1. What is the reason why activites are often called effective concentrations? Explain why there are differences between activities and concentrations.
2. Methane dissociates into H2(g) and C(s, graphite).
- Calculate the equilibrium constant K at 298 K.
- Calculate K at 50°C (assuming that ΔrH^Θ is temperature independent.
- Calculate α (degree of dissociation of methane) at 25°C and a total pressure of 0.010 bar.
3. What is the value of ΔrG for the reaction
NO2(g) ⇔ N2O4(g) when
Q = 0.1
Q = 1.0
Q = 10.0
Q= 100.0
Estimate (by interpolation) the value of K from the values you calculated.
Compare with the value obtained from the thermodynamic definition of the equilibrium constant.
In: Chemistry
Consider separate 1.0 L samples of the following gases at STP: Cl2, C2H6, and Xe. Which of the following statements are true regarding these gas samples?
The C2H6 gas sample has the smallest average kinetic energy.
The mass of the gas in each container is the same.
The C2H6 gas molecules collide with the container walls most frequently.
The C2H6 gas sample has the lowest density.
Each Cl2 gas particle collision with the container wall is more forceful as compared to each C2H6 and Xe collision.
The Cl2 gas sample has the most molecules of gas present.
In: Chemistry
Consider the reaction
C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)
in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. Calculate the change in internal energy, ΔE, for this reaction per mole of sucrose.
Express the change in internal energy in kilojoules per mole to three significant figures.
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WORKSHEET 1- answers. i need explanation and wrok shown for each questions.
1) A 2) C 3) E 4) E 5) E 6) E 7) D 8) E 9) B 10) E 11) D 12) C 13) D 14) D 15) B 16) D
http://east.cherryhill.k12.nj.us/Summer_Assignments/pdfs/c01ws01.pdf
In: Chemistry
a) Magnesium metal reacts with HCl solution, liberating H2 gas and generating Mg2+ cations in solution. A 2.780-g sample of Mg metal is added to 50.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. What mass of H2 is formed?
b) What is the concentration of Mg2+ ions in the resulting solution? (Assume the final volume of solution is still the same as the original volume of the acid.)
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When Acetic acid (CH3COOH) reacts with sodium bicarbonate a neutralization reaction occurs: [20 pts]
(a) Write the balanced chemical equation for this reaction.
(b) If you are given 1.26 x 102 g of acetic acid and 1.68 x 102 g of sodium bicarbonate, what reagent would be limiting?
(c) What would be the theoretical yield of the product(s)?
(d) How many grams of excess reagent would be left over?
(e) If the reaction yielded 68.46 g of the gas, 27.52 g of the liquid, and 159.6 g of the salt, what would their percent yields be?
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On the basis of your research, respond to the following:
Why and how does atomic nuclear decay take place? Explain.
What is the significance of atomic nuclear decay?
What is your analysis on the societal implications of using this process?
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What is the purpose of sodium hydrosulfite addition? What is the purpose of potassium ferricyanide in the conversion of luminol to an excited state?
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Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen)
a.) H2(g) + 1/2 O2(g) = H2O(g)
b.) CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)
c.) CH3OH(l) + 3/2 O2(g) = CO2(g) + 2H2O(g)
d.) C6H14(g) + 9 1/2 O2(g) = 6CO2(g) + 7H2O(g)
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A buffer contains 1.0 mol of CH3CO2H and 1.0 mol of CH3CO2- diluted with water to 1,0 L. How many moles of NaOH are required to increase the pH of the buffer to 5.10? pKa of CH2CO2H is 4.74
Can someone explain this step by step please!
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Consider the distillation of ethanol (C2H5OH) and the combustion of ethanol . Use a bullet point list to compare and contrast the 2 processes. There should be at least 5 points of comparison
In: Chemistry
NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.011 M in NH4Cl at 25 °C?
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Calculate the pH of a 0.19 M CH3COOLi solution. (Ka for acetic acid = 1.8 × 10−5.)
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Rank the following compounds in order of increasing strength of intermolecular attractions: H2O2, CF4, KF, and CHCl3
In: Chemistry