At - 10.0 °C the concentration equilibrium constant K = 4.0 × 10 Here are some facts about the reaction: 5 for a certain reaction. • If the reaction is run at constant pressure, 85.0 kJ/mol of heat are released. • If the reaction is run at constant pressure, the volume increases by 13.%. • The net change in moles of gases is -1. Using these facts, can you calculate K at -23. °C? Yes. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. ☐ If you said no, can you at least decide whether Kat -23. °C will be bigger or smaller than K at -10.0 °C? C C Yes, and K will be bigger. Yes, and K will be C smaller. No.

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At - 10.0 °C the concentration equilibrium constant K = 4.0 × 10
Here are some facts about the reaction:
5
for a certain reaction.
• If the reaction is run at constant pressure, 85.0 kJ/mol of heat are released.
• If the reaction is run at constant pressure, the volume increases by 13.%.
• The net change in moles of gases is -1.
Using these facts, can you calculate K at -23. °C?
Yes.
No.
If you said yes, then enter your answer at right. Round it to
2 significant digits.
☐
If you said no, can you at least decide whether Kat
-23. °C will be bigger or smaller than K at -10.0 °C?
C
C
Yes, and K will be
bigger.
Yes, and K will be
C
smaller.
No.
Transcribed Image Text:At - 10.0 °C the concentration equilibrium constant K = 4.0 × 10 Here are some facts about the reaction: 5 for a certain reaction. • If the reaction is run at constant pressure, 85.0 kJ/mol of heat are released. • If the reaction is run at constant pressure, the volume increases by 13.%. • The net change in moles of gases is -1. Using these facts, can you calculate K at -23. °C? Yes. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. ☐ If you said no, can you at least decide whether Kat -23. °C will be bigger or smaller than K at -10.0 °C? C C Yes, and K will be bigger. Yes, and K will be C smaller. No.
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