Biochemistry
9th Edition
ISBN: 9781319114671
Author: Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher: W. H. Freeman
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Calculate the value of K for a reaction that has ΔG° = 37.6 kJ mol-1 at 37.0 °C. (R = 8.3145 J mol-1 K-1) in kj/mol
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- Calculate ΔG° (answer in kJ/mol) for each of the following reactions from the equilibrium constant at the temperature given. (d)CoO(s)+CO(g)⇌Co(s)+CO2(g) T=550°C Kp=4.90×102 (e)CH3NH2(aq)+H2O(l)⟶CH3NH3+(aq)+OH−(aq) T=25°C Kp=4.4×10−4 (f)PbI2(s)⟶Pb2+(aq)+2I−(aq) T=25°C Kp=8.7×10arrow_forwardNonearrow_forwardNonearrow_forward
- Predict the approximate ratio peaks in the mass spectrum of 1,2-Dichloroethane at m/z values 98, 100, and 102.arrow_forwardFor the gas - phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 \deg C, it is found that the partial pressure of C is 0.220 atm. What is AG\deg for this reaction? (R = 8.314 J/mol ·K).arrow_forwardAt 25.0 °C the Henry's Law constant for dinitrogen monoxide (N,0) gas in water is 0.025 M/atm. Calculate the mass in grams of N,0 gas that can be dissolved in 450. mL of water at 25.0 °C and a N,0 partial pressure of 1.31 atm. Be sure your answer has the correct number of significant digits. ?arrow_forward
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