The reactants of two chemical equations are listed.

An ice freezer behind a restaurant has a freon leak, releasing 41.60 g of C2H2F3Cl into the air every week. If the leak is not f

zlopas [31]

Weeks = 6 x 4 = 24
Mass leak rate of freon = 41.60 g/week
Mass leak rate of fluorine
Fluorine mass in Freon
= —————————————- X leak rate
M.M. Of Freon

19 x 3
——— X 41.60 = 20.010 gm/week
118.5

Total leaked in 6 months

= 24 x 20.010 = 480.24 gm = 0.480 Kg

5 0

3 years ago

) The reaction below is exothermic: 2SO2 (g) O2 (g) 2SO3 (g) Le Cha^ telier's Principle predicts that __________ will result in

Lynna [10]

Answer:

A) increasing the pressure

Explanation:

Given the exothermic reaction:

2SO₂(g) + O₂(g) ↔ 2SO₃(g)

the question asks what will make the number of moles of SO₃(g) to increase.

When an equilibrium is disturbed, the system will shift in order to counteract the change (see Le Chatelier's Principle) So when the pressure is increased in a reaction involving gases, the equilibrium will shift trying to decrease the number of moles (because pressure is produced by molecules hitting the container), that is in this case it will shift towards the right side, towards the production of SO₃, thus increasing the number of moles of SO₃.

The number of moles in the right side is 2 and the number of moles in the left side is 3.

3 0

3 years ago

The second step to the scientific method is to state the "problem", the scientific question to be solved. What is one requiremen

Aleks [24]

The answer is B. In order to test something out you need to be able to solve it.

7 0

3 years ago

Read 2 more answers

An aqueous solution of a certain chemical is found to boil at 104.5 oC. At what temperature is this solution likely to freeze? T

xeze [42]

Answer:

16.4 °C

Explanation:

Boiling point elevation is the phenomenon in which the boiling point of a solvent will increase when another compound is added to it; meaning that athe resultant solution has a higher boiling point than its pure solvent.

Using the ebullioscopic constant,

ΔT = m * i * Kb

Where,

Δ T is the temperature difference between the boiling point of the solution, Temp.f and boiling point of the pure solvent, Temp.i

Kb is the ebulliscope factor of water = 0.510 °C.kg/mol

i is the van hoffs number = 1

m is the molality in mol/kg.

Calculating the molality of the solution,

Temp.i = 100°C

Temp.f = 104.5 °C

= 4.5/(1*0.510)

= 8.8235 mol/kg

Freezing point depression is defined as the decrease in the freezing point of a solvent on the addition of a solute.

Using the same equation, but kf = 1.86 °C.kg/mol

ΔT = m * i * Kf

Temp.i = freezing point of water = 0°C

Temp.f = (8.8235*1.86) - 0

= 16.412 °C

Freezing point of the solution = 16.4 °C

3 0

3 years ago

Consider the following reaction where Kc = 1.80×10-2 at 698 K:

Klio2033 [76]

Answer:

The system is not in equilibrium and the reaction must run in the forward direction to reach equilibrium.

Explanation:

The reaction quotient Qc is a measure of the relative amount of products and reagents present in a reaction at any given time, which is calculated in a reaction that may not yet have reached equilibrium.

For the reversible reaction aA + bB⇔ cC + dD, where a, b, c and d are the stoichiometric coefficients of the balanced equation, Qc is calculated by:

$Qc=\frac{[C]^{c}*[D]^{d} } {[A]^{a}*[B]^{b}}$

In this case:

$Qc=\frac{[H_{2} ]*[I_{2} ] } {[HI]^{2}}$

Since molarity is the concentration of a solution expressed in the number of moles dissolved per liter of solution, you have:

$[H_{2} ]=\frac{2.09*10^{-2} moles}{1 Liter}$ =2.09*10⁻² $\frac{moles}{liter}$

$[I_{2} ]=\frac{4.14*10^{-2} moles}{1 Liter}$ =4.14*10⁻² $\frac{moles}{liter}$

$[I_{2} ]=\frac{0.280 moles}{1 Liter}$ = 0.280 $\frac{moles}{liter}$

So,

$Qc=\frac{2.09*10^{-2} *4.14*10^{-2} } {0.280^{2} }$

Qc= 0.011

Comparing Qc with Kc allows to find out the status and evolution of the system:

If the reaction quotient is equal to the equilibrium constant, Qc = Kc, the system has reached chemical equilibrium.

If the reaction quotient is greater than the equilibrium constant, Qc> Kc, the system is not in equilibrium. In this case the direct reaction predominates and there will be more product present than what is obtained at equilibrium. Therefore, this product is used to promote the reverse reaction and reach equilibrium. The system will then evolve to the left to increase the reagent concentration.

If the reaction quotient is less than the equilibrium constant, Qc <Kc, the system is not in equilibrium. The concentration of the reagents is higher than it would be at equilibrium, so the direct reaction predominates. Thus, the system will evolve to the right to increase the concentration of products.

Being Qc=0.011 and Kc=1.80⁻²=0.018, then Qc<Kc. The system is not in equilibrium and the reaction must run in the forward direction to reach equilibrium.

8 0

3 years ago