Ideal Gas Law Constant Lab Report Dr Z Edits

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Hi! I'm a college student and i need your help in answering my chemistry subject. Please do help me and I promise to rate it helpful. Please put an understandable or clearer solutions and if possible you can put a brief explanation. Thank you so much and God bless!  Nitrogen oxide is oxidized ina air to give brown nitrogen dioxide. If you have 2.2 moles of NO, 2NO(g)  + O2(g) → 2NO2(g), therefore,  you need _____ moles of O2 for complete reaction and produce _____ moles of NO2

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Can I get help on Moles of H2O2 and O2 please?? Based on my numbers what numbers do I need to punch into the calculator to get my calculation?

Answer With Work Shown Please . 1. CaO + H2O → Ca(OH)2 If you start with 2400 g of CaO, add excess water, and produce 2060 g of Ca(OH)2, what is the percent yield of the reaction? 2.Draw the Lewis dot structure of SiCl4 then determine if the molecule has polar bonds and if it is a polar or non-polar molecule. 3.If you have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 870C, how many moles of gas do I have? R=0.0821 L*atm/K*mol

2.) It’s a bad day in the lab!  Two students are doing experiments.  Each is 20 feet away from the professor.  At the same time, each of them lets the same amount of a smelly gas into the room.  One of them releases ammonia, NH3, and the other releases SO2.  NH3 has a pungent odor, and SO2 smells like rotten eggs.  The professor has no idea that this has happened, until she smell the first gas.  Which chemical will the professor smell first?   (NH3 or SO2)                                .  If the professor starts to smell the first gas 42. seconds after the gas is released, how long will it take her to smell the second gas?       sec. * Note: It is unsafe practice to work with these chemicals in an open lab.

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s.com/course.html?courseld%3D15828855&HeplD353706194671Of71a192e43597b01c6e0#10301 Principles of Chemistry I (Chem 1107-327) signments <09 - Pre-Lab 9.11 Pre-Lab Methane burns in oxygen to produce CO2 and H2O. CH:(9) + 202(g)→2H»O(1) +CO2(g) Part A If 0.55 L of gaseous CH, is bumed at STP, what volume of O, is required for complete combustion? Hνα ΑΣφ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining 40 DELL

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Gas Stoichiometry Soenario #3 What mass (in grams) of sodium chloride (NaCl) will be produced when enough sodium (Na) is combined with 2.4 L of chlorine gas (Cl₂) at 25 C and 1.2 atm? Na + Cl₂ ⇒ NaCl 1. Check for a balanced chemical equation. . 2. Check for STP. If it's not balanced, balance it. This is important for mole ratio if you'll need it. R = gas constant 8.31 L kPa/mole * K 0.0821 L* atm/mole * K 3. Are you given liters or grams? PV = nRT If there's not STP (0 C, 1 atm), you'll need to use Ideal Gas Law to find "V" or "n". . If you're given liters, change to moles using the Ideal Gas Law. Once you have moles, you can use mole ratio and molar mass stoichiometry to determine a mass for the product. If you're given grams, change to moles using molar mass and apply a mole ratio to determine "n" for the other chemical. Once you have "n" for the other chemical, you can use the Ideal Gas Law to solve for "V"."

●●● 6 15 16 Keynote File Edit Insert Slide Format Arrange View Play ... 17 18 19 20 21 ✓ View 100% Zoom :0 F1 + Add Slide V View 125% Zoom ► Play + Add Page Keynote Live F2 O 38,742 Table 20 T Insert F3 Share Window Help APR 13 000 000 6 Table GAS LAWS HOMEWORK ASSIGNMENT (You can examine the data on the Student Data Sheets for assistance.) F4 GASES LAB HW (1) ~ GASES LAB Chart . Chart T Text 1.The pressure of a gas is doubled. Assuming that n and T are constant, what should happen to the volume of the gas? T Text 2.The pressure of a gas is doubled. Assuming that n and V are constant, what should happen to the temperature of the gas? Shape 3.The number of moles of gas is doubled. Assuming P and T are constant, what should happen to the volume of the gas? F5 P Media Shape density PA Media Comment F6 MacBook Air ◄◄ Comment F7 No Collaborate Color Fill Appearance Title Body [Slide Number ▾ Background ▶11 4 Collab F8 ● For Sli Edit M

