1.NaN3 (s)- Na (s) + N2 (g)Provided above is the UNBALANCED decomposition reaction of sodium azide, NaN3used to inflate safety airbag. Determine the amount (in gram) of NaN3 required to beused if the target volume of N2 gas is 6.6 L. Given the airbag is tested in standardtemperature and pressure (STP) condition.A measurement of lead concentration in a river water is 4.2 x 10° mol/L. If thedrinking water safety limit of lead is set 15 ppb, determine whether the river water issafe for drinking. Given the density of the solution is 1 g/mL.2.A 42 L gas cylindrical tank was filled with oxygen gas. The gas tank was moved froma storage with a temperature of 37 °C (25 atm pressure) to a laboratory with atemperature of 21 °C. Determine the pressure of the tank in the laboratory.3.A fully filled 1000 L sewage water tank contains 55 mol of dissolved non-volatilewaste material.i.Calculate the osmotic pressure required for the reverse osmosis system toproduce clean water. Given the temperature of the tank is 35 °C.Determine the pressure if the waste material above are replaced with similaramount of glucose (MW = 180.156 g/mol). Explain your answer.ii.4.

Balancing a chemical equation is necessary so as to abide by the law f conservation of mass and to…

1. NaN3 (s) → Na (s) + N2 (g) Provided above is the UNBALANCED decomposition reaction of sodium azide, NaN3 used to inflate safety airbag. Determine the amount (in gram) of NaN3 required to be used if the target volume of N, gas is 6.6 L. Given the airbag is tested in standard temperature and pressure (STP) condition.

1. NaN3 (s) → Na (s) + N2 (g) Provided above is the UNBALANCED decomposition reaction of sodium azide, NaN3 used to inflate safety airbag. Determine the amount (in gram) of NaN3 required to be used if the target volume of N, gas is 6.6 L. Given the airbag is tested in standard temperature and pressure (STP) condition.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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+ ou add to the document will 1. At 18°C and 102.0 kPa, 1.29 L of a gas weighs 2.71 g. Calculate the approximate molar mass of the gas. 2. Determine the volume occupied by 4.00 g of oxygen gas at STP. 3. What volume would 15.0 g of argon occupy at 90°C and 735 mm of mercury? 4. Compute the approximate density of methane CH4, at 20°C and 5.00 atm. 5. If the density of carbon monoxide is 3.17 g/L at -20°C and 238 kPa, what is its approximate molar mass? 6. If 200 mL of a gas weighs 0.268 g at STP what is its molar mass? 7. Compute the volume of 11.0 g of nitrous oxide, N₂O, at STP. 8. What volume will 1.216 g of SO, gas occupy at 18°C and 100.6 kPa? 9. Compute the mass of one litre of ammonia gas at STP. 10. Determine the density of H₂S gas at 27°C and 2.00 atm. 11. A 1.225 g mass of volatile liquid is vapourized giving 400 mL of vapour when measured over water at 30°C and 102.6 kPa. The vapour pressure of water at 30°C is 4.27 kPa. What is the molar mass of the liquid. 12. Find the…
[References] Use the References to access important values if needed for this question. How many grams of carbon disulfide are needed to completely consume 91.1 L of chlorine gas according to the following reaction at 25 °C and 1 atm? carbon disulfide ( s ) + chlorine ( g ) → carbon tetrachloride (I) + sulfur dichloride (s) grams carbon disulfide Submit Answer Try Another Version 1 item attempt remaining EGO Not Visited ot Previous Next Show Hint 10 四图t 10 tv 27 MAR 34 280 MacBook Air
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O Macmillan Learning An herbicide contains only C, H, Cl, and N. The complete combustion of a 200.0 mg sample of the herbicide in excess oxygen produced 209.2 mL of CO₂ and 122.0 mL of H₂O vapor at STP. A separate analysis determined the 200.0 mg sample contained 55.14 mg Cl. Determine the percent composition of the herbicide. percent carbon: percent hydrogen: percent chlorine: percent nitrogen: Determine the empirical formula of the herbicide. empirical formula: The herbicide has a molar mass of 257.16 g/mol. What is the molecular formula of the herbicide? molecular formula: % % % %
Since volume and pressure are inversely related, we can make some assumptions about initial and final states using the data provided. We can also identify initial and final states by finding trigger words in the language of the problem. Look for words like “first,” “initially,” or “originally” to describe initial states and “result” or “after” for final states. What volume would a sample of helium occupy at 6.0 atm if the helium was initially compressed in a 1.0 L tank at 20. atm at constant temperature? Organize your data into the table to help analyze the problem. Leave blank any boxes for which you do not have information. Drag the appropriate labels to their respective targets.
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