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Consider 1.00 L of air in a patient's lungs at 37.0 C and 1.00 atm pressure. What volume would this air occupy if it were at 25.0°C under a pressure of 5.00* 10-2 atm (a typical pressure in a compressed air cylinder)?
Suppose that coal of density 1.5 g/cm3 is pure carbon. (It is, in fact, much more com- plicated, but this is a reasonable ?rst ap proximation.)
if a molecule of a neon gas travels at an average of 400.m/s at a given temperature, estimates the average speed of a molucule of butane gas, C4H10, at the same temperature.
What is the molarity of a HCl solution if the reaction of 223 mL HCl with excess CaCO3 produces 10.7 L CO2 gas at 714 mmHg and 36°C?
If the minimum energy required to break the C-Cl bond in CF3Cl is 540 kJ/mol, what is the longest wavelength of radiation that will break this bond?
The density of aluminum is 2.702 g/cm3. What is the final liquid level of water if 1.130 ounces (oz) of aluminum is dropped into a graduated cylinder containing
consider the following equilibrium system H2(g)+ Br2(g)=2HBr(g) Keq= 14.8 A closed container is initially filled with equal moles of H2 and Br2.When equilibrium is reached the (HBr) is 0.329 mol/L What is the initial (H2)
If 69.5 kJ of heat is applied to a 1038 g block of metal, the temperature of the metal increases by 11.4°C. Calculate the specific heat capacity of the metal in J/g°C.
How much water must be added to 534. mL of 0.180 M HCl to produce a 0.135 M solution? (Assume that the volumes are additive.)
A 4.70 g nugget of pure gold absorbed 285 J of heat. The initial temperature was 24.0°C. What was the final temperature.
Does beta-D-fructose in its cyclic form have the same number of chiral carbons as beta-D-glucose?
Calculating the molecular formula of an organic compound. Worked example, using fundamental formula and balanced equations.
What mass of this substance must evaporate in order to freeze 230 of water initially at 24? (The heat of fusion of water is 334 the specific heat of water is 4.18 .)
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