Concept explainers
(a)
Interpretation:
The given equation should be converted to one relating P(psig), V(ft3), n (lb-mole) and T (°F).
Concept introduction:
The equation given is in standard unit as
Here, it has to be converted into FPS unit for which different equality factors and conversations have to be used.
(b)
Interpretation:
The total amount of gas (lb-mole) and the mass of CO (lbm) in the tank should be calculated.
Concept introduction:
The derived equation must be used as:
(c)
Interpretation:
The temperature (°F) which is required to gain certain gas pressure of 300 psig, the rated safety limit of cylinder should be calculated.
Concept introduction:
The derived equation should be used as:
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Chapter 3 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- 3. (a) jf 10.0 mjL of H2jSO4 (sp. jr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SO4 = 98; SO3 = 80 %3Darrow_forwardNitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the On decomposition of liquid nitroglycerin (C;H;(NO3),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 74.0 L of carbon dioxide gas are produced by this reaction, at a temperature of - 13.0 °C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits.arrow_forward5.53 The vapor pressure of liquid water at 25°C is 23.8 torr, and its molar enthalpy of vaporization at 25°C and 23.8 torr is 10.5 kcal/mol. Assume the vapor behaves ideally, neglect the effect of a pressure change on H and S of the liquid, and calcu- late AH298, AS%98, and AG398 for the vaporization of water; use only data in this problem. Compare your results with values found from data in the Appendix. 298arrow_forward
- The relationship between pressure (in kPa), temperature (in Kelvin), and the specific volume (in- m/kg) ofa gas can-be expressed by the Redlich-Kwong equation of state as follows:¶ RT p = a v - b v(v+ b)VT" Where R=universal-gas constant (0.518 kJ/kg.K), a = 0.427R?T?* /Pc, dan-b = 0.0866R T./ Pe; Wwhere T, and-p, are critical temperature and the critical pressure of the gas, respectively. The transportation of compressed natural gas (CNG)'usesa special tank that can withstand high- pressure and ·low temperature. Assume that the CNG-contains-100% methane (critical- temperature =191-K, critical pressure=4600-kPa) at -40°C and 6500-kPa. Use the-bisection method to determine the mass of CNG-in the tank-if the tank volume is 3.5-m³. (Hint: Derive the- abovementioned-equation to form-0 =f(v,a,b,T,R),use VL=0.01 m³/kg-as the lower bound- and vu=0.02 m/kg as the upper-bound, and perform the iteration until the approximate error less- then 10%).arrow_forward1. [15] Atmospheric pressure (P) decreases with increasing altitude (h) based on the following exponential function (with e as the base): P = Pº 1 exp Mgh RT where Pº=1 atm at h=0 (sea level) and T'is the average temperature of the atmosphere, M the molar mass of air (29 g mol-¹), and g the standard gravity. Please estimate the boiling point of water at atmospheric temperature T=293.2 K, and height h=3000 m. The heat of vaporization of water at 293.2 K is 44.22 kJ mol-arrow_forwardDetermine the volume (L) of hydrogen needed (based on room temperature 25 °C and l atm) to hydrotreat 1 liter crude oil with 1.8 wt % S to a sulfur content of 0.2 wt%. The oil has a specific gravity of 0.8 (compared to water). The stoichiometry follows the following reaction: Oil-S + 2H2¬→O¡I-H2 + H2Sarrow_forward
- How many of the following are found in 15.0 kmol of xylene (C3H10)? (a) kg C3H10; (b) mol C3H10; (c) Ib-mole C3H10: (d) mol (g-atom) C; (e) mol H; (f) g C; (g) g H; (h) molecules of C3H10.arrow_forwardThe liquefied petrolieum gas(LPG) is composed of 80% C;Hg and 20% C4H10 in mass basis. (1). Determine the molar fraction of C3H8 and C4H10 in LPG. (2). Determine the stoichiometric air fuel ratio of the LPG. (3). Determine the lower heating value of LPG in kJ/m³ at 25°C and 100 kPa. (4). LPG is mixed with excess air to burn in a boiler at 100 kPa. The CO2 in burned gas is 7% on dry basis. Determine the equivalence ratio of the mixture.arrow_forward1. A wet gas from a field in Iran is processed through two stages of separation; first stage separator operates at 220 psia and 71°F, while the stock tank operates at atmospheric pressure and 69°F. The separator gas condensate ratio is 41,000 scf/STB and the stock tank gas condensate ratio is 450 scf/STB. The molecular weights of the separator gas and stock tank gas are 25.0 and 35.0 lb/lb-mol, respectively. The stock tank condensate gravity is 0.85 and its molecular weight is 125 lb/lb-mol. Let us calculate the specific gravity of the reservoir gas in a step-wise manner, by considering quantities for one STB of condensate. Note that 1.0 bbl is 5.614 ft. Separator gas MWsg = 25 lb/lb-mol 41,000 scf/STB Reservoir gas 1st stage separator 220 psia and 71°F Stock tank gas MWsg = 35 lb/lb-mol 450 scf/STB 2nd stage separator (Stock tank) 14.7 psia and 69°F MW=125 lb/lb-mol SGstc = 0.85 Stock tank condensate a. to one STB. Calculate the mole number [lb-mole] of the stock tank condensate that…arrow_forward
- Methane (CH4) is burned with air (79% N2 and 21% O2 by volume) at atmospheric pressure. The molar analysis of the flue gas yields CO, %3D 10.00%, O2 = 2.41%, C0= 0.52%, and N2 = 87.07%. Balance the combustion %3D equation and determine the mass air-fuel ratio, the of stoichiomet- percentage ric air, and the of excess air. percentagearrow_forwardTo evaluate the use of renewable resources, an experiment was carried out with rice hulls. After pyrolysis, the product gas analyzed 6.4% CO2, 0.1% O2, 39% CO, 51.8% H2, 0.6% CH4, and 2.1% N2. It entered a combustion chamber at 90 °F and a pressure of 35.0 in. Hg and was burned with 40% excess air (dry) at 70 °F and an atmospheric pressure of 29.4 in. Hg; 10% of the CO remains. a. How many cubic feet of air were supplied per cubic foot of entering gas? b. How many cubic feet of product gas were produced per cubic foot of entering gas if the exit gas was at 29.4 in. Hg and 400 °F?arrow_forwardNitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H;(NO3),) into gaseous dinitrogen, 5 gaseous dioxygen, gaseous water and gaseous carbon dioxide. x10 2. Suppose 30.0 L of carbon dioxide gas are produced by this reaction, at a temperature of -7.0 °C and pressure of exactly 1 atm, Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits. garrow_forward
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