Please correct answer and don't use hend raiting moles=☐Hydrogen gas has a density of 0.090 g/L, and at normal pressure and 2.49 °C one mole of it takes up 22.4 L. How would you calculate the moles in 160. g ofhydrogen gas?Set the math up. But don't do any of it. Just leave your answer as a math expression.Also, be sure your answer includes all the correct unit symbols.°G0.0

This can be done using dimensional analysis. By starting with the mass of H2, you can convert it to…

Answered: moles= ☐ Hydrogen gas has a density of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter5: Gases

Section: Chapter Questions

Problem 175MP

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62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
You heat 1.000 quart of water from 25.0C to its normal boiling point by burning a quantity of methane gas, CH4. What volume of methane at 23.0C and 745 mmHg would you require to heat this quantity of water, assuming that the methane is completely burned? The products are liquid water and gaseous carbon dioxide.
What does “STP’ stand for? What conditions correspond to STP? What is the volume occupied by one mole of an ideal gas at STP
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
Define the joule in terms of SI base units.
For many purposes we can treat methane (CH) as an ideal gas at temperatures above its boiling point of -161. °C. Suppose the temperature of a sample of methane gas is raised from -21.0 °C to 23.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.28 kPa and the volume decreased by 60.0%, what is the final pressure? Round your answer to 2 significant digits. kPa x10 X S
A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 113. kPa. The piston is now pulled up, expanding the gas, until the gas has a final volume of 20.0 L. Calculate the final pressure of the gas. Be sure your answer haş the correct number of significant digits. piston cylinder gas olo Ar ||kPa x10
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Q2a. Sulfur dioxide (SO2), a gas that plays a central role in the formation of acid rain, is found in the exhaust of automobiles and power plants. Consider a 1.53L sample of gaseous SO2 at a pressure of 5.6 x 103 Pa. If the pressure is changed to 1.5 x 104Pa at a constant temperature, what will be the new volume of the gas? b.If one molecule with the empirical formula C3H7 has a mass of 1.428 x 10-22 g, determine the molecular formula of the compound
Please show how you got your answer. Thanks
A sample of Hydrogen Gas (H2) has a volume of 8.56 L at a temperature of 0 o C and a Pressure of 1.5 atm. Calculate the number of H2 molecules present in this gas sample. (R= 0.08206 L • atm/K • mol).

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