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Fiesta28 [93]
3 years ago
14

15 grams of HCl should theoretically produce 0.42 grams of H2. The reaction actually produced 0.15 grams of H2. What is the perc

entage yield of H2?
Steps to solution please
Chemistry
1 answer:
Helen [10]3 years ago
8 0

Answer:

35.7%

Explanation:

The percent yield is calculated by the formula:

<em>[(actual yield) / (theoretical yield)] * 100</em>

In this case, the actual yield is 0.15 grams, and the theoretical yield is 0.42 grams. So, putting these values into the equation, we have:

\frac{0.15}{0.42} *100=0.357*100=35.7

Thus, the percent yield of H_2 is 35.7%.

Hope this helps!

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Answer:

The pH is 2, 60

Explanation:

The pH gives us an idea of the acidity or basicity of a solution. It is calculated as:

pH = -log (H +)= -log (2.5x10-3 )

<em>pH=2, 60</em>

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Based on the activity series of metal, which reaction with water will not happen?
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B

Explanation:

B, H2O + Na The elements toward the bottom left corner of the periodic table are the metals that are the most active in the sense of being the most reactive. Lithium, sodium, and potassium all react with water,

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A____is a prediction about the outcome of a test or experiment.
Annette [7]

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Explanation:

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When an electron falls from an excited state to ground state, is energy released or absorbed?
strojnjashka [21]

Answer:

Energy is released.

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3 years ago
A chemistry student weighs out of sulfurous acid , a diprotic acid, into a volumetric flask and dilutes to the mark with distill
nadezda [96]

The question is incomplete, here is the complete question:

A chemistry student weighs out 0.104 g of sulfurous acid, a diprotic acid, into a 250.0 mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0700 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.

<u>Answer:</u> The volume of NaOH needed is 36.2 mL

<u>Explanation:</u>

To calculate the molarity of solution, we use the equation:

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

Given mass of sulfurous acid = 0.104 g

Molar mass of sulfurous acid = 82 g/mol

Volume of solution = 250 mL

Putting values in above equation, we get:

\text{Molarity of sulfurous acid}=\frac{0.104\times 1000}{82\times 250}\\\\\text{Molarity of sulfurous acid}=5.07\times 10^{-3}M

To calculate the volume of base, 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 acid which is H_2SO_3

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=2\\M_1=5.07\times 10^{-3}M\\V_1=250mL\\n_2=1\\M_2=0.0700M\\V_2=?mL

Putting values in above equation, we get:

2\times 5.07\times 10^{-3}\times 250.0=1\times 0.0700\times V_2\\\\V_2=\frac{2\times 5.07\times 10^{-3}\times 250}{1\times 0.0700}=36.2mL

Hence, the volume of NaOH needed is 36.2 mL

5 0
2 years ago
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