Strawberries contain about 15 wt% solids and 85 wt% water. To make strawberry jam, crushed strawberries and sugar are mixed in a 45: 55 mass ratio, and the mixture is heated to evaporate water until the residue contains one-third water by mass. Calculate how many pounds of strawberries are needed to make a pound of jam and drew

Strawberries contain about 15 wt% solids and 85 wt% water. To make strawberry jam, crushed strawberries and sugar are mixed in a 45: 55 mass ratio, and the mixture is heated to evaporate water until the residue contains one-third water by mass. Calculate how many pounds of strawberries are needed to make a pound of jam and drew

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter1: Introduction To Chemistry

Section: Chapter Questions

Problem 1.11PAE: Some farmers use ammonia, NHS, as a fertilizer. This ammonia is stored in liquid form. Use the...

See similar textbooks

Similar questions

Mass of unchewed gum - 9.1 g mass of chewed gum - 3.6 g mass of sugar - 5.5 g percent of sugar in gum - 60.4% Molar mass of sugar - 342.34 g/mol question? to convert the mass of dissolved sucrose to moles. Show work using dimensional analysis and report the answer with current units and sig. figs
In biological systems, enzymes are used to accelerate the rates of certain biological reactions. Glucoamylase is an enzyme that aids in the conversion of starch to glucose (a sugar that cells use for energy). Experiments show that 1 μg mol of glucoamylase in a 4% starch solution results in a production rate of glucose of 0.6 μg mol/(mL)(min). Determine the production rate of glucose for this system in units of lb mol/(ft3)(day). A. 0.0015 lb mol/(ft3)(day) B. 0.0315 lb mol/(ft3)(day) C. 0.0539 lb mol/(ft3)(day) D. 0.3569 lb mol/(ft3)(day)
The U.S. proven natural gas reserves in 2013 were 323 trillion ft3 . How long will these reserves last if there are no imports or exports and if the U.S. annual rate of use of 24.5 trillion ft3 continues?
Given (2.30x10^6) grams of glucose, C6H12O6, calculate the grams of carbon dioxide, CO2, formed upon complete oxidation of the glucose. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O Express your answer in three significant digits as grams. Note: Your answer is assumed to be reduced to the highest power possible.
Some farmers use ammonia, NHS, as a fertilizer. This ammonia is stored in liquid form. Use the particulate perspective to show the transition from liquid ammonia to gaseous ammonia.
A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 26.742g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool and finds it has a lower mass; the crucible, cover and contents then weigh 25.598g. In the process the sample was converted to off-white anhydrous MnCl2. a. What was the mass of the hydrate sample? _ghydrate b. What is the mass of the anhydrous MnCl2? _gMnCl2 c. How much water was driven off? _gH2O d. What is the percent by mass of water in the hydrate? water=massofwaterinsamplemassofhydrateinsample100 _massH2O e. How many grams of water would there be in 100.0g hydrate? How many moles? _gH2O; _molesH2O f. How many grams of MnCl2 are there in 100.0g hydrate? How many moles? What percentage of the hydrate is MnCl2? Convert the mass of MnCl2 to moles. The molar mass of MnCl2 is 125.85g/mol. _gMnCl2; _molesMnCl2 g. How many moles of water are present per mole MnCl2? _ h. What is the formula of the hydrate? _
During a recent winter month in Sheboygan, Wisconsin, it was necessary to obtain 3500 kWh of heat provided by a natural gas furnace with 89% efficiency to keep a small house warm (the efficiency of a gas furnace is the percent of the heat produced by combustion that is transferred into the house). (a) Assume that natural gas is pure methane and determine the volume of natural gas in cubic feet that was required to heat the house. The average temperature of the natural gas was 56 F; at this temperature and a pressure of 1 atm, natural gas has a density of 0.68 1 g/L. (b) How many gallons of LPG (liquefied petroleum gas) would be required to replace the natural gas used? Assume the LPG is liquid propane [ C3H8 : density, 0.5318 g/mL; enthalpy of combustion, 2219 Id/mo for the formation of CO2(g) and H2O(l) ] and the furnace used to burn the LPG has the same efficiency as the gas furnace. (c) What mass of carbon dioxide is produced by combustion of the methane used to heat the house? (d) What mass of water is produced by combustion of the methane used to heat the house? (e) What volume of air is required to provide the oxygen for the combustion of the methane used to heat the house? Air contains 23% oxygen by mass. The average density of air during the month was 1.22 g/L. (f) How many kilowatt—hours ( 1kWh=3.6106 J) of electricity would be required to provide the heat necessary to heat the house? Note electricity is 100% efficient in producing heat inside a house. (g) Although electricity is 100% efficient in producing heat inside a house, production and distribution of electricity is not 100% efficient. The efficiency of production and distribution of electricity produced in a coal-fired power plant is about 40%. A certain type of coal provides 2.26 kWh per pound upon combustion. What mass of this coal in kilograms will be required to produce the electrical energy necessary to heat the house if the efficiency of generation and distribution is 40%?
The correct equation for net filtration pressure is Group of answer choices NFP = (BHP + IFOP) – (BCOP + IFHP) NFP = (BHP - IFOP) + (BCOP – IFHP) NFP = (BHP + BCOP) – (IFHP + IFOP) NFP = (BHP – BCOP) + (IFHP – IFOP)
The density or specific gravity of the liquid can be used in computing the equivalent weight of the reactant given in milliliters. A. True B. False
High fructose corn syrup is a sweetener found in everyday food items especially carbonated beverages. It is derived from the "fruit" of corn using a bioprocess that degrades corn starch into its constituent sugars. Given the quantity of corn syrup (d = 1.4 kg L^-1) needed for many industries. It should be no surprise that this product is often transported from place to place in tank cars (via railway) where the typical transport mass is 2.290 x 10^5lbs. In the space provided below, calculated the diameter in (meters) of such a tank car's 11.12m long-cylindrical transport container. Recall that 1 gal =3.785 L, kg= 2.205lbs, and 1cm^3 =exactly 1mL
Fill in the remaining columns except kj/mole
A student was given an unknown hydrate, which could be one of threepossibilities: magnesium sulfate heptahydrate, sodium dichromate tetrahydrate orbarium chloride dihydrate. Using the following data identify the unknown.Wt. of crucible/lid empty 39.46 gWt. of crucible/lid/hydrate sample 46.84 gWt. of crucible/lid/sample after heating 45.77 g