#89 ill lbe producect? Which 1s the limiting reactont Brass of NHuCls)89.) Ammonia andchloride NH, (4)+ HC/q)'NHYCI(5)If 4.21L of NH3g)5.352 ofgasas hydrogen chloride combine to form ammanivemat 27°c and l.02 aton is combineel with.af 210°C and 998ortm, whatpresent in excess??Whichge'sTOL) During the making of steel, iron (I) oxide is reduced to metalticiron' by treatment with-carbon monoxideFeOrs) +CO (g)- Fe(s) +COz (g)Suppose 1.45kg of Fe reots. What volume of COg) is requirod,and what volume of COzegs is produced, tach measuced ot STP?gas.

In the given reaction below, ammonia and gaseous HCl combine together to form solid NH4Cl NH3(g) +…

89.) Ammonia and chloridea NHa (a) °t HCI (a)-NHy CI(s) 1f 4.21L of NH3ca) at 27°c and 1.02 aton is combineed with. 5.35E af HClia af 20°c and 998artm, what pmass of NtyCIS) will be producect Which is the li present in excess? gaseavs hydrogen chloride combine to form ammenivem. niting reactont?which go's is

89.) Ammonia and chloridea NHa (a) °t HCI (a)-NHy CI(s) 1f 4.21L of NH3ca) at 27°c and 1.02 aton is combineed with. 5.35E af HClia af 20°c and 998artm, what pmass of NtyCIS) will be producect Which is the li present in excess? gaseavs hydrogen chloride combine to form ammenivem. niting reactont?which go's is

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 113AE: Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN....

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At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of O2 will be produced during the production of 1.00 mole of gold?
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)
Nitric acid can be prepared by bubbling dinitrogen pentoxide into water. N2O5(g)+H2O2H+(aq)+2NO3(aq)(a) How many moles of H+ are obtained when 1.50 L of N2O5 at 25C and 1.00 atm pressure is bubbled into water? (b) The solution obtained in (a) after reaction is complete has a volume of 437 mL. What is the molarity of the nitric acid obtained?
A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour. Given the following data, determine Hf for the hydrocarbon: Hreaction=2044.5KJ/molhydrocarbonHf(CO2)=393.5KJ/molHf(H2O)=242KJ/mol Density of CO2 and H2O product mixture at 1.00 atm, 200.c = 0.751g/L. The density of the hydrocarbon is less than the density of Kr at the same conditions.
A 230-L sample of a colorless gas at STP decomposed to give 230 L of N2 and 1.25 L of O2 at STP. What is the colorless gas?
A 36.0—L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g 02, and 4,880 g N2. At 25 degrees C. what is the pressure in the cylinder in atmospheres?
9.87 What will be the final temperature of a mixture made from equal masses of the following: water at 25.0 C, ethanol at 35.5 C, and iron at 95.0 C?
5-39 An 8.00-g sample of a gas occupies 22.4 L at 2.00 atm and 273 K. What is the molar mass of the gas?
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?
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.
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