Make the indicated pressure conversions.
msp;
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Introductory Chemistry: A Foundation
- perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forwardA 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?arrow_forwardWhile resting, the average 70-kg human male consumes 14 L of pure O2 per hour at 25 C and 100 kPa. How many moles of 02 are consumed by a 70 kg man while resting for 1.0 h?arrow_forward
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- Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?arrow_forwardA tank is filled with gas to a pressure of 875 mm Hg at 25C. The gas is transferred without loss to a tank twice the size of the original tank. If the pressure is to remain constant, at what temperature (in C) should the tank be kept?arrow_forwardCalculate the molar volume of ethane at 1.00 atm and 0C and at 10.0 atm and 0C, using the van der Waals equation. The van der Waals constants are given in Table 5.7. To simplify, note that the term n2a/V2 is small compared with P. Hence, it may be approximated with negligible error by substituting nRT/P from the ideal gas law for V in this term. Then the van der Waals equation can be solved for the volume. Compare the results with the values predicted by the ideal gas law.arrow_forward
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