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Laboratory experiment produces volatile compound in gaseous form. You need to collect this sample by adding just enough cryogen (cooling agent) into a rigid vessel to condense your compound as liquid (boiling temperature -23 oC). It is important to keep final pressure at a minimum. You have a choice of dry ice (sublimation from solid to gas at -78.5C (change Sublimation H 25.2kJ/mol, Cp (Co2, gas)= 54.6 J/mol*K) or liquid nitrogen (boiling point -195.8C, Change H vaporization 5.6 kJ/mol, and Cp (NO2, gas)=29.1 J/mol*K) which cryogen should you use?
Homologous recombination is initiated
Using the value of Ka from your titration curve, calculate that pH at the equivalence point?
How do you figure out how long it takes in minutes for light to reach the Earth from the Sun, a distance of 150500000 km
Vinegar must contain at least 4% acetic acid (0.67M). A 5.0mL sample of commercial vinegar required 33.5mL of 0.100M NaOH to reach the equivalence point. Does the vinegar meet the legal limit of 4% acetic acid
Consider a sample of calcium carbonate in the form of a cube measuring 2.305in on each edge. If the sample has a density of 2.73cm^3 , how many oxygen atoms does it contain
The normal melting and boiling points of O2 are -218C and -183C respectively. Its triple point is at -219C and 1.14 torr, and its critical point is at -119C and 49.8 atm.
How much heat is released when 4.50 g of methane gas is burned CH4 (g) + 2O2(g) -> CO2 (g) + 2H2O(l) H=-890kJ
A 2.2g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 45.6 mL of water at 23 degrees C. What is the osmotic pressure of the solution
calculate the amount of heat required to completely sublime 20.0 g of solid dry ice rmco2 at its sublimation
The freezing point depression of water is a rather small 1.86 deg C kg/mol. Addition of 0.454g of zinc chloride to 3.33g of water lowers the melting point by 5.2 deg C. Calculate the expected melting point for this mixture and account for any diff..
More gas is then added to the container until it reaches a final volume of 13.9 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.
Calculate the maximum amount of CO2 that can be produced when 64.0 g of O2 and 64.0 g of CH3 OH are mixed for the reaction 2 CH3OH + 3 O2 → 2 CO2 + 4 H2 O .
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