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One of the vibrational modes (the asymmetry stretch) of the CO2 molecule is at 2349 cm-1. Convert this to eV, nm and K.
The equilibrium constant is always greater than one for an extensive reaction 6.The value of q is always equal to the value of w for a reversible reaction 7.The energy change of the universe for any spontaneous process is always positive
A solution of water at 30 degrees Celsius is placed in a freezer at a constant temperature of -8 degrees Celsius. Calculate the entropy change of the system, surroundings, and the universe.
Really confused on calculating/finding the half-equivalence point in a titration curve. This was a lab experiment done in my chem lab. We added 0.0750 M NaOH to acetic acid (pipet 10.00mL of ~0.1M HCH3CO2 into the beaker and add 40mL of DI water).
For each of the following pairs of compounds, explain the difference in melting point in terms of the intermolecular forces involved. a) hexane (C6H14) m.p. = -96 0C vs. octadecane (C18H38) m.p. = 28 - 30 0C
What are the primary uses of the 3 products mentioned? 2.) What are the ACTIVE ingredients?
The partial pressures of gas A and gas B, respectively, are 0.379 atm and 0.675 atm. If 0.190 mol a third gas is added with no change in volume or temperature, what will the total pressure become?
A sample of sodium reacts completely with 0.142 of chlorine, forming 234 of sodium chloride. What mass of sodium reacted?
NaOH + CO2 -→ Na2CO3 + H2O . If the average human body discharges 536 g of CO2 per day, how much NaOH is needed each day for each person in the spacecraft?
Refer to the Galvanic cel below (the contents of each half-cell are written beneath each compartment): 0.10 M MnO4- 0.40 M Cr3+
2I2 + N2H4 4HI + N2 a.How many grams of I2 are needed to react with 36.7 g of N2H4?
Which of the following statements is/are correct. i. KBr, HClO3, and HClO2 are strong acids ii. NaH, KOH, and Li2O are strong bases iii. HI, HClO3, and HNO3 are strong acids
If the barometeric pressure was 0.98 atm when the mercury level in an open-end manometer connected to a flask of gas was 177 mmHg higher on the side open to the atmosphere than on the flask side
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