Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Glycine is an amino acid made up of carbon, hydrogen, oxygen, and nitrogen atoms. Two samples of glycerine are combusted during an experiment to determine the empirical formula of glycerine.
Sample 1: Combustion of a 0.2036 g sample produced 132.9 mL of CO2 at 25°C and 1.00 atm. and 0.122 g of water.
Sample 2: 0.2500 g of glycine is treated in such a way that all the nitrogen atoms are converted to N2 gas. The volume of the nitrogen gas collected was 40.8 mL at 25°C and 1.00 atm.
Determine:
1. The percentages of carbon and hydrogen in glycine.
2. The percentage of nitrogen in glycine.
3. The percentage of oxygen in glycine.
4. The empirical formula of glycine.
2. The SOHIO ammoxidation process of propyle ne to acrytonitrile is given by the reaction:
C3 HG (9) + Oa (9) + NH3 (g)
Ca Hg N(9) + Hạ0 (g9)
kg
Reaction was done at 430°C and 0.126 atm. If it is desired to produce 2400
of
hr
acrylonitrile, how much propylent in
is used? consider 80% conversion on
hr
propylene.
How many liters of CO2 would be produced at STP from the combustion of 29.1 gg of ethylcyclopentane?
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- Assume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °C and 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?arrow_forwardAssume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °Cand 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?arrow_forwardAt 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropanearrow_forward
- 3. An acetylene tank, C,,, is used for an oxyacetylene welding torch that undergoes a combustion with oxygen. 1. Write the balanced chemical equation h. One acerylene tank provides 8340L of acetylene gas, C,11, at 0 °C and I atm. I How many tanks of molecular oxygen, cach providing 7.00 x 10' L of O. at 0 "C and I atm, will be required to burn the acetylene?arrow_forwardEthane (C2H6) is burned with atmospheric air, and the volumetric analysis of the dry products of combustion yields the following: 10% CO2, 1% CO, 3% O2, and 86% N2. (a) What is the complete combustion equation? (b) What is the theoretical oxygen? (c) What is the percentage of excess air? (d) What is the volume of air in liters (at 25 OC and 1 atm) per / kg fuel?arrow_forwardCalculate the volume of air required for complete combustion of 1m3 of a gaseous fuel having the composition: CO = 46%; CH4 = 10%; H2 = 40%; C2H2 = 2%; N2 = 1% and the remaining being CO2.arrow_forward
- (Record your answer with rounded answer to proper significant digits and the proper units.) 1.How many moles of butane (C4H10(g)) were combusted in the presence of excess oxygen gas if 55.8 L of water vapour at STP is collected?Hint: Write a balanced chemical reaction equation first. 2.One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur. 16H2S(g)+8SO2(g)----->16H2O(g)+3S8(s) 8.75 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur dioxide. Calculate the mass, in kg, of sulfur produced.arrow_forwardThe boiling points of group 16 binary hydrides are as follows: H2O 100 oC; H2S -60 oC; H2Se -41 oC.arrow_forward1) when you start with the original formula, p1 v1=p2v2, what do you get when you isolate P1? 2) A sample of neon gas occupies 200cm3 at 4.0 atm. What would be the volume of the sample at 1.0 atm, assuming th tempature is held contant. 3) A sample of oxygen gas has a volume of 4.0 L, At standard temp and pressure. If the temperature remains constant, what would be the volume of the gas at 202.6 kPa?arrow_forward
- At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropanearrow_forwardwhat is obtained when CaC2 is heated in nitrogen at 1000 degree celsius ?arrow_forwardWhich is more volatile, benzene or ethylbenzene?arrow_forward
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