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MrRissso [65]
3 years ago
8

A reaction takes place that results in an amount of 585 grams of product that is recovered. The theoretical amount calculates to

be 650 grams. What is the percent yield?
Chemistry
1 answer:
lisov135 [29]3 years ago
7 0

Answer:

90%

Explanation:

Data obtained from the question include:

Actual yield = 585g

Theoretical yield = 650g

%yield =?

%yield = Actual yield /Theoretical yield x100

% yield = 585/650 x 100

% yield = 90%

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Explanation:

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The given reaction equation is not balanced because:

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In a balanced chemical equation number of atoms of each elements are equal on both sides.

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7 0
3 years ago
How do I find the moles of OH- which reacted (mol) in the titration. Table Attached
BaLLatris [955]

Answer:

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3 years ago
The density of a gas cannot be measured.<br> True<br> False
likoan [24]

Answer:

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Explanation:

7 0
3 years ago
58. A cylinder of a gas mixture used for calibration of blood gas analyzers in medical laboratories contains 5.0% CO2, 12.0% O2,
erica [24]

<em><u>Answer and Explanation:</u></em>

Greetings!

Let's~answer~your~question!

Partial ~pressure ~of ~gas ~can ~be ~directly~ calculated ~by ~multiplying ~the~ percentage\\ of~ pressure~ of~ gases~ to ~the ~total ~pressure.

\boxed{Pgas~ = ~P~total~ * \% ~P ~of ~gas}

<em><u>For % of N2 gas: </u></em>

<em><u /></em>100\% - (5\% + 12\%) = 83\% ~N2<em><u /></em>

<em><u /></em>

<em><u /></em>PN_2 ~= ~146~ atm~ *~ 0.83 ~ = 121.18 ~atm<em><u /></em>

<em><u /></em>PO_2 ~= ~146~ atm~ *~ 0.12~ = 17.52 ~atm<em><u /></em>

<em><u /></em>~PCO_2~ = ~146~ atm ~* 0.05 = 7.3 ~atm<em><u /></em>

3 0
3 years ago
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