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3 years ago

How many electrons does a single hydrogen gain or lose in the following reaction? H 2 + O 2 → H 2 O

Chemistry

2 answers:

True [87]3 years ago

4 0

Answer:

Lose 1

Explanation:

Answer via Educere/ Founder's Education

wariber [46]3 years ago

3 0

Answer:

option B. Lose 1.

Explanation:

To determine the number of electrons that a single hydrogen gains or loses you need to realize that the chemical reaction is an oxidation-reduction (redox) reaction and state the changes in the oxidation states.

The substance that gains electrons is being reduced, reducing its oxidation number, and the substance that lose electrons is being oxidized, increasing its oxidation state.

1) State the oxidation state of hydrogen atoms in the rectant side:

H₂: the oxidation state of any element in its atomic or molecular form is zero. That is indicated as a superscript to the right of the chemical symbol: H₂⁰

2) State the oxidation state of the hydrogen atoms in the product side:

H₂O: the rule says that the oxidation state of oxygen, when combined with other elements, except in the case of peroxides, is -2.

Hence, in order to the molecule H₂O be neutral, the total charge contributed by the two atoms of hydrogen must be + 2: +2 - 2 = 0.

Since there are two hydrogen atoms, each contributes +2 / 2 = +1 charge.

3) Conclusion:

Every atom of hydrogen changes from a 0 oxidation number to a +1 oxidation number, which, in turn, means that every hydrogen atom loses one electron.

Thus, the answer is, the option B. Lose 1.

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How many atoms in 1kg of platinum a 2.5x10^24 b 3.1x10^24

Nutka1998 [239]

Answer:

3.1x10^24 it will be in 1 kg of platinum

6 0

3 years ago

How much energy will it take to raise the temperature of 75.0 g of water from 20.0°C to 55.0°C?

Hatshy [7]

Answer:

We can use heat = mcΔT to determine the amount of heat, but first we need to determine ΔT. Because the final temperature of the water is 55°C and the initial temperature is 20.0°C, ΔT is as follows:

ΔT = Tfinal − Tinitial = 55.0°C − 20.0°C = 35.0°C

given the specific heat of water as 1 cal/g·°C. Substitute the known values into heat = mcΔT and solve for amount of heat:

= heat=(75.0 g)(1 cal/ g· °C )(35.0°C) =

= 75x1x35=2625 cal

6 0

3 years ago

The enthalpy of solution (dissolving) of sodium hydroxide is given below. Determine the change in temperature of a coffee cup ca

geniusboy [140]

Answer:

The change in temperature of a coffee cup calorimeter is 8.87°C.

Explanation:

Volume of the water = V = 150 g

Density of the water , d =1.0 g/mL

Mass of the water = M

$M=d\times V=1.00 g/mL\times 150 ml =150.0 g$

Mass of solution = m = M = 150.0 g

$NaOH(s)\rightarrow NaOH(aq),\Delta H =-44.51 kJ/mol$

Moles of NaOH = $\frac{5.00 g}{40 g/mol}=0.125 mol$

Energy released when 0.125 moles of NaOH added in water = Q

$Q=0.125 moles\times (-44.51 kJ/mol)=-5.5638 kJ=-5,563.8 J$

1 kJ = 1000 J

Heat gained by water = Q' = -Q ( conservation of energy)

$Q'= 5,563.8 J$

Specific heat of solution = c = 4.184 J/g°C

Change in temperature of the solution = $\Delta T$

$Q'=mc\times \Delta T$

$5,563.8 J=150.0 g\times 4.184 J/g^oC\times \Delta T$

$\Delta T=\frac{5,563.8 J}{150.0 g\times 4.184 J/g^oC}=8.87^oC$

The change in temperature of a coffee cup calorimeter is 8.87°C.

7 0

3 years ago

Consider the reaction:

murzikaleks [220]

Answer: The formation of given amount of oxygen gas results in the absorption of 713 kJ of heat.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of oxygen gas = 83 g

Molar mass of oxygen gas = 32 g/mol

Putting values in above equation, we get:

$\text{Moles of oxygen gas}=\frac{83g}{32g/mol}=2.594mol$

For the given chemical equation:

$2Fe_2O_3\rightarrow 4Fe+3O_2;\Delta H^o_{rxn}=+824.2kJ$

Sign convention of heat:

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

By Stoichiometry of the reaction:

When 3 moles of oxygen gas is formed, the amount of heat absorbed is 824.2 kJ

So, when 2.594 moles of oxygen gas is formed, the amount of heat absorbed will be = $\frac{824.2kJ}{3mol}\times 2.59mol=713kJ$

Hence, the formation of given amount of oxygen gas results in the absorption of 713 kJ of heat.

7 0

3 years ago

What is a hot spot? Must be in your own words ( please hurry)

kenny6666 [7]

Answer:

It depends. what hot spot are you looking for?

7 0

3 years ago

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