For this equation, (NH4), Cr2 O7(s) Cr2O3 (s) + N2 (g) + 4H2O(9). an engineer has to calculate the volume of gases that are produced under standard temperature and pressure conditions, given that 5,882 g of ammonium dichromate will decompose. Select the three values that they need to solve this problem. the molar mass of ammonium dichromate the molar mass of nitrogen gas the molar mass of water STP molar gas volume: 22.4 L/mol O Avogadro's number: 6.02e23 particles/mol The molar ratio from the balanced equation

For this equation, (NH4), Cr2 O7(s) Cr2O3 (s) + N2 (g) + 4H2O(9). an engineer has to calculate the volume of gases that are produced under standard temperature and pressure conditions, given that 5,882 g of ammonium dichromate will decompose. Select the three values that they need to solve this problem. the molar mass of ammonium dichromate the molar mass of nitrogen gas the molar mass of water STP molar gas volume: 22.4 L/mol O Avogadro's number: 6.02e23 particles/mol The molar ratio from the balanced equation

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 46QRT

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Similar questions

109 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed volume in advance?
Dichlorine oxide is used as bactericide to purify water. It is produced by the chlorination of sulfur dioxide gas. SO2(g)+2Cl2(g)SOCl2(l)+Cl2O(g)How many liters of Cl2O can be produced by mixing 5.85 L of SO2 and 9.00 L of Cl2? How many liters of the reactant in excess are present after reaction is complete? Assume 100% yield and that all the gases are measured at the same temperature and pressure.
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.
The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the compression stroke to the pressure in the beginning. Assume that compression occurs at constant temperature. The total volume of the cylinder in an automobile is 350 cm3, and the displacement the reduction in volume during the compression stroke is 309 cm3. What is the compression ratio in that engine?
What is the value of the ideal gas constant R if the volume is specified in milliliters rather than liters?
A sample of a breathing mixture for divers contained 34.3% helium, He; 51.7% nitrogen, N2; and 14.0% oxygen, O2 (by mass). What is the density of this mixture at 22C and 775 mmHg?
5-113 Ammonia and gaseous hydrogen chloride react to form ammonium chloride according to the following equation: If 4.21 L of NH3(g) at 27°C and 1.02 atm is combined with 5.35 L of HCI(g) at 26°C and 0.998 atm, what mass of NH4CI(s) will be generated?
A sample of natural gas is 85.2% methane, CH4, and 14.8% ethane, C2H6, by mass. What is the density of this mixture at 18C and 771 mmHg?
Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do this, calculate a 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). On a graph show the apparent molar mass versus the 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?
A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are ZnS(s)+2HCL(aq)ZnCl2(aq)+H2S(g)PbS(s)+2HCL(aq)PbCl2(aq)+H2S(g) If the sample reacted completely and produced 1.049 L of hydrogen sulfide, H2S, at 23C and 762 mmHg, what were the percentages of ZnS and PbS in the mixture?
Uranium hexafluoride, UF6, is a white solid that sublimes (vaporizes without melting) at 57C under normal atmospheric pressure. The compound is used to separate uranium isotopes by effusion. What is the rms speed (in m/s) of a uranium hexafluoride molecule at 57C?

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