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soldier1979 [14.2K]
2 years ago
14

Between reaction of magnesium powder and lead oxide which is oxidized in the reaction and which is oxidizing agent

Chemistry
1 answer:
GuDViN [60]2 years ago
7 0

Answer:

Mg is oxidized and Pb is the oxidizing agent

Explanation:

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A scientist performs an experiment in which they create an artificial cell with a selectively permeable membrane through which o
lozanna [386]

Answer:

Water moves into the cell

Explanation:

As shown in the question above, the cell is high in glucose and placed in a glass filled with water. This cell has a semi permeable membrane that allows only water to pass through, as the concentration of water within the cell is low, the cell will attempt to strike a balance with the medium it is inserted into. For this reason, what is likely to happen is the passage of water from the most concentrated to the least concentrated medium, that is, the water will pass from the cup to the cell.

water moves into the cell through osmosis.during osmosis water moves from a region of low concentration of solute to a region of high concentration of solute.the glucose introduced into the cell makes it more concentrated.

In this case the cell is hypertonic and water would enter into the cell through the semi permeable membrane.this membrane allows water to pass through but not glucose.this movement of water into the cell causes the cell to become turgid.

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2 years ago
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Ammonia can be prepared by the reaction of magnesium nitride with water. The products are ammonia and magnesium hydroxide. Write
deff fn [24]

Answer:

Mg3N2 +6H2O--> 2NH3 + 3Mg (OH)2

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2 years ago
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Manganese dioxide (MnO2(s), Hf = –520.0 kJ) reacts with aluminum to form aluminum oxide (AI2O3(s), Hf = –1699.8 kJ/mol) and mang
Temka [501]

Answer : The enthalpy of the reaction = -1839.6 KJ

Solution : Given,

\Delta (H_{f})_{MnO_{2}} = -520.0 KJ/mole

\Delta (H_{f})_{Al_{2}O_{3}} = -1699.8 KJ/mole

The balanced chemical reaction is,

3MnO_{2}(s)+4Al(s)\rightarrow 2Al_{2}O_{3}(s)+3Mn(s)

Formula used :

\Delta (H_{f})_{reaction}=\sum n(\Delta H_{f})_{product}-\sum n(\Delta H_{f})_{reactant}

\Delta (H_{f})_{reaction}=(2\times \Delta H_{Al_{2}O_{3}(s)}+3\times \Delta H_{Mn(s)} )-(3\times \Delta H_{MnO_{2}(s) }+4\times\Delta H_{Al}(s))

We know that the standard enthalpy of formation of the element is equal to Zero.

Therefore, the enthalpy of formation of (Mn) and (Al) is equal to zero.

Now, put all the values in above formula, we get

\Delta (H_{f})_{reaction}=[2moles\times (-1699.8 KJ/mole)}+3moles\times (0\text{ KJ/mole}})]-[(3moles\times(-520.0KJ/mole }+4moles\times(0\text{ KJ/mole})]

                        = (-3399.6) + (1560)

                        = -1839.6 KJ



5 0
3 years ago
A student submits the following work on the mass number, but he has made a few mistakes. Select the sentences that are incorrect
rewona [7]

Answer

 

Calculating the mass number for an atom requires that we know the atomic number and the number of protons in the atom’s nucleus. The mass number then gives us the average weight of atoms of a given element. However, as long as the number of protons equals the number of neutrons, the values balance out and we always obtain a whole number for the mass number.

Explanation:

those 3

7 0
3 years ago
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