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IgorC [24]
3 years ago
14

1. The actual yield of a product in a reaction was measured as 1.20 g. If the theoretical yield of the product for the reaction

is 1.82 g, what is the percentage yield of the product?
65.9%

67.2%

71.9%

73.3%

_______________

2. Which of the following statements best defines the percentage yield of a reaction? (5 points)


The ratio of measured yield over actual yield

The amount of product measured after a reaction

The amount of measured yield over calculated yield

The maximum amount of product that can be obtained

________________________

3. A chemist reacted 17.25 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.


Na + Cl2 → NaCl


If the percentage yield of the reaction is 88%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.
__________________
4. Two gas jars are connected to each other, but they are separated by a closed valve. One gas jar contains oxygen, and the other contains hydrogen. What will happen when the valve is opened?

Oxygen and hydrogen molecules will mix because of random movement of their molecules.

Oxygen and hydrogen molecules will remain in separate jars because of different partial pressures.

Oxygen and hydrogen molecules will remain in separate jars because of different rates of expansion.

Oxygen and hydrogen molecules will mix because the molecules have a much lower volume than the volume of the jars.
Chemistry
1 answer:
n200080 [17]3 years ago
5 0
<h3>1. <u>Answer;</u></h3>

Percentage yield = 65.9%

<h3><u>Explanation;</u></h3>
  • Percentage yield of a reaction is obtained by dividing the actual yield by theoretical yield and multiplying by 100 percent.

Therefore;

  • Percentage yield = Actual yield/theoretical yield × 100%

                                      = (1.20 g/1.82 g) × 100%

                                      =  65.9%

<h3 /><h3>2. <u>Answer;</u></h3>

The amount of measured yield over calculated yield

<h3>Explanation;</h3>
  • Percentage yield of a reaction is obtained by dividing the actual yield by theoretical yield and multiplying by 100 percent.
  • The actual yield is the actual amount produced when the experiment or reaction is carried out.
  • Theoretical yield is the calculated or expected amount of the product. It is based on the limiting reactant.

<h3>3. <u>Answer</u>;</h3>

= 37.71 g

<h3><u>Explanation;</u></h3>

The balanced equation is:

2 Na + Cl₂ → 2 NaCl.

From the balanced equation:

2.0 moles of Na reacts with 1.0 mole of chlorine gas to give 2.0 moles of NaCl.

  • The number of moles of Na = mass/atomic mass),

                                                    n = (17.25 g / 22.989 g/mole of Na)

                                                         = 0.75 moles

Thus;

  • Using cross multiplication and from the equation:

                         2.0 moles of Na → 2.0 moles of NaCl

                         0.75 moles  of Na → 0.75 moles of NaCl

Therefore;

  • The mass of the produced NaCl (m = n x molar mass)

                    m = (0.75 mole x 58.443 g/mole of NaCl)

                         = 43.85 g.

  • This is the yield if the percentage of yield is 100%, but the percentage yield of the reaction is 86%.

Hence;

The actual yield = (43.85 g) (86/100)

                            = 37.71 g.

<h3>4. <u>Answer;</u></h3>

Oxygen and hydrogen molecules will mix because of random movement of their molecules.

<h3><u>Explanation;</u></h3>
  • Both gasses will diffuse into the other jar until the molecules are well distributed into both containers.
  • Diffusion is the movement of molecules from a point of high concentration to areas of low concentration until equilibrium is attained.  
  • The mixture of gases will have a partial pressure that is equal to the sum of the partial pressures of the component gases.
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Determine what is missing from this neutralization reaction: AgNO3+KCl→AgCl+−−−−
lapo4ka [179]

Answer:

The answer to your question is: KNO₃

Explanation:

                                AgNO3  +  KCl   →   AgCl  +   −−−−

A. KNO3    this option is correct because it is a double replacement reaction then potassium must attached to NO₃.

B. KOH  this product is not possible because there is no water to form OH⁻ ions.

C. Ag2K  this product is not possible because both Ag and K are metals, then it is difficult that they attach.

D. KN2O This product is imposible to form, this option is wrong.

7 0
3 years ago
Determine the [OH−] , Ph, and POH of a solution with a [H+] of 0. 00017 m at 25 °C.
tino4ka555 [31]

Main Answer:

Given

pH = -log[H+]

= -log[0.00017]

= 3.769

We know that

pW = pH + pOH

and pW =14

pOH = 14-pH

=14-3.769

=10.231

According to the definition

pOH = -log[OH-]

10.231 = log[OH-]-1

[OH-]= 5.87 x 10-11

Explanation:

What is pH?

pH is defined as the concentration of H+ ion in the solution. If the pH value is less than 7, then the solution will be acidic. If the pH value is greater than 7, then the solution will be basic.

To know more about pH, please visit:

brainly.com/question/8758541

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4 0
2 years ago
The mole is defined as the amount of a substance containing the same number of particles as exactly 12 g of C-12. The amu is def
Pavlova-9 [17]

Answer:

Because it wouldn't make any sense

Explanation:

First of all, I think it's important to highlight the definition of isotope.

Isotope (Wikipedia): Variants of a particular chemical element <u>which differ in neutron number</u>...

This means that two isotopes are the same element but have different net mass per atom, due to the different number of neutrons.

Therefore, it's important to make the definition on the same isotope so that the proportion is equal. If the definition would be made on different isotopes, the proportion wouldn't have any sense. Let me be clear with this example:

mass in grams of a C-12 atom = 1.9944235 × 10 ^ -23 g  --> this is the mass of a single C atom.

By definition --> 1 mol of anything = 6.02 x 10 ^ 23 particles of anything

Therefore, we know how much a single C atom weights. How many grams do you think that 6.02 x 10 ^ 23 atoms of C (i.e a mol of C) could weight??

1 single C atom ----------------------------- 1.9944235 × 10 ^ -23 g

6.02 x 10 ^ 23 atoms of C   ------------ <u>12.006 g  !!</u>

These 12 g is the same quantity than above! Therefore, 1 mol of C weights 12 g. If the definition were made with 13 g of C-13 (the other C isotope), these numbers will not be the same --> There would be a contradiction.

Regarding the second question, we need to search Ne-20 atomic mass in grams -->  3,3509177 × 10 ^ -23 g

Hence, if we follow the same rule, the amu would be 1/12 of Ne-20.

[ 3,3509177 × 10 ^ -23 g ] / 12 = 2.79 ^ -24 g

3 0
3 years ago
How many moles (of molecules or formula units) are in each sample?
Alexus [3.1K]

The number of moles in each sample will be 0.391 moles, 30.7 moles, 0.456 moles, and 1350 moles

<h3>What is the number of moles?</h3>

The number of moles of a substance is the ratio of the mass of the substance to the molar mass.

In other words; mole = mass/molar mass.

Thus:

  • moles of 18.0 g NO_2 = 18.0/46

                                   = 0.391 moles

  • moles of 1.35 kg CO_2 = 1350/44

                                         = 30.7 moles

  • moles of 46.1 g KNO_3 = 46.1/101.1

                                          = 0.456 moles

  • moles of 191.8 kg Na_2SO_4 = 191800/142

                                                 = 1350 moles

More on the number of moles of substances can be found here: brainly.com/question/1445383

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5 0
2 years ago
HELP ME THIS IS 1 MONTH OVER DUE PLS HURRY
AVprozaik [17]
1false
2false
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4 0
2 years ago
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