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Helen [10]
3 years ago
8

22. A flask containing 450 mL of 0.50 M H2SO4 was accidentally knocked to the floor. How many grams of NaHCO, do you need to put

on the spill to neutralize the acid according to the following equation: H2SO4(aq)+2 NaHCOs(aq) Na,SO(aq) +2 H20()+2 CO2(g) D) 38 g A) 2.3 g B) 9.5 g C) 19 g
Chemistry
1 answer:
Dvinal [7]3 years ago
7 0

<u>Answer:</u> The correct answer is Option D.

<u>Explanation:</u>

To calculate the moles of a solute, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}\text{Volume of solution (in L)}}

We are given:

Volume of sulfuric acid = 450mL = 0.45 L      (Conversion factor: 1 L = 1000 mL)

Molarity of the solution = 0.5 moles/ L

Putting values in above equation, we get:

0.5mol/L=\frac{\text{Moles of sulfuric acid}}{0.45L}\\\\\text{Moles of sulfuric acid}=0.225mol

For the given chemical reaction:

H_2SO_4(aq.)+2NaHCO_3(aq.)\rightarrow Na_2SO_4(aq.)+2H_2O(l)+2CO_2(g)

By Stoichiometry of the reaction:

1 mole of sulfuric acid reacts with 2 moles of sodium bicarbonate.

So, 0.225 moles of sulfuric acid will react with = \frac{2}{1}\times 0.225=0.45mol of sodium bicarbonate

To calculate the mass of sodium bicarbonate, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of sodium bicarbonate = 0.45 moles

Molar mass of sodium bicarbonate = 84.007 g/mol

Putting values in above equation, we get:

0.45mol=\frac{\text{Mass of sodium bicarbonate}}{84.007g/mol}\\\\\text{Mass of sodium bicarbonate}=38g

Hence, the correct answer is Option D.

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Answer:

Explanation:

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To identify the limiting reactant ...

- write and balance the reaction of interest. Express it in standard form. That is, standard form of a reaction is when the coefficients of the balanced equation are in their lowest whole number values. Also, remember that the standard equation is 'assumed' to be at STP conditions (0°C & 1atm).

- convert all given reactant values to moles

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Your Problem:

Given:        3Ba  +  N₂  => Ba₃N₂

               22.6g    4.2g        ?

moles Ba => 22.6g/137.34g/mol = 0.165 mole Ba

moles N₂ =>    4.2g/14.007g/mol= 0.150 mole N₂

Part A: Determining the Limited Reactant

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Barium => 0.165/3 = 0.055  <=> (Limiting Reactant)

Nitrogen => 0.15/1 = 0.15

  • Barium is the smaller result and is therefore the limiting reactant. This works for ALL limiting reactant type problems. However, be sure to use the mole values calculated first (Ba = 0.165mol & N₂ = 0.150mol) when doing ratio calculations.

Part B: Max (theoretical) amount of Ba₃N₂ produced:

<em>Note: The product yield amounts are based upon the given 'moles' of limiting reactant, NOT the results of the 'divide by respective coefficient' step used to ID the limiting reactant.     </em>

                   3Ba        +          N₂         =>     Ba₃N₂    (3:1 rxn ratio for Ba:Ba₃N₂)

moles      0.165mole        0.150mole         1/3(0.165)mole = 0.055mole Ba₃N₂

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Part C: Excess N₂ remaining after reaction stops:

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moles of N₂ used = 1/3(0.165)mole = 0.055mole N₂ used  

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mass N₂ remaining = 0.095mole x 28g/mole = 2.66 grams N₂ remaining in excess.

                   

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<span> </span>

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