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MariettaO [177]
2 years ago
7

The burning of magnesium is a highly exothermic reaction. How many kilojoules of heat are released when 0. 75 mol of Mg burn in

an excess of O2?
2Mg(s) + O2(g) → 2MgO(s) + 1204 kJ
Chemistry
1 answer:
alexandr402 [8]2 years ago
4 0

Taking into account the definition of enthalpy of a chemical reaction, the quantity of heat released when 0.75 moles of Mg are burned is 451.5 kJ.

<h3>Enthalpy of a chemical reaction</h3>

The enthalpy of a chemical reaction is known as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.

The enthalpy is an extensive property, that is, it depends on the amount of matter present.

<h3>Heat released in this case</h3>

In this case, the balanced reaction is:

2 Mg(s) + O₂ (g) → 2 MgO(s) + 1204 kJ

This equation indicates that when 2 moles of Mg reacts with 1 mole of O₂, 1204 kJ of heat is released.

When 0.75 moles of Mg are burned, then you can apply the following rule of three: if 2 moles of Mg releases 1204 kJ of heat, 0.75 moles of Mg releases how much heat?

heat=\frac{0.75 moles of Mgx1204 kJ}{2 moles of Mg}

<u><em>heat= 451.5 kJ</em></u>

Finally, the quantity of heat released when 0.75 moles of Mg are burned is 451.5 kJ.

Learn more about enthalpy of a chemical reaction:

<u>brainly.com/question/15355361</u>

<u>brainly.com/question/16982510</u>

<u>brainly.com/question/13813185</u>

<u>brainly.com/question/19521752</u>

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245 g water sample initially at at 32 oC absorbs 17 kcal of heat. What is the final temperature of water?
steposvetlana [31]

Answer:62.66°C or 235.66K

Explanation:Q=McpT, the energy was given in calories so you first convert to Joules by multiplying the value in calories by 4.184J.

17*4.184=71.128kJ.

71.128kJ=mcpT

71.128kJ=245*4.187*(T-Tm)

Tm is the final temperature of the mixture. The T is the temperature given which should be converted to Kelvin by adding 273...T=32+273=305K.

71128J=245*4.187*(305-Tm)

71128=312873.575-1025.815Tm

1025.815Tm=312873.575-71128

1025.815Tm=241745.58

Tm=241745.58/1025.815

Tm=235.66K

4 0
3 years ago
A serving of Cheez-Its releases 1.30 x 10^4 kcal (1 kcal = 4.18 kJ) when digested by your body. If this same amount of energy we
kondor19780726 [428]

Answer:

The final temperature is:- 7428571463.57 °C

Explanation:

The expression for the calculation of heat is shown below as:-

Q=m\times C\times \Delta T

Where,  

Q  is the heat absorbed/released

m is the mass

C is the specific heat capacity

\Delta T  is the temperature change

Thus, given that:-

Mass of water = 1.75 mg = 0.00175 g ( 1 g = 0.001 mg)

Specific heat of water = 4.18 J/g°C

Initial temperature = 35 °C

Final temperature = x °C

\Delta T=(x-35)\ ^0C/tex]&#10;Q = [tex]1.3\times 10^4 kcal

Also, 1 kcal = 4.18 kJ = 4.18\times 10^3 J

So, Q = 1.3\times 10^4\times 4.18\times 10^3 J = 54340000 J

So,  

54340000=0.00175\times 4.18\times (x-35)

0.00175\times \:4.18\left(x-35\right)=54340000

x-35=\frac{54340000}{0.007315}

x=7428571463.57

Thus, the final temperature is:- 7428571463.57 °C

3 0
2 years ago
We gave an object with a density of 620 g/cm^3 and a volume of 75cm^3. What is the mass of this object?
Hitman42 [59]
d=\frac{m}{V} \ \ \ \Rightarrow \ \ m=dV\\\\&#10;d=620\frac{g}{cm^{3}}\\&#10;V=75cm^{3}\\\\\&#10;m=620\frac{g}{cm^{3}}*75cm^{3}=46500g
6 0
3 years ago
How many atoms are in 578g Na
borishaifa [10]

1.51 x 10²⁵atoms

Explanation:

Given parameters:

Mass of Na = 578g

Unknown:

Number of atoms = ?

Solution:

 To find the number of atoms, we must first find the number of moles the given mass contains.

  Number of moles  = \frac{mass}{molar mass}

   molar mass of Na = 23g

 Number of moles =  \frac{578}{23} =  25.13moles

   1 mole of a substance = 6.02 x 10²³atoms

    25.13 mole of Na = 25.13 x  6.02 x 10²³atoms

 This gives  1.51 x 10²⁵atoms of Na

Learn more:

Avogadro's constant brainly.com/question/2746374

#learnwithBrainly

5 0
3 years ago
Describe how replacing one light on a holiday string of bulbs with a "blinking" light would cause all the lights in the string t
stiks02 [169]

Answer: Chemical Reaction

Explanation:

6 0
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