Tag: interpreting a balanced chemical reaction

Questions Related to interpreting a balanced chemical reaction

$4Co+3{ O } _{ 2 }\rightarrow 2C{ o } _{ 2 }{ O } _{ 3 }$
$66.8\ g$ of Cobalt reacted with oxygen and $70.50\ g$ of $C{ o } _{ 2 }{ O } _{ 3 }$ was collected after the reaction was completed. Calculate the percent yield. (At. mass of $Co=59\ g/mol$)

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $75$%

  2. $80$%

  3. $85$%

  4. $90$%

Show answer
Correct Option: A
Explanation:

$ 4Co \space + \space 3O _2 \rightarrow 2Co _2O _3$

$4\space moles$ of cobalt produce $2\space moles$ of $Co _2O _3$

$\Rightarrow 2\space mole$  $Co \rightarrow$  $1 \space mole \space Co _2O _3$ 

$\Rightarrow 2\times 59 \rightarrow (2\times 59 + 3\times 16)$

$\Rightarrow 118\space g \space Co \rightarrow 166\space g \space Co _2O _3$

$\Rightarrow 66.8\space g \space \rightarrow (x)$

$\Rightarrow x = \dfrac{166 \times 66.8}{118} = 93.97\space g$

$\%$ Yield $= \dfrac{70.50}{93.97}\times 100 \approx 75\%$


A reaction produced $30.0$ grams of carbon dioxide. If the theoretical (expected) yield was $45$ grams, what is the percentage yield?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $15$%

  2. $30$%

  3. $67$%

  4. $150$%

Show answer
Correct Option: C
Explanation:

Percentage yield of a compound is the ratio of actual yield to the excepted yield of the compound.

$\%$ Yield = $ \dfrac{\text{Actual Yield}}{\text{Expected Yield}} \times 100 = \dfrac{30}{45} \times 100 = \dfrac{2}{3}\times 100 = 67\%$

When the fertilizer plant completes its small batch process, they find that they have only collected $26\ mL$ of $NH _{3}$ which was supposed to be $100\ mL$. They are disappointed with this result due to the low yield. What is the % yield of their process?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $26$%

  2. $38$%

  3. $52$%

  4. $76$%

Show answer
Correct Option: A
Explanation:

$26$ ml of $NH _3$ yeild into 100 ml 

$=26/100$ 
= $26%$

A reaction is known to have a percent yield of $80$%. It the actual yield is $25$ grams, what was the expected yield?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $3.2\ grams$

  2. $19\ grams$

  3. $31.25\ grams$

  4. $190\ grams$

Show answer
Correct Option: C
Explanation:

Percent yield is the ratio of actual yield to the expected yield of compound.

$\%$ Yield $= \dfrac{\text{Actual Yield}}{\text{Expected Yield}} \times 100$
$\Rightarrow 80 = \dfrac{25}{\text{Expected Yield}} \times 100$
$\Rightarrow$ Expected Yield $= \dfrac{25}{80} \times 100 = \dfrac{250}{8} = 31.259\space g$

A bacterium can convert xylose to lactic acid with a percent yield of $85$%. What mass of lactic acid would be produced from $50.0\ g$ sample of xylose by this bacterium? (At. mass of xylose$(C _5H _{10}O _5) =150\ g/mol,$ At. of lactic acid$(C _3H _6O _3)=90\ g/mol$).

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $58.8\ g$

  2. $85\ g$

  3. $50\ g$

  4. $42.5\ g$

Show answer
Correct Option: D
Explanation:

Percent Yield is the ratio of actual yield of a substance to the theoretical yield.

Percent Yield $= \dfrac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100$
Given, Theoretical Yield $50\space g,$ Percent Yield $= 85$
So, $(\dfrac{85}{100} \times 50) =$ Actual Yield
$\Rightarrow$ Actual Yield $= 42.5 \space g$

A student conducts an experiment to produce a $Ca{CO} _{3}$ precipitate. The student collects $1.80\ g$ of product after predicting it should be possible to produce $2.00\ g$ of the product.
What is the student's percent yield for this experiment?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $-10$%

  2. $+90$%

  3. $+10$%

  4. $+111$%

Show answer
Correct Option: B
Explanation:

Percent Yield is the ratio of actual yield to the theoretical yield.

