross multiply and solve for x:

4x=1.89

x=47 molesO₂

So now we know that 0.47 moles of oxygen gas will react with 43.9g of gallium metal.

imma come back to you hold on

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.