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3 years ago

The addition of an electron and a hydrogen atom to nad to form nadh is an example of what type of chemical reaction

1 answer:

4 0

The addition of an electron on to the element of hydrogen and ultimately to the electron carrier is an example of reduction. The molecule is becoming reduced or has electrons, and or hydrogen to help facilitate the addition of the electrons on it.

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Two objects are brought into contact Object 1 has mass 0.76 kg, specific heat capacity 0.87) g'c and initial temperature 52.2 'C

taurus [48]

Answer:

$T_F=77.4\°C$

Explanation:

Hello there!

In this case, according to the given information, it turns out possible to set up the following energy equation for both objects 1 and 2:

$Q_1=-Q_2$

In terms of mass, specific heat and temperature change is:

$m_1C_1(T_F-T_1)=-m_2C_2(T_F-T_2)$

Now, solve for the final temperature, as follows:

$T_F=\frac{m_1C_1T_1+m_2C_2T_2}{m_1C_1+m_2C_2}$

Then, plug in the masses, specific heat and temperatures to obtain:

$T_F=\frac{760g*0.87\frac{J}{g\°C} *52.2\°C+70.7g*3.071\frac{J}{g\°C}*154\°C}{760g*0.87\frac{J}{g\°C} +70.7g*3.071\frac{J}{g\°C}} \\\\T_F=77.4\°C$

Yet, the values do not seem to have been given correctly in the problem, so it'll be convenient for you to recheck them.

Regards!

4 0

3 years ago

considering what you now know about boyle’s law, make a prediction based on the following situation. what would happen to the pr

Tju [1.3M]

Answer:

The pressure would increase because the volume of space the gas takes up decreases once the bottle is squeezed. There is less room for the gas particles to move around meaning more collisions between the particles occur.

Explanation:

5 0

3 years ago

Draw a structural formula of an alkene or alkenes (if more than one) that undergo acid-catalyzed hydration and without rearrange

lara31 [8.8K]

Answer:

-) 2-methylbut-2-ene

-) 2-methylbut-1-ene

-) 3-methylbut-1-ene

Explanation:

in this case, the hydration of alkenes is a marknovnikov reaction, this means that the "OH" group would be added in the most substituted carbon of the double bond. (Figure 1)

For 2-methylbut-2-ene the most substituted carbon is the tertiary carbon (the carbon in the right of the double bond), so we will obtain the desired molecule. In 2-methylbut-1-ene the most substituted carbon is again the tertiary carbon (the carbon in the bottom of the double bond), so we will obtain 2-methyl-2-butanol. Finally, for 3-methylbut-1-ene the carbocation would be formed on carbon 3, this is a secondary carbocation. We can obtain a most stable carbocation if we do a hydride shift (Figure 2). With this new molecule is possible to obtain 3-methylbut-1-ene.

6 0

4 years ago

An example of an atom that has no charge is one that has

VikaD [51]

For an atom to have no charge, that is neutral, the number of electrons should be the same to the number of electrons. If the number of electron is more than the number of proton, the atom is negatively charged. Also, when the number of proton is more than the number of electron, the atom is positively charged. The answer to this item is letter C.

7 0

3 years ago

Read 2 more answers

Gaseous methane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . If of carbon dioxide is pro

yaroslaw [1]

The question is incomplete, the complete question is;

Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 28.2 g of carbon dioxide is produced from the reaction of 15.1 g of methane and 81.2 g of oxygen gas, Calculate the percent yield of carbon dioxide. Be sure your answer has the correct number of significant digits in it.

Answer:

71.1%

Explanation:

The balanced reaction equation must first be written;

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)

Let us obtain the number of moles of carbon dioxide corresponding to 28.2 g

Number of moles = mass/ molar mass= 28.2/44.01 g/mol = 0.64 moles of CO2

Next, we obtain the limiting reactant. This is the reactant that yields the least amount of product.

For methane;

Number of moles in 15.1 g= mass/molar mass= 15.1/16gmol-1 = 0.9 moles

From the reaction equation;

1 mole of methane yields 1 mole of carbon dioxide

Hence 0.9 moles of methane yields 0.9 moles of carbon dioxide.

For oxygen

Number of moles of oxygen corresponding to 81.2 g of oxygen= mass/ molar mass= 81.2g/32gmol-1 = 2.5 moles of oxygen

From the reaction equation;

2 moles of oxygen gas yields 1 mole of carbon dioxide

2.5 moles of oxygen gas yields 2.5 × 1 /2 = 1.25 moles of carbon dioxide.

Methane is the limiting reactant.

Theoretical yield of carbon dioxide= 0.9 moles

Actual yield of carbon dioxide= 0.64 moles

% yield = actual yield/ theoretical yield × 100

% yield= 0.64/0.9 ×100

% yield = 71.1%

3 0

3 years ago