Question

Part A At 100°C, $K_c$ = 4.72 for the reaction 2NO2 (g) $\rightleftharpoons$ N2O4 (g) An empty 10.0 L flask is filled with 2.30 g of NO2 at 100°C. What is the total pressure in the flask at equilibrium? $P_{total}$ = 0.147 atm Check your rounding. Your final answer should be rounded to 3 significant figures in the last step. No credit lost. Try again. Submit Previous Answers Request Answer

          Part A
At 100°C, $K_c$ = 4.72 for the reaction
2NO2 (g) \(\rightleftharpoons\) N2O4 (g)
An empty 10.0 L flask is filled with 2.30 g of NO2 at 100°C.
What is the total pressure in the flask at equilibrium?
$P_{total}$ = 0.147 atm
Check your rounding. Your final answer should be rounded to 3 significant figures in the last step.
No credit lost. Try again.
Submit Previous Answers Request Answer

Part A
At 100°C, Kc = 4.72 for the reaction
2NO2 (g) ⇌ N2O4 (g)
An empty 10.0 L flask is filled with 2.30 g of NO2 at 100°C.
What is the total pressure in the flask at equilibrium?
Ptotal = 0.147 atm
Check your rounding. Your final answer should be rounded to 3 significant figures in the last step.
No credit lost. Try again.
Submit Previous Answers Request Answer

Added by Jason M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

03/14/2023

Step 1

Given: - Mass of NO2 = 2.30 g - Molar mass of NO2 = 46.01 g/mol Calculate moles of NO2: moles = mass / molar mass moles = 2.30 g / 46.01 g/mol moles = 0.050 mol Show more…

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Part A At 100°C, Kc = 4.72 for the reaction 2NO2(g) ⇌ N2O4(g) What is the total pressure in the flask at equilibrium? An empty 10.0 L flask is filled with 2.30 g of NO2 at 100°C. Ptotal = 0.147 atm Check your rounding. Your final answer should be rounded to 3 significant figures in the last step. No credit lost. Try again.