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The four unit separation train shown in figure 1.1 has been designed to separate 1000 gmol/hr of a hydrocarbon feed containing 20% CH4, 25 % C2H6, 40 % C3H8, and the rest C4H10 (molar basis) into five fractions. Given the indicated compositions (molar basis) and assuming that the recycle to unit I is 50% of bottoms from unit II (m6 = 0.5 m5), determine`
A 0.160 g sample of rock was found to have 2.11 × 10-6 mol of potassium-40 (t1/2 = 1.3 × 109 yr) and 2.11 × 10-6 mol of argon-40. How old was the rock? (What assumption is made about the origin of the argon-40?)
For a given reaction, the reaction forms predominantly products at equilibrium (i.e. it essentially goes to completion). Which of the following represents a reasonable value for K
Write the net ionic reaction from the following balanced reactions: 1. FeCl3 (aq) + K3PO4 (aq) = FePO4 (s) + 3 KCI (aq) 2. Ba(NO3)2 (aq) + Ag2SO4 (aq) = 2 AgNO3(aq) + BaSO4 (s)
Calcite (CaCO3) has two types of bond. (covalent and ionic) a) Demonstrate which is the stronger by calculating the degree of ionic character of each bond
Amphetamines in urine can be confirmed by mass spectroscopy at a concentration of 500 ng/mL. Assuming a urine density of 1.025 g/mL, what is this concentration in parts per million
"A mixture of CH4 and H2O is passed over a nickel catalyst at 100 degrees K. The emerging gas is collected in a 5.00-L flask is found to contain 8.62g of CO, 2.60 g of h2, 43.0 g of CH4, and 48.4 g of H2O.
Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to 20.0 mL of 0.100 M NH3
a solution of NaOH is added to the supnatant liquid until it is strongly alkaline. No precipitate is formed. Which ions are present in each of the precipitates. Which cations are not present in the original solution?
Rank the following slightly insoluble compounds from the most soluble to the least soluble. CaCO3 Ksp = 2.8 x 10-9 Co(OH)2 Ksp = 1.6 x 10-15 CaF2 Ksp = 3.9 x 10-11 BaSO4 Ksp = 1.1 x 10-10
If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 202 kPa.
Complete and balance the following redox equation using the smallest whole-number coefficients. Show the steps. Sn (s) + HNO3 ? SnO2 (s) + NO2 + H2O (not balanced, assume acidic solution)
Assume that the maximum number of ATP's is produced (38). At pH 7, and in the presence of excess Mg2+
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