Chem 121 Module 3 Exam

app.101edu.co Question 59 of 59 How many grams of Na solid are required to completely react with 19.2 L of Cl, gas at STP according to the following chemical reaction? Remember 1 mol of an ideal gas has a volume of 22.4 L at STP. 2 Na(s) + Ch(g) 2 NaC(s) STARTING AMOUNT ADOFACTOR ANSWER RESET 0.0373 19.7 1.71 22.99 0.857 6.022 x 1023 30.4 68.90 22.4 35.45 39.4 19.2 mol Cl g Na g/mol Na L Na mol Na g/mol Cl g Ch L C,

I start with 21.60 g of nitrogen . After reacting it yields 1.3 moles of ammonia. What is the percent yield of my reaction? N2 + 3H2 – > 2NH3 (This nitrogen fixation reaction is called the Haber process and is used to produce ammonia for things such as fertilizer.

STARTING AMOUNT X What volume in liters of H₂ gas would be produced by the complete reaction of 2.93 2 g of Al solid at STP according to the following reaction? Remember 1 mol of an ideal gas has a volume of 22.4 L at STP. 2 Al(s) + 6 HCI (aq) → 2 AICI, (aq) + 3H₂(g) = ANSWER 3 ADD FACTOR x( ) 6 mol H₂ 26.98 22.4 g Al 2.93 LAI DELETE X A 1 2.02 1.62 LH₂ 2 mol Al 6.022 × 1023 7.30 g H₂ RESET 5 3.65 g/mol H₂ 0.329 g/mol Al +

Bree Serif 26 6. 3 A gas at 25°C has a volume of 335 mL and a pressure of 1.01 atm. If we increase the pressure of this gas to 1.35 atm, then what is the new volume of the gas? Inventory: Equation: P, V = P, V, P, P, = %3D 1 1 2 1 BYJU'S V, = V = 1 5 Kg 5 Kg V1 a 1/P1 V2 a 1/P2

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Part A How many liters of CO₂ gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3Hg and an excess of O₂ according to the following equation? C3Hg (g) +502 (g) → 3CO2 (g) + 4H2O(g) ▾ View Available Hint(s) ▼ Hint 1. General approach to solving the problem First, convert from moles of C3Hg to moles of CO2 using the mole ratio from the balanced chemical reaction. Then use the ideal gas equation to find volume of CO₂ using the given temperature and pressure, and the number of moles you calculated in step one. See Section 10.5 (Page 408). O24.6 L O249 L O27.6 L 82.9 L Submit de Feedback Review | Constants I Periodic T Request Answer Pearson

app.101edu.co Question 22 of 24 At STP, 22.50 mol of gas occupies approximately what volume? 1 4 6. 8 9. +/- х 100 MacBook Pro Q Search or type URL & ( ) 4 8 R { | 2. ト %24

A 5.60 g of solid CO2 sample is placed in an empty sealed 500 mL container at a temperature of 80°C. When all the solid CO2 becomes gas:  (i) What is the number of moles of CO2? Answer mol (Answer to 2decimal place) (ii) What is the temperature in Kelvin? AnswerK  (ii) What will be the pressure in the container? Answer atm (Answer to 2decimal places) (Hint: assume CO2 is a perfect (ideal) gas)

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Determine-Molar-Volume-of-Gas (1) - Word ilings Review View Help O Tell me what you want to do 三 外|T AaBbCcDc AaBbC AaBbCcC AaB AABBCCD AaBb- AaBbCcDc I Normal T No Spac. Heading 1 Heading 2 Title Subtitle Subtle Paragraph Styles Table 3: Molar Volume - 2 trials Information Trial 1 Trial 2 Atmospheric Pressure" (mmHg) Mass of Mg Ribbon (g) Volume of H2 gas collected (mL) Temperature of H2 gas (°C) Temperature of Water Bath (°C) Vapor Pressure of Water (mmHg) *Use the atmospheric pressure given 756.14 756.14 0.0342 g 0.0350 g 36.5 36.5 21.2 21.2 21.2 21.2 18.7 18.7 Calculations A. Use the atmospheric pressure and the vapor pressure of water to determine the pressure of the hydrogen gas you collected (in atmospheres, atm). B. Use the combined gas law with your calculated pressure, measured temperature and measured volume to determine the volume of the hydrogen gas at STP. C. Calculate the moles of magnesium ribbon used. DELI

1 4 7 +/- Question 13 of 21 1.65 g of an unknown gas at STP fills a 500. mL flask. What is the molar mass of the gas? 2 5 8 | g/mol 3 60 9 O Submit Tap here or pull up for additional resources XU x 100

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Problems1. The decomposition of ammonia gas (a process that occurs at high temperatures) is 2NH3(g) → N2(g) + H2(g)If a balloon was filled with 3.5 L of ammonia gas and all of the gas decomposed, what wouldbe the total volume of gas in the container? Assume the pressure and temperature remainconstant. Is your equation balanced? Is that necessary?

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A mixture containing 2.27 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture. PCH4    ?  =  atm PC2H4    ?  =  atm PC4H10    ?  =  atm (b) Calculate the total pressure of the mixture. _____ atm

A 0.418 g sample of gas has a volume of 115 L at25 C° and 10 atm. What is the molar mass of this gas. (R=0.082 Latm/Kmol)   Pls answer on paper ty :)

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*00 Pl nq 4 2. 4. $4 V< IIC g Al partial pressure of water at 27°C is 26.8 mmHg. of hydrogen gas over water at 27°C and 751 mmHg. How many grams of aluminum reacted? The Aluminum reacts with excess hy drochloric acid to form aqueous aluminum chloride and 44.9 mL answer in "Xog papiAo.d əyn u JƏ

© Macmillan Learning A container of N₂O₂(g) has a pressure of 0.460 atm. When the absolute temperature of the N₂O3(g) is tripled, the gas completely decomposes, producing NO₂(g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change. # 3 final pressure: E D C $ 4 R F 1.38 Incorrect V % 67 5⁰ 5 T G < 6 B MacBook Pro Y H & 7 N U J * 8 M K 9 H < O L I ) 0 L P 1 command option { [ ? 1 11 + } ] atm delete retu

What temperature (in °C) did an ideal gas shift to if it was initially at -23.5 °C at 4.33 bar and 35.0 L and the pressure was changed to 8.71 bar and the volume changed to 15.0 L?

||| O STATES OF MATTER Calculating the mass of a gas collected over water Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 63.9 mL. x10 X collected Ś gas water 0/5 Sketch of a gas-collection apparatus Calculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. 1 g 1 chemical reaction SI

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At 1.25 atm and 685 K, what volume of CO2 gas forms from the combustion of 34.28 g of C4H10? 2C,Но(8) + 13 0,(8) — 8СО,(g) + 10H,0() First, calculate the number of moles of CO, formed in this reaction and show the conversions required to solve this problem. mol CO2 34.28 g CH10х Answer Bank 44.01 g CO2 13 mol O2 1 mol H2O 18.02 g H20 10 mol H2O 1 mol CO2 58.14 g C4H10 1 mol O2 1 mol C4H10 8 mol CO2 32.00 g O2 2 mol C4H10 Then, use the ideal gas law to calculate the volume of CO2 gas formed. L V = II