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MAXImum [283]
3 years ago
8

If one wants 100g of Ag, how much ag2o is needed?

Chemistry
1 answer:
KonstantinChe [14]3 years ago
3 0

Mass Ag₂O needed = 107.416 g

<h3>Further explanation</h3>

Given

100 g Ag

Required

mass of Ag2O

Solution

Proust stated the Comparative Law that compounds are formed from elements with the same Mass Comparison so that the compound has a fixed composition of elements

mass of Ag in Ag2O :

= ((2 x Ar Ag)/molar mass Ag2O )x mass Ag2O

\tt mass~Ag=\dfrac{2.Ar~Ag}{MW~Ag_2O}\times mass~Ag_2O

Ar Ag : 107,8682 g/mol

MW Ag₂O = 231,735 g/mol

Input the value :

mass Ag₂O=(mass Ag x MW Ag₂O) : (2 x Ar Ag)

mass Ag₂O = (100 g x 231,735 g/mol) : ( 2 x 107,8682 g/mol)

mass Ag₂O = 107.416 g

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Given the balanced equation representing a reaction:
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Consider the nuclear equation below. Superscript 235 subscript 92 upper U right arrow superscript 4 subscript 2 upper H e. What
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Answer:

\rm_{90}^{231}\text{Th}

Explanation:

The unbalanced nuclear equation is

\rm _{92}^{235}\text{U} \longrightarrow \,  _{2}^{4}\text{He} + X

Let's write X as a nuclear symbol.

\rm _{92}^{235}\text{U} \longrightarrow \,  _{2}^{4}\text{He} + _{Z}^{A}\text{X}

The main point to remember in balancing nuclear equations is that the sums of the superscripts and of the subscripts must be the same on each side of the reaction arrow.

Then

235 = 4 + A , so A = 235 - 4 = 231, and

 92 = 2 + Z , so  Z =   92 - 2 =  90

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\rm _{92}^{235}\text{U} \longrightarrow \,  _{2}^{4}\text{He} +\, _{90}^{231}\text{X}

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if a leaf falls from a tree we assume that it is in free fall and not affected by air resistance, how many force vectors does th
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Write the net ionic equation for the reaction that occurs when equal volumes of 0.546 M aqueous acetylsalicylic acid (aspirin) a
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Answer:

C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to figure out the required net ionic equation by firstly writing out the complete molecular equation between aspirin and sodium acetate:

C_9H_8O_4+NaC_2H_3O_2\rightarrow C_2H_4O_2+NaC_9H_7O_4

Whereas acetic acid and sodium acetylsalicylate are formed. Now, we write the complete ionic equation whereby sodium acetate and sodium acetylsalicylate are ionized because they are salts yet neither aspirin nor acetic acid are ionized as they are weak acids:

C_9H_8O_4+Na^++C_2H_3O_2^-\rightarrow C_2H_4O_2+Na^++C_9H_7O_4^-

Finally, for the net ionic equation we cancel out the sodium spectator ions to obtain:

C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-

Regards!

7 0
3 years ago
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