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DedPeter [7]
3 years ago
13

A 13.00 g sample of citric acid reacts with an excess of baking soda as shown in the equation. What is the theoretical yield of

carbon dioxide?
Chemistry
2 answers:
Mariulka [41]3 years ago
6 0
The answer on the quiz would be (d) 8.93 g 
julia-pushkina [17]3 years ago
3 0
Chemical equation of the reaction between citric acid and baking soda:

C_{6}  H_{8}  O_{7} +3NaHCO_{3} -\ \textgreater \  Na_{3} C_{6} H_{5} O_{7} +3 H_{2} O+3CO_{2}

Ratios

Citric Acid        Baking soda    ->  Sodium Citrate  Water    Carbon Dioxide
C6H8O7                                                                                CO2
1 mole                                                                                     3moles

Molecular masses
Citric acid
6*12 + 8*1 + 7*16 = 192 g/mole
Carbon dioxide
12 + 2*16 =   44 g/mole

Proportion carbon dioxide / citric acid

3 * 44 g of carbon dioxide / 192 g of citric acid

132 g of carbon dioxide / 192 g of citric acid

13.00 g of citric acid * [132 g of carbon dioxide / 192 g of citric acid] =  8.94 g of carbon dioxide.

Answer: 8.94 grams.
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7 0
3 years ago
How many milliliters of a 3.0 M HCL solution are required to make 250.0 milliliters of 1.2 M HCL
tiny-mole [99]
You can use M x V = M' x V'

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3 years ago
The free energy change for the following reaction at 25 °C, when [Cr3+] = 1.32×10-3 M and [Fe3+] = 1.14 M, is 131 kJ: Cr3+(1.32×
larisa [96]

Answer:

E°cell = - 1.3575 V

This reaction is spontaneous in the reverse direction

Explanation:

The given cell reaction:

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

The given Gibbs free energy: ΔG = 131 kJ = 131 × 10³ J     (∵ 1 kJ = 10³ J)

As we know,

ΔG = - n F E°cell

Here, n - the number of moles of electrons transferred = 1

F - Faraday constant = 96500

E°cell - cell potential = ?

\therefore E^{\circ }_{cell} = -\frac{\Delta G}{n \: F} = -\frac{131\times 10^{3}\, J}{1\, mol\times96500 \, C.mol^{-1}}

\Rightarrow E^{\circ }_{cell} = -1.3575\, V

<u>For a given chemical reaction if-</u>

1. ΔG = negative and E°cell = positive

⇒ <em>The reaction is spontaneous and proceeds spontaneously in the forward direction.</em>

2.  ΔG = positive and E°cell = negative

⇒ <em>The reaction is non-spontaneous and proceeds spontaneously in the reverse direction.</em>

<u>Since, for this chemical reaction: </u>

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

ΔG = + 131 × 10³ J ⇒ positive

and, E°cell = - 1.3575 V ⇒ negative

<u>Therefore, this reaction is spontaneous in the reverse direction.</u>

6 0
3 years ago
An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark wit
Anon25 [30]

<u>Answer:</u> The molar mass of unknown triprotic acid is 97.66 g/mol

<u>Explanation:</u>

To calculate the molarity of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of triprotic acid

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is NaOH.

We are given:

n_1=3\\M_1=?M\\V_1=250mL\\n_2=1\\M_2=0.0600M\\V_2=95.9mL

Putting values in above equation, we get:

3\times M_1\times 250=1\times 0.0600\times 95.9\\\\M_1=0.0077M

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Molarity of solution = 0.0077 M

Given mass of triprotic acid = 0.188 g

Volume of solution = 250 mL

Putting values in above equation, we get:

0.0077M=\frac{0.188\times 1000}{\text{Molar mass of triprotic acid}\times 250}\\\\\text{Molar mass of triprotic acid}=97.66g/mol

Hence, the molar mass of unknown triprotic acid is 97.66 g/mol

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