the following sets of information write an equation. Assume that each set of information describes a linear relationship. Assume Y is the variable measured on the vertical axis and X is the variable measured on the horizontal axis. Write all equations in slope-intercept form. a. When X = 10‚ Y = 5 and when X = 7‚ Y = 2. Answer: First find the slope of the line: slope = rise/run = (5 – 2)/(10 – 7) = 1. Then‚ write the equation in general form: Y = mX + b and substitute
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PROPORTION METHOD The proportion method is used in both of these expressions. A proportion is an equation that says that two ratios are equivalent. The use of cross multiplying is in use in both expressions as well. I believe the first expression (#56) uses the extreme-means property; the product of the means is equal to the product of the extremes. #56. To estimate the size of the bear population on the Keweenaw Peninsula‚ conservationists captured‚ tagged‚ and released 50 bears
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Math IA IB MATH SL Math IA Introduction: In this task I will consider a set of numbers that are presented in a symmetrical pattern and try to find a general equation to find the elements in the [pic]row. Consider the five rows of number shown below. Figure 1 Lacsap’s Fractions The aim of this task is to find the numerator of the sixth row and to find the general statement for [pic]. Let [pic] be the [pic]element
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reactors‚ or nature‚ can be described by reaction equations. Knowing the skeletal reaction equation‚ the reactants and the products are also known‚ but for quantitative predictions‚ the reaction equation needs to be balanced. A balanced equation is an equation or a chemical reaction in which the number of atoms for each element in the reaction and the total charge are the same for both the reactants and the products. (1) From a balanced equation‚ the mole relationship can be figured out. The amount
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calculate their mole-to-mole ratio. The mole-to-mole ratio relating to the disappearance of copper and the formation of silver metal will be used to write the balanced equation for the reaction. The reaction of copper metal with silver nitrate solution is a single replacement reaction‚ represented by the following unbalanced equation: Cu(s) + AgNO3(aq) → Cu(NO3)2(aq) + Ag(s) The values of the coefficients can be determined experimentally by measuring the mass of copper wire that reacts with
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Rate = [pic] Rate = -[pic] = -[pic] = [pic] = [pic] Notes: • The minus sign makes the value of the rate positive (since A2 < A1). • The division of each concentration by the coefficient from the balanced equation makes all of the above rates equal. • The unit of rate could be moles per liter per second (mol L-1s-1) or Ms-1 Example: Write the rate expressions of the following reaction in terms of the reactants and products H2(g) +
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Aim To investigate the relationships that exists when lines are drawn on a plane. Strategies To develop some conjectures‚ rules and patterns by investigating the relationships that form between the number of lines‚ intersections points‚ and bounded and unbounded regions. I plan to use rules to further define the relationship. The following relationships will be investigated: # Lines# Lines# Lines# Lines # Lines# Intersects# Lines# Lines# Lines# Lines- # unbounded regions min # bounded
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Chapter 2: Linear Functions Chapter one was a window that gave us a peek into the entire course. Our goal was to understand the basic structure of functions and function notation‚ the toolkit functions‚ domain and range‚ how to recognize and understand composition and transformations of functions and how to understand and utilize inverse functions. With these basic components in hand we will further research the specific details and intricacies of each type of function in our toolkit and use
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Introduction The purpose of this experiment is to determine the rate equation for the “Iodine Clock Reaction” experiment. The experiment will consider the equations 〖2I〗^-+S_2 O_8→2〖〖SO〗_4〗^(2-)+I_2 and I_2+2〖S_2 O_3〗^(2-)→2I^-+S_4 O_6 in order to determine the rate law of Rate=k[〖〖S_2 O_8〗^(2-)]〗^a 〖[I^-]〗^b by using the experimental data to calculate the values of exponents a and b as well as the rate constant k. Experimental Supplies Needed: 250 mL Erlenmeyer flask‚ 100 mL beaker‚ graduated
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k1=[CH4][Cl2] CH3(g)+Cl2(g)⟶CH3Cl(g)+Cl−(g)(step 2 (fast)) with an elementary rate law of‚ k2=[CH4][Cl2] The steps combine to generate the final reaction equation‚ CH4(g)+2Cl2(g)⟶CH3Cl(g)+HCl(g)+Cl−(g)(overall reaction) Example 2a nsider the following reaction: CO(g)+NO2(g)→CO2(g)+NO(g)(overall reaction) This reaction equation suggests that the carbon monoxide directly reacts with nitrogen dioxide to form the products. However‚ its reaction mechanism shows this is not the case. Consider
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