The addictive power of nicotine is enhanced by which of the following chemicals?

When is a roman numeral most likely needed in the name of an ionic compound?

Sauron [17]

The answer is I’m guessing c

5 0

3 years ago

A reaction produced 37.5 L of oxygen gas at 307 K and 1.25 atm. How many moles of oxygen were produced? 0.538 mol, O2 1.86 mol,

zlopas [31]

Answer:

O 2 has a mass of 1.78g

Explanation:

We are at STP and that means we have to use the ideal gas law equation!

P represents pressure (could have units of atm, depending on the units of the universal gas constant)

V represents volume (must have units of liters)

n represents the number of moles

R is the universal gas constant (has units of

L

× a t m

m o l

×

K

)

T represents the temperature, which must be in Kelvins.

Next, list your known and unknown variables. Our only unknown is the number of moles of

O

2

(

g

)

. Our known variables are P,V,R, and T.

At STP, the temperature is 273K and the pressure is 1 atm. The proportionality constant, R, is equal to 0.0821

L

×

a

t

m

o

l

×

K

Now we have to rearrange the equation to solve for n

n

=

P

V

R

T

n

=

1

atm

×

1.25

L

0.0821

Lxxatm

m

o

l

×

K

×

273

K

n

=

0.05577

m

o

l

To get the mass of

O

2

, we just have to use the molar mass of oxygen as a conversion factor:

0.0577

mol

O

2

×

32.00

g

1

mol

= 1.78g

O

2

3 0

3 years ago

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Using relative enthalpy and entropy values, determine how the process is affected after each of the following temperature or pre

lutik1710 [3]

The question is incomplete, the complete question is:

Using relative enthalpy and entropy values, determine how the process is affected after each of the following temperature or pressure changes? Consider that a more effective reaction produces more product or more product in a shorter amount of time.

Reaction: SO2 (g) + 2H2S (g) ↔ 3S(s) + 2H2O (g)

Substance | ΔG kJ/mol | ΔH kJ/mol

H2O(g) | -228.6 | -241.8

H2O(l) | -237.1 | -285.8

SO2(g) | -300.4 | -296.9

SO3(g) | -370.4 | -395.2

H2S(g) | -33.01 | -20.17

S(s) | 0 | 0

Categorize into: "More Effective" ~ "Less Effective" ~ "Equally Effective"

- Temp. decreases while maintaining container size

- Temp. increases while maintaining container size

- Pressure decreases while maintaining container size

- Pressure increases while maintaining container size

Answer:

Explanation:

ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants)

ΔH∘rxn= [0+2(-241.8)] - [(-296.9) + 2(-20.7)]= -145.6KJ/mol

ΔG∘rxn=[(0+ 2(-228.6) -[(-300.4) + 2(-33.01)]= -90.78KJ/mol

The reaction is spontaneous since ΔG∘rxn is negative

The reaction is exothermic since ΔH∘rxn= negative

1) increase in pressure is less effective because it favours the reverse reaction.

2) increase in temperature is less effective since it favours the reverse reaction given that the reaction is exothermic in nature

3) decrease in pressure is more effective, it favours the forward reaction

4)Decrease in temperature is more effective because it favours the forward reaction.

5 0

3 years ago

4. Assuming the reaction below is at equilibrium, which of the following changes will drive the reaction to the left? C(s) + O2(

shepuryov [24]

Answer:

Increasing temperature

Explanation:

$C(s) + O_2(g) \leftrightharpoons CO_2(g)$

Enthalpy of the reaction = -393.5 kJ/mol

Negative sign implies that reaction is exothermic.

Effect of change in reaction condition is explained by Le chateliers principle.

According to Le chateliers principle, if the reaction conditions of a reversible reaction in a state of dynamic equilibirum is changed, the reaction will move in a direction to counteract the change.

1. Increasing the temperature

Forward reaction is exothermic that means temperature increases in forward direction. Backward reaction will be endothermic and so there is decrease in temperature in backward direction or in left direction.

On increasing temperature, reaction will be move in direction to counteract the increased temperature, therefore reaction will move in left direction.

2. Adding O2

If O2 is added, then reaction will move in a direction in which its get consumed. So, reaction will move in forward direction or in right direction.

3. Removing C (s)

Le Chatelier's principle does not apply on solids, so removal of C(s) does not affect the equilibrium.

4 0

4 years ago

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Given the reaction 2CO + O2 = 2CO2, what is the minimum number if moles of O2 required to produce one mole of CO2?

Aliun [14]

Answer:

0.5 moles of O₂

Explanation:

See the stoichiometry of the reaction:

2CO + O₂ → 2CO₂

2 moles of carbon monoxide need 1 mol of oxygen to react in order to produce 2 moles of carbon dioxide.

If I want to produce 1 mol of CO₂, I just need the half of O₂.

You will see in this rule of three. Ratio is 2:1

2 moles of CO₂ are produced by 1 mol of O₂ (Stoichiometry - reaction)

1 mol of CO₂ will be produced by ( 1 . 1) / 2 = 0.5 moles

8 0

3 years ago

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