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3 years ago

2 SO3 (g) + Heat <-----> 2 SO2 (g) + O2 (g)

Chemistry

1 answer:

Step2247 [10]3 years ago

7 0

Answer:

The concentration of SO₂ will decreases

Explanation:

As you can see in the reaction

2 moles of gas ⇆ 3 moles of gas

Based on Le Châtelier's principle, a change doing in a system will produce that the system reacts in order to counteract the change made.

If the pressure is increased, the system will shift to the left in order to produce less moles of gas and decrease, thus, the pressure.

As the system shift to the left, the concentration of SO₂ will decreases

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You placed 43.1 g of an unknown metal at 100 °C into a coffee cup calorimeter that contained 50.0 g of water that was initially

nika2105 [10]

Answer :

(a) The heat released by the metal is -312.48 J

(b) The specific heat of the metal is $0.0944J/g^oC$

Explanation :

For part A :

Heat released by the metal = Heat absorbed by the calorimeter + Heat absorbed by the water

$q=[q_1+q_2]$

$q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]$

where,

q = heat released by the metal

$q_1$ = heat absorbed by the calorimeter

$q_2$ = heat absorbed by the water

$c_1$ = specific heat of calorimeter = $51.5J/^oC$

$c_2$ = specific heat of water = $4.184J/g^oC$

$m_2$ = mass of water = 50.0 g

$\Delta T$ = change in temperature = $(T_{final}-T_{initial})=23.2-22.0=1.2^oC$

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

$q=[(51.5J/^oC\times 1.2^oC)+(50.0g\times 4.184J/g^oC\times 1.2^oC)]$

$q=312.48J$

Thus, the heat released by the metal is -312.48 J

For part B :

$q=m\times c\times \Delta T$

q = heat released by the metal = -312.48 J

m = mass of metal = 43.1 g

c = specific heat of metal = ?

$\Delta T$ = change in temperature = $(T_{final}-T_{initial})=23.2-100=76.8^oC$

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

$-312.48J=43.1g\times c\times 76.8^oC$

$c=0.0944J/g^oC$

Thus, the specific heat of the metal is $0.0944J/g^oC$

8 0

4 years ago

What is the mass of 3.2 moles of Sulfur?

FinnZ [79.3K]

Answer:

820.864 g

Explanation:

1) The atomic mass of sulfur (found from the periodic table) is 32.065 amu. Use this mass to find the molar mass of Sulfur. Sulfur is S8 so the molar mass of sulfur is:

8 × 32.065 = 256.52 g/mol

2) To find the mass use the formula:

m = n × M where m is the mass, n is the number of moles, and M is the molar mass.

$m \: = 3.2 \times 256.52$

$m = 820.864 \: g$

8 0

3 years ago

2 C6H14 + 19 O2 --> 12 CO2 + 14 H2O

vivado [14]

Answer:

1.27 moles (3 s.f.)

Explanation:

Mole ratio of water: C6H14

= 14:2

= 7:1

This means that to produce 7 moles of water, 1 mole of C6H14 is needed. Or 1/7 mole of C6H14 is needed to produce 1 mole of water. So if you need 8.86 moles of water, 8.86(1/7) moles of C6H14 is needed.

For 8.86mol of water, moles of C6H14 needed

= 8.86/7

= 1.27 moles (3 s.f.)

4 0

4 years ago

Which type of reaction is represented by this graph?

enot [183]

Answer:

D. Exothermic.

Explanation:

Hello there!

In this case, since the potential energy versus reaction progress diagrams are related to the energetic profile of a chemical reaction, we can set the initial point at the beginning of the reaction as the energy of the reactants and the final point as the energy of the products.

Next, since the change in the enthalpy of a reaction is quantified by subtracting products minus reactants, we can see that the products have less energy than the reactants and therefore ΔH for this reaction is negative, which matches with the definition of D. Exothermic reaction.

Regards!

7 0

3 years ago

Read 2 more answers

A sample of unknown gas in a closed container has a temperature of 37oC and a pressure of 2 atm. What will be the pressure if th

vodomira [7]

Answer:

hdfcghbjhaiedg

Explanation:

6 0

3 years ago