Question

The sign of delta H is positive. Increasing the temperature will: A. Increase extent and reaction...

The sign of delta H is positive. Increasing the temperature will:

A. Increase extent and reaction rate

B. Decrease extent and reaction rate

C. decrease extent and increase reaction rate

D. increase extent and decrease reaction rate

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

If the sign of ∆H is positive it means it is an endothermic reaction and as the reaction proceeds Temperature falls due to absorption of heat.

Hence by Le chattliers principle if the temperature is increased then the reaction will move in that direction in which the temperature will fall to minimise the effect of change . Hence the reaction will move in forward direction i.e the extent of reaction will increase . Also with increase in temperature the reaction rate increases , which can be clearly observed from Arrhenius equation.

Therefore the correct option is A. I.e increase extent and reaction rate.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For a Reaction that has positive activation energy, would you expect increasing the temperature to increase...
For a Reaction that has positive activation energy, would you expect increasing the temperature to increase or decrease the reaction rate? Please explain your answer in using "rate=K[A]^x[B]^y" and "K=Ae*-Ea/rT"
1.   Which of the following is true of enzyme catalyzed reactions? a.   Reaction rates are temperature dependent b.   Reaction...
1.   Which of the following is true of enzyme catalyzed reactions? a.   Reaction rates are temperature dependent b.   Reaction rates are pH dependent c.   Reaction rates depend on substrate concentration d.   Reaction rates depend on enzyme structure e.   All of the above f.    a, b, and c 2.   Which of the following is NOT true of enzymes? a.   Enzyme activity depends on reaction conditions. b.   Enzymes are catalysts that decrease the rate of reaction. c.   Enzymes can be inhibited by other proteins d.   Enzymes do not alter the change in free energy...
A) For the reaction CH4(g) + H2O(g) ---> 3H2(g) + CO(g) delta H° = 206.1 kJ...
A) For the reaction CH4(g) + H2O(g) ---> 3H2(g) + CO(g) delta H° = 206.1 kJ and delta S° = 214.7 J/K The equilibrium constant for this reaction at 325.0 K is _____ Assume that delta H° and delta S° are independent of temperature. B) For the reaction N2(g) + 2O2(g)-->2NO2(g) deltaH° = 66.4 kJ and deltaS° = -121.6 J/K The equilibrium constant for this reaction at 327.0 K is _____ Assume that delta H° and delta S° are independent...
1)When delta G= 0; a system is at equilibrium. Use values for delta H and delta...
1)When delta G= 0; a system is at equilibrium. Use values for delta H and delta S to determine the temperature at which the following system would reach equilibrium. N2(g)+ O2(g)--->2NO(g) 2)Complete te following table: Enthalpy change delta H, Etropy change delta S, Predicted Sign for delta G. +(positive) -(negatve) ? +(positive) -(negative) ? -(negative) -(negative) ? -(negative) +(positive) ?
Find the temperature (in K) above which a reaction with a delta H of 123.0 kJ/mol...
Find the temperature (in K) above which a reaction with a delta H of 123.0 kJ/mol and a delta S of 90.0 J/K×mol becomes spontaneous. Use four significant figures. T=________K
If delta H=-50.0kJ and deltaS=-0.500 kj/k, the reaction is spontaneous below a certian temperature. Calculate the...
If delta H=-50.0kJ and deltaS=-0.500 kj/k, the reaction is spontaneous below a certian temperature. Calculate the temperature express your answer numerically in kelvins
What would you predict for the sign of delta h and delta s for the dissolution...
What would you predict for the sign of delta h and delta s for the dissolution of NaF?
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?...
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ A.) The reaction will shift to the right in the direction of products. B.) The equilibrium constant will increase. C.) The equilibrium constant will decrease. D.) The reaction will shift to the left in the direction of reactants. E.) No effect will be observed.
For a particular reaction, delta H is 67.6 kJ/mol and delta S is 126.9 J/(molk). Assuming...
For a particular reaction, delta H is 67.6 kJ/mol and delta S is 126.9 J/(molk). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? The reaction is spontaneous for temperatures less than? Greater than? T= ???? K
given the following information A+B->2D delta H=-710.9kJ delta S= 298.0J/K C->D     delta H =515kJ delta S=-192...
given the following information A+B->2D delta H=-710.9kJ delta S= 298.0J/K C->D     delta H =515kJ delta S=-192 J/K calculate the delta G for the following reaction at 298K. A+B->2C **PLEASE SHOW WORK**
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT