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Due to the difficulty of locating the precise point at which the slope of the modulus line begins to change, indicating the onset of plastic deformation and the yield point. By placing a line parallel to the modulus line it is much easier to see the precise point at which they intersect. The selection of .2% is just a convenient distance to provide a good visible intersection and assure a very reasonable degree of accuracy.
What else can I help you with?
Find the yield strength from a stress-strain graph?
Follow the graph's positive slope (across the first quadrant) until the graph is no longer linear. The yield strength is determined to be the last point (with concern given to the stress value) on the linear section. After this point the graph is irregular because the material has failed to a point of no return and can no longer handle the load (stress).
What is the tensile strength of .375 bolt?
Tensile strength is a material propery, it does not depend on size. Look at a material chart to find its yield and tensile strenghts. Then use the stress equation, Stress = Force / Area to determine if your .375 bolt can handle the force on it. If your bolt is in shear, you need to find Shear strenghts.
What is axial load?
An axial load is a force administered along the lines of an axis. This is typically used to describe an injury in which there is compression of the spine from the head, such as when a person dives head first into shallow water and hits the top of his head on the bottom. This frequently causes fractures of the spine and possibly spinal cord injury. It is also commonly used to describe a specific strength of materials known as their uniaxial compressive or tensile strength and also to find the variation of their strength with increasing confining pressure (as used in triaxial testing).
What is the tensile strength of dry paper?
Oh, dude, you're asking about the tensile strength of dry paper? Well, buckle up because dry paper can typically withstand around 20-30 megapascals of force before it tears. So, like, next time you're tearing up some paper, just remember it's putting up a decent fight with that tensile strength.
Find offsets with elbows on round ductwork?
adding an elbow is like adding another piece of duct,in other words you will gain length. you have to measure using centers. lets say that you have a duct that you want to make an offset to change your location or elevation,measure the distance from starting point to finish point either end to center or center to center,say your measurement is 12in. end to center, measure the elbow from the end to the center,usually by putting it on a table or againist a wall, say your meas. is 6in. bear in mind that the elbow will fit over the duct,lets say 2in. that means the elbow will add 4in. to your duct, subtact 4in.from your 12in.meas. that leaves you with 8in. of duct to make your offset
How do you find 85.0 percent in percent yield?
if you received 85.0 percent back from your product then your percent yield is 85 percent.
What is the percent yield of 122 grams of product?
If this is the actual yield, real amount produced, then you need the theoretical yield to find the percent yield. % yield = (actual yield / theoretical yield) x 100
When 320g octane C8H18 is burned in oxygen 392g of water is recovered what is the percent yield of the experiment?
To find the percent yield, first calculate the theoretical yield of water by converting the mass of octane to moles, using stoichiometry to find the mole ratio between octane and water, and then converting back to grams. Next, divide the actual yield (392g) by the theoretical yield and multiply by 100 to get the percent yield.
Calculate the percent yield of chlorine gas in the decomposition of hydrochloric acid if 25.8 grams of hydrochloric acid produces 13.6 grams of chlorine gas?
Percent yield can be calculated using the formula: (actual yield / theoretical yield) x 100. First, determine the theoretical yield of chlorine gas by finding the molar ratio between hydrochloric acid and chlorine gas. Once you have calculated the theoretical yield, plug the values into the formula to find the percent yield.
When 300g of ammonia reacted with excess sulfuric acid to produce ammonium sulfate 985 g of product were obtained what is the percent yield of ammonium sulfate for this reaction?
The theoretical yield of ammonium sulfate can be calculated based on the amount of ammonia used. To find the percent yield, divide the actual yield (985 g) by the theoretical yield and multiply by 100. Percent yield = (actual yield / theoretical yield) x 100.
When 50.9 g of silicon dioxide is heated with an excess of carbon 32.3 g of silicon carbide is produced SiO2 plus 3C ----- SiC plus 2CO what is the percent yield of this reaction?
To calculate percent yield, we need to compare the actual yield to the theoretical yield. The actual yield is the measured amount of product produced, which is 32.3 g of silicon carbide. The theoretical yield can be calculated by stoichiometry. Convert 50.9g of SiO2 to moles, determine the limiting reactant, and calculate the theoretical yield of SiC. Finally, using the formula: percent yield = (actual yield / theoretical yield) * 100, we find the percent yield.
Why do you find percent yield?
This allows you to compare different investments. In general (other things being equal), you would normally prefer an investment which gives you a larger percent yield for any given time period.
Two successive reaction a to b and b to c have yields of 86 and 47 respectively what is the overall percent yield for conversion of A to C?
As a general rule, the overall percent yield is the product of individual yields of the successive reactions under consideration. In this case, the overall percent yield for conversion of A to C can be calculated as (0.86 X 0.47 = 0.4042) i.e. 40.42% or about 40% after rounding up. Hope this answers the question.
Nitrogen and hyrogen form ammonia by the reaction N2 plus 3H2 to 2NH3. If 56 grams of nitrogen and 85 grams of hydrogen react to form 62 grams of ammonia. What is the percent yield?
To find the percent yield, first calculate the theoretical yield of ammonia based on the given amounts of nitrogen and hydrogen. Then compare the actual yield (62g) with the theoretical yield to calculate the percent yield using the formula: (actual yield/theoretical yield) x 100%. The percent yield would be the actual mass of ammonia produced (62g) divided by the theoretical yield of ammonia.
What is the percent yield for the reaction of 6.92 g of K and 4.28 g of O2 if 7.36 g of KO2 is recovered in the laboratory?
First you need to find the theoretical yield for the reaction:2Na + O2 ---> Na2O2(1) find the theoretical yield of 3.74 g of Na, i.e. if all of the Na is reacted3.74 g Na *(1 mol Na/22.99 g Na)*(1 mol Na2O2 formed/2 mol Na reacted)*(77.98 g Na2O2/1 mol Na2O2) = 6.34 g Na2O2(2) % yield = (actual yield / theoretical yield)*(100%)% yield = (5.34 g / 6.34 g) *(100%) = 84.2% yield
What is the percent yield of carbon disulfide if the reaction of 33.4 g of sulfur dioxide produces 10.1 g of carbon disulfide?
Percent yield is calculated by dividing the actual yield by the theoretical yield, then multiplying by 100. Actual yield = 10.1 g Theoretical yield of carbon disulfide can be calculated using stoichiometry. The molar mass of SO2 is 64.07 g/mol and the molar mass of CS2 is 76.14 g/mol. By stoichiometry, we find that 33.4 g of SO2 would produce 12.6 g of CS2. Using the formula: Percent yield = (10.1 g / 12.6 g) x 100 = 80.2%.
How do you calculate the percent yield of an element in a reaction?
The actual yield is given within the worded problem. The theoretical yield however is to be found. In order to calculate the theoretical yield, you need to convert the mass of the limiting reagent (LR) to the mass of the reagent in excess (ER). To find the limiting reagent, you need to first convert the mass of the limiting reagent to the mass of the reagent in excess (to find the theoretical yield)A. Convert mass of limiting reagent to mass reagent in excess (mass --> mass); in other words, find the mass of the reagent consumed.1. Multiply the mass of the limiting reagent by the # molecules of the reagent in excess and its molar mass.2. Divide the above by the # of molecules LR which is multiplied by its molar mass.Mass LR x # molecules ER x molar mass ER-- # molecules LR x molar mass LR3. Subtract the original mass of reagent in excess and the consumed reagent in excess.Original mass Reagent in Excess - Consumed Reagent in Excess= Reagent leftover/unused (theoretical yield).B. Find the percent yield of the product.--- Actual YieldTheoretical Yield x 100%
