H2(g) + Cl2(g) ----> 2 HCl(g) (OR H2(g) + Cl2(g) right arrow 2 HCl(g) Use the following conversions: 1 mol = MW in g (2 d.p.) = 22.414 L What is the percent yield of HCI if 50.00 g of H2 (MW = 2.02 12 ads to formation of 231 g of HCI (MW= Theoretical yield = (Express with unit and compound, for example 'g Zn'). Percent yield = (Express as '%'). x (1805 g HCI, 1800 g HCI, 1805.0 g HCI, 1804.95 g HCI, 1810 g HCI) Theoretical Yield x (12.8 %, 12.8%, 12.80 %, 12.798 %, 13 %, 13%, 12.80%, 12.798%, 13.%, 13. %) Percent Yield

H2(g) + Cl2(g) ----> 2 HCl(g) (OR H2(g) + Cl2(g) right arrow 2 HCl(g) Use the following conversions: 1 mol = MW in g (2 d.p.) = 22.414 L What is the percent yield of HCI if 50.00 g of H2 (MW = 2.02 12 ads to formation of 231 g of HCI (MW= Theoretical yield = (Express with unit and compound, for example 'g Zn'). Percent yield = (Express as '%'). x (1805 g HCI, 1800 g HCI, 1805.0 g HCI, 1804.95 g HCI, 1810 g HCI) Theoretical Yield x (12.8 %, 12.8%, 12.80 %, 12.798 %, 13 %, 13%, 12.80%, 12.798%, 13.%, 13. %) Percent Yield

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 63QAP: Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L....

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Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
17. A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetraoxide (N2O4), which ignite on contact to form nitrogen gas and water vapor. How much in grams of the excess reagent is used up when 435.0 g of N2H4 and 718.5 g of N2O4 are mixed? (, MW: N204 = 92.011g/mol, N2H4 = 32.05g/mol, N2 =28.013 g/mol 2N2H4(0) + N2O40) –> 3N2(9) + 4H2O(g)
Hydrogen gas (MW = 2.02 g/mol) can be produced from the reaction of methane (MW = 16.05 g/mol) and water vapor (MW = 18.02 g/mol) according to the following reaction equation (called methane reforming): CH4(g) + H2O(g) --> CO(g) + 3 H2(g) If 262 g of CH4 reacts with excess H2O at 423 K and 0.862 atm, what volume of H2 gas will form?
PV=nRT R= 0.0821 atmL/molK Molar Mass of H, = 2 g/mol. Ammonium sulfate, (NH,),SO, is an important fertilizer and can be prepared by the reaction of ammonia (NH,) with sulfuric acid (H,SO,) according to the following balanced equation: 2 NH, + H,SO, (NH,),SO, 11. a. Calculate the moles of NH, needed to react with 0.35L of a 1.25 M H, SO, solution. b. How many liters of NH, gas are needed if the pressure is 0.9 atm and the temperature is 266 K? (NOTE: You will need your answer from part a to calculate this answer)
A sample containing a mixture of SrCl, · 6 H,0 (MW = 266.62 g/mol) and CSCI (MW = 168.36 g/mol) originally weighs 1.6017 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl, · 6 H,0, leaving the anhydrous SrCl,. After cooling the sample in a desiccator, it has a mass of 1.1433 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 320 °C SrCl, · 6 H,0(s)- SrCl, (s) + 6 H,O(g) wt% Sr = wt% Cs = wt% CI =
+ vill 2) Consider the reaction in this experiment: NaNO2(aq) + H₂NSO,H(s) □NaHSO4(aq) + N2(g) + H₂O) If you start with 1.3 g of H₂NSO,H and an excess amount of NaNO2, (a) How many moles of N₂ will be produced? (b) What volume will the N₂ occupy at 25°C and 0.978 atm?
16. The combustion of gasoline (octane) in a car engine can be represented by the following equation: 2C3H18(1) + 2502(g) a. What mass of oxygen is used up to burn a full tank of 36.00 kg of gasoline? Text --> 16CO2(g) +18H20(g) b. Why might a vehicle that is calibrated to run perfectly at sea level run poorly at higher elevations? Text Тext According to the Canadian Automobile Association, the average Canadian drives 20,000 km/yr. C. Assuming that distance, how many more kg of carbon dioxide are added to the atmosphere each year by a Toyota Tacoma (fuel economy of 12.8 L/100 km) than a Toyota Prius (4.52 L/100 km)? The density of gasoline is 0.719 kg/L.
1) The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between NaHC03 and citric acid CO2(8) + H,0(1) + Na3CgH;O;(aq) NaHCO;(aq) + H;C,H;O;(aq) a) In a certain experiment 1.00 g of NaHCO3 and 1.00 g of citric acid are allowed to react. Which is the limiting reactant? b) How many grams of sodium citrate (the last compound in the equation) form? c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? d) If 0.723 g of sodium citrate was obtained in this reaction, then what is the percentage yield?
For the following reaction: 5Ca + V2O5 --> 5CaO + 2V In one process 5 moñ of V2O5 react with 3 mol of acá. Calculate the theoretical yield of V in the unit of mol.
9:08 PM ☹ & = ikf MB² = 5.12 °C/m 19²2- (-130%) = AT £ 1Jf=18492 ug°c = (5.12 L/m) n = 3.611 ●●● 25 Question 9 of 14 | g 1 3 4 6 7 9 +/- 0 Tap here or pull up for additional resources 8 What mass in grams of NaCl would need to be added to 2051 g of water to increase the boiling temperature of the solution by 1.500 °C? (Kb for water is 0.5100 °C/m) X C 20% 0 Submit x 100
5.) If 2.45 liters of benzene are consumed in this reaction at 1.1 atm and 25 C, how many liters of water are formed? 2 C6H6(g) + 15 02(g) --> 12 CO2(g) + 6 H20(g) * O 0.110 Liters O 0.330 Liters O 5.3 Liters O 7.34 Liters O 22.4 Liters