At — 10.8 °C the concentration equilibrium constant Kc= 4.0 x 10^-5 for a certain reaction.

Here are some facts about the reaction:

If the reaction is run at constant pressure, the volume increases by 14. %.

The constant pressure molar heat capacity Cp= 2.63 J. mol^-1 K^-1

If the reaction is run at constant pressure, 120. kJ/mol of heat are released.

Required:

a. Using these facts, can you calculate Kc at -16. °C?

i. Yes

ii. No

b. If you said yes, then write your answer.

c. If you said no, can you at least decide whether Kc at -16 °C will be bigger or smaller than Kc at-10.8 °C?

i. Yes, and Kc will be bigger.

ii. Yes, and Kc will be smaller.

iii. No

Someone offer some answers to this, i will give 98 coins and mark as brainliest! i will put the rest of the lab down in the comments, solutions pre-lab questions: in this lab, you will make fruit drinks with powdered drink mix. complete the pre-lab questions to get the values you need for your drink solutions. calculate the molar mass of powered fruit drink mix, made from sucrose (c12h22o11).using stoichiometry, determine the mass of powdered drink mix needed to make a 1.0 m solution of 100 ml. (hint: use molarity = to find the moles of drink mix, then convert moles to grams using a mole conversion.)what mass of powdered drink mix is needed to make a 0.5 m solution of 100 ml?

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