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finlep [7]
4 years ago
14

galium has a weighted average atomic mass of 69.7 and two naturally occurring isotopes: Gallium-69 and Gallium-71. Gallium-69 ha

s a relative abundance of 60.1% and a mass of 68.9. The relative abundance of gallium-71 is 39.9%. Based on the information, what is the mass of gallium-71?
Chemistry
1 answer:
dimulka [17.4K]4 years ago
6 0
Figure it out yet????
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Tall plants are dominant to short plant?
Hunter-Best [27]

Answer:

TT gives you a tall plant

Tt gives you a tall plant cause the dominant  trait over powers the non dominant trait

tt gives you a short plant because it has two rescesive traits

Explanation:

4 0
4 years ago
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Need it fast!! Given the balanced equation below, calculate the moles of aluminum that are needed to react completely with 13.2
satela [25.4K]
By looking closely into the given balanced chemical reaction, it can be deduced that the number of moles needed for every mole of FeO is only 2/3. Calculating for the number of moles of aluminum,

                      x = (13.2 moles FeO)(2 mols Al/3 moles FeO)
 
                       x = 8.8 moles Al

Answer: 8.8 moles Al
4 0
3 years ago
1.11 grams divided by 16.04 grams = how many moles?
Sever21 [200]
1.14912614 x 10^-25 moles would be your answer
4 0
4 years ago
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What is the concentration of ammonia in a solution if 23.4 mL of a 0.117 M solution of HCl are needed to titrate a 100.0 mL samp
Georgia [21]

Answer: 0.0274 M

Explanation:-

The balanced chemical solution is:

NH_4OH(aq)+HCl(aq)\rightarrow NH_4Cl(aq)+H_2O(l)

According to the neutralization law,

n_1M_1V_1=n_2M_2V_2

where,

M_1 = molarity of HCl solution = 0.117 M

V_1 = volume of HCl solution = 23.4 ml

M_2 = molarity of NH_4OH solution = ?

V_2 = volume of NH_4OH solution = 100.0 ml

n_1 = valency of HCl = 1

n_2 = valency of NH_4OH = 1

1\times 0.117M\times 23.4=1\times M_2\times 100.0

M_2=0.0274

Therefore, the concentration of ammonia in a solution will be 0.0274 M

8 0
3 years ago
What are the consequences of poor nutrition.
Anton [14]

Explanation:

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3 0
3 years ago
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