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If a sample of q that is currently P=0.5atm and T=100K and you increase the temperature to 200K, what phase change have you caused? (a) melting (b)sublimation (c) freezing (d) boiling (e) no phase change, system is at equilibrium throughout heating. The phase diagram starts at 0K and gradually increases from 100k to 200k and as it hits 200K, the line splits apart increasing in pressure
compute the enthalpy change, (Delta H), for this reaction per mole of A. suppose that the specific heat =[4.18J/(g*Degrees C) and density=1.00(g/mL)?
According to Avogadro's law, how many liters of hydrogen are required to react with 1.9L of oxygen at STP.
Determine after how many days will one-sixteenth of a given amount of radon-222 remain and Determine the values of Delta E and Delta H for the system?
How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO) molecules? Enter the ratio of the rates of effusion.
What mass of ethylene glycol, HOCH2CH2OH, must be dissolved in 4.510 kg of water to result in a freezing point of 18.0°C? What is the boiling point of the same solution?
what is the density of hydrogen sulfide at 1.2 atm and 307 K? answer in units of g/L
Explain the fact that even though dibenzoylmethane (C6H5COCH2COC6H5) is not a methyl ketone, it gives a positive iodoform test when treated with the NaOH and I2.
4 HNO3(aq) + Cu(s) => Cu(NO3)2(aq) + 2 H2O(l) + 2 NO2(g) Considering which elements are being oxidized and reduced, determine
C2H5OH(l) + C3H7COOH(l) C3H7COOC2H5(l) + H2O(l) Determine the mass of ethyl butanoate produced if 3.30 mol of ethanol is used.
butane has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -.4 degrees Celsius. A 250 mL sealed flask contains .75 g of butane at -22 degrees C.
What volume, in liters, of O2 at 35°C and 1.19 atm can be produced from the decomposition of 10.0 g KNO3? 2 KNO3(s) → 2 KNO2(s) + O2(g)
Calculate the density of a block.
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