HCl is at 2.30 atm, O2 is at 1.00 atm and they both react at 750 K. Equilibriumpressure of Cl2 is .93 atm. How do you go about finding the Kp at 750 K?
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For a reaction of the type, aA + bB ---- cC + dD involving gases, we have, Kp = {[pC]^c * [pD]^d }/[pA]^a ...
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The following solution is comprised of an explanation of how to go through the following chemistry-based question step-by-step. The solution is about 50 words.
2NOBr(g) + Br2(g) <----> 2BrNO(g) @ equilibrium. NOBr is 34% dissociated at 25degreesC and total pressure is 0.25 atm.
Calculate Kp and Kc.
I know how to get Kp and Kc with given # of moles @ equilibrium, but cannot figure out how to get it from the percent dissociation. I tried inputting various values that I thought wer
(See attached file for full problem description)
1) The slope field for the system
dx/dt = 2x + 6y
dy/dt = 2x - 2y
is shown to the right
a) determine the type of the equilibrium point at the origin.
b) calculate all straight-line solution.
2) show that a matrix of the form A =(a b; -b a) with b!=0 must have complex eig
GDP/Equilibrium and MPC questions:
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C = 250 Billion +. 80GDP
Please use equation above for following questions:
1. If the planned investment is $200 billion, the equilibrium level of GDP is:
2. If the equilibrium is $2000 billion, autonomous investment is:
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The Equilibrium Constant.
Question:
Consider the reaction 2 NO2Cl(g) = 2 NO2(g) + Cl2(g).
A 12.0-L container holds these gases at equilibrium. What is the value of Kc for this reaction if there are 1.036 g NO2Cl, 5.962 g NO2, and 4.578 g Cl2 at equilibrium?
How will each of the following changes in demand and/or supply affect equilibrium price and equilibrium quantity in a competitive market; that is, do price and quantity rise, fall, or remain unchanged, or are the answers indeterminate because they depend on the magnitudes of the shifts?
a Supply decreases and demand is const
Given the following reaction: C0(g) + H2O(g) <> C02(g) + H2(g) (Please see the attachment for the properly formatted reaction).
a) Write the equilibrium constant expression for this reaction. Note: gaseous-phase H20 is included in the equilibrium expressions, unlike liquid phase H20.
b) The equilibrium constant for the reactio
