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tangare [24]
3 years ago
14

The following reaction is exothermic. C6H12O6(s)+6O2(g)⇌6CO2(g)+6H2O(g)C6H12O6(s)+6O2(g)⇌6CO2(g)+6H2O(g) Predict the effect (shi

ft right, shift left, or no effect) of increasing and decreasing the reaction temperature.
Chemistry
2 answers:
inna [77]3 years ago
7 0

Answer:

Increasing temperature = balance will shift to the left

Decreasing temperature = balance will shift to the right

Explanation:

Step 1: Data given

The increase or decrease in temperature can have an influence on the position of the equilibrium.

If the temperature is increased, the system will ensure that less heat is released. So the balance will shift to the left.

When the temperature drops, however, the system will produce more heat: the balance will shift to the right.

Step 2: The balanced equation

C6H12O6(s) + 6O2(g) ⇌ 6CO2(g) + 6H2O(g)

This is an endothermic reaction

Step 3: Increasing the temperature

If the temperature were increased, the heat content of the system would increase.

In exothermic reactions, increase in temperature decreases the K value. This means less products will be formed. The balance will shift to the left.

Step 4: Decreasing the temperature

If the temperature were decreased, the heat content of the system would increase.

In exothermic reactions, decrease in temperature increases the K value. This means more products will be formed, less reactants. The balance will shift to the right.

elena55 [62]3 years ago
4 0

Answer:

According to Le Chatelier's principle, increasing the reaction temperature of an exothermic reaction causes a shift to the left and decreasing the reaction temperature causes a shift to the right.

Explanation:

C6H12O6(s) + 6O2(g) ⇌6CO2(g) + 6H2O(g)

We are told that the forward reaction is exothermic, meaning heat is removed from the reacting substance to the surroundings.

According to Le Chatelier's principle,

1. for an exothermic reaction, on increasing the temperature, there is a shift in equilibrium to the left and formation of the product is favoured.

2. if the temperature of the system is decreased, the equilibrium shifts to right and the formation of the reactants is favoured.

3. if the reaction temperature is kept constant, the system is at equilibrium and there is no shift to the right nor to the left.

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Given the equation representing a reversible reaction:which formula represents the h+ acceptor in the forward reaction?
AnnyKZ [126]
Question is incomplete. Complete question is attached below
.............................................................................................................................

Answer: Option A: HCO3-(aq.)

Reason:
From the reaction, it can be seen that following reaction occurs in forward direct

HCO3-(aq)     +     H2O(l)      →      H2CO3(aq)     +      OH-(aq)

In above forward reaction, HCO3- accepts proton from H2O to generate H2CO3. Thus, according to Lowry and Bronsted theory of acid-base, HCO3- is a base, while H2CO3 is a conjugate acid. 

8 0
3 years ago
How many mL of a stock 50% (w/v) KNO3 solution are needed to prepare 250 mL of a 20% (w/v) KNO3 solution?
Andre45 [30]

Answer:

100ml of a stock 50% KNO3 solutions are needed to prepare 250ml of a 20% KNO3 solution.

Explanation:

In the given question it is mentioned that

     S1=50%

      V2=250ml

      S2= 20%

We all know that

                     V1S1=V2S2

                     ∴V1=  V2×S2÷S1

                     ∴V1=  V2S2×1/S1

                      ∴V1= 250×20÷50

                       ∴V1= 100ml

 

6 0
3 years ago
Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2NO+2 H2(g)-N29)+2H2O(9) Write the pressure equilibr
lara31 [8.8K]

Answer:

Partial pressure N₂ . (Partial pressure H₂O)² / (Partial pressure H₂)² . (Partial pressure NO)² = Kp

Explanation:

The reaction is:

2NO + 2H₂ → N₂ + 2H₂O

The expression for Kp (pressure equilibrium constant) would be:

Partial pressure N₂ . (Partial pressure H₂O)² / (Partial pressure H₂)² . (Partial pressure NO)²

There is another expression for Kp, where you work with Kc (equilibrium constant)

Kp = Kc (R.T)^Δn

where R is the Ideal Gases constant

T° is absolute temperature

Δn = moles of gases formed - moles of gases, I had initially

4 0
3 years ago
Take some points!!!​
VMariaS [17]

Answer: thanks babe

Explanation:

8 0
3 years ago
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