$\Rightarrow \% $ Yield $= \dfrac{E}{T} \times 100$
$\Rightarrow$ Here, $E = 1.8 \space g; \space T = 2\space g$
So, percent yield $= \dfrac{1.8}{2} \times 100 = 90\%$

If $100\ mL$ of the acid is neutralised by $100\ mL$ of $4\ M\ NaOH$, the purity of concentrated $HCl$ (sp. gravity $= 1.2)$ is:

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $12$%

  2. $98$%

  3. $73$%

  4. $43$%

Show answer
Correct Option: A
Explanation:

No of equivalent of acid $=$ No of equivalent of base.

$100 \times m _1=100 \times4$
$m _1=4m$
$4$mole of $HCL$ in $1$liter of water..........$(1)$
$\frac{{\rho HCl}}{{\rho {H _2}O}} = k$
density of $HCl=1200gm/l$...........$(2)$
purity of $HCl\Rightarrow 1200gm\,\,in\,1liter$
purity of $HCl$ in gram in $1$ liter $\Rightarrow 1200gm$
purity of $HCl \Rightarrow$ $\frac{{4 \times 36.5}}{{1200}} \times 100 \Rightarrow  \sim 12\% $
hence, purity of $HCl$ is $ \sim 12\% $
so option $A$ is correct.

$50\ g$ of a sample of $NaOH$ required for complete neutralisation of $1\ litre\ N\ HCl$. What is the percentage purity of $NaOH$?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. $80$

  2. $70$

  3. $60$

  4. $50$

Show answer
Correct Option: A
Explanation:

for complete neutralisation we have

moles of acid = moles of base
moles of acid = normality $$ volume = $1 *1$
moles of base = 1 =$\dfrac{given mass}{molecular mass}$

so, given mass = moles $$ molecular mass = 1$*$ = 40

percentage purity = $\dfrac{40 }{50} * 100$ = 80 %

In a reaction vessel,100 g $H _2$ and 100 g $Cl _2$ are inbred and suitable conditions are provided for take following reaction: 

$H _2 ( g)+ Cl _2(g)\rightarrow 2HCl(g)$


The amount of $HCI$ formed (at 90% yield) will be:

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. 36.8 g

  2. 62.5 g

  3. 80 g

  4. 91.98 g

Show answer
Correct Option: D
Explanation:

100 g of $H _2$ = 50 mole

100 g of $Cl _2$ = 1.4 mole
According to the reaction 1 mole of $H _2$ is reacting with 1  mole of $Cl _2$
So, $Cl _2$ is th limiting reagent 
So, moles of $HCl$ formed = 2 $\times$ 1.4 mole
 
Amount of $HCl$ = 2.8 $\times$ 36.5 = 102.2 g

Since, the reaction is giving 90 % yield
therefore , amount of $HCl$ formed = $102.2 \times \dfrac{90}{100}$

Amount of HCl formed = 91.98 g

Hence, the correct option is $(D)$.

In the Haber process:
$N _2(g) + 3H _2(g) \rightarrow 2NH _3(g) $
$30 L$ of $H _2$ and $30 L$ of ${N _2}{^-}$ were taken for reaction which yielded only $50\%$ of expected product. What will be the composition of the gaseous mixture in the end?

chemistry introduction to analytical chemistry interpreting a balanced chemical reaction percentage yield stoichiometric calculations

  1. 20 L $NH _3$, 25 L $N _2$ and 20 L $H _2$

  2. 10 L $NH _3$, 25 L $N _2$ and 15 L $H _2$

  3. 20 L $NH _3$, 10 L $N _2$ and 30 L $H _2$

  4. 20 L $NH _3$, 25 L $N _2$ and 15 L $H _2$

Show answer
Correct Option: A