Chapter 5: Problem 12
Why do astronauts have to wear protective suits when they are on the surface of the moon?
Chapter 5: Problem 12
Why do astronauts have to wear protective suits when they are on the surface of the moon?
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Get started for freeDry ice is solid carbon dioxide. A 0.050 -g sample of dry ice is placed in an evacuated \(4.6-\mathrm{L}\) vessel at \(30^{\circ} \mathrm{C}\). Calculate the pressure inside the vessel after all the dry ice has been converted to \(\mathrm{CO}_{2}\) gas.
A \(2.5-\mathrm{L}\) flask at \(15^{\circ} \mathrm{C}\) contains a mixture of three gases, \(\mathrm{N}_{2},\) He, and \(\mathrm{Ne},\) at partial pressures of \(0.32 \mathrm{~atm}\) for \(\mathrm{N}_{2}, 0.15 \mathrm{~atm}\) for \(\mathrm{He},\) and \(0.42 \mathrm{~atm}\) for Ne. (a) Calculate the total pressure of the mixture. (b) Calculate the volume in liters at STP occupied by He and Ne if the \(\mathrm{N}_{2}\) is removed selectively.
At \(27^{\circ} \mathrm{C}, 10.0\) moles of a gas in a \(1.50-\mathrm{L}\) container exert a pressure of 130 atm. Is this an ideal gas?
Convert \(562 \mathrm{mmHg}\) to atm.
Dissolving \(3.00 \mathrm{~g}\) of an impure sample of calcium carbonate in hydrochloric acid produced \(0.656 \mathrm{~L}\) of carbon dioxide (measured at \(20.0^{\circ} \mathrm{C}\) and \(792 \mathrm{mmHg}\) ). Calculate the percent by mass of calcium carbonate in the sample. State any assumptions.
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