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Write the chemical formulas for the products formed when each of the following hydrocarbons undergoes complete combustion. For each part, there are two answers.  Input one chemical formula in each blank.  Order doesn't matter. Do NOT include equation coefficients, ONLY the two products When typing a compound formula, use an underscore "_" to depict a subscript for example for K2CO3 you would type K_2CO_3 a)  C2H4         b)  C7H8

Kinetics & Equilibrium: Predicting relative forward and reverse rates of a reaction in a dynamic equilibrium.

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Help with these. please show work so I can check with my answers

If the percent yield of the reaction below is 78%, how many grams of chlorine gas are needed to produce 315.0 g of PCI3 Show all work on a separate piece of paper and submit work in part B. Clearly label question # and answer. Failure to show work will result in a zero for this question. P4(s) + 6CI2 eDetA 4PCI3(1) Type your answer...

Union State Cc x Assignments: CHM111 11790- C x O Question 6 - Chapter 4 &13.5 HC X+ https://ezto.mheducation.com/ext/map/index.html?_con%3Dcon&external_browser%3D0&launchUr 5 HOMEWORK #1 Saved 3 attempts left Check my work Enter your answer in the provided box. A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass. What is the molarity of the solution? to search 立

5.00 mol of ammonia are introduced into a 5.00 L reactor vessel in which it partially dissociates at high temperatures.2NH3(g)    3H2(g) + N2(g)At equilibrium and a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction. Hint - divide 5.00 mol of ammonia by 5.00 L to get initial concentration.  Round off the answer to three significant digits. Group of answer choices Kc = 15.3 Kc = 17.3 Kc = 19.3 Kc = 21.3 None of the above

Chemistry For this exercise, you can simulate the described conditions by changing the values in the Run Experiment tool, under the Experiment tab, in the simulation. The hints run through each step in the calculation, where the equations are given before this part. The second hint calculates the temperature change, which is the only step that requires the simulation.   Use the simulator to react 61 mLmL of 1.6 MM HNO3HNO3 with 57 mLmL of 1.8 MM KOHKOH at an initial temperature of 20.00 ∘C∘C; note the final temperature. Use the data from the simulation to calculate the change in enthalpy per mole of product (nn). Estimate the density of the liquid to be 1.00 g/mLg/mL.   Final temp: 31.27 C

Part A) For the reaction below, what volume of oxygen gas reacts with 20.0 mL of hydrogen chloride? (Assume temperature and pressure remain constant)             4HCl(g) +   O2(g)--> 2Cl2(g) + 2H2O(g) A) 20.0 mL B) 10.0 mL C) 5.00 mL D) 40.0 mL E) none of the above Part B)  For an experiment, the decomposition of 1.500 g of baking soda gave 0.300 L of carbon dioxide gas. If the calculated volume of carbon dioxide gas is 0.310 L, what is the percent yield? A) 40.0% B) 96.8% C) 103.3% D) 75.0% E) 20.6% Part C) Based on the limiting reactant concept, how many moles of cobalt(III) oxide are produced from the reaction of 2.00 mol of cobalt and 2.00 mol of oxygen gas?             4 Co(s) + 3 O2(g)-->  2 Co2O3(s) A) 2.00 mol B) 1.33 mol C) 0.50 mol D) 1.00 mol E) none of the above

1) ВНз, THF 2) NaOH, H2O2, H20

A student wants to know how many grams of water are made from 5.00 grams of oxygen gas during the synthesis of water from basidelements. Which step should be substituted for the question marks? 2 Hz+ O2→2 H;0 5.0 g 02 1.0 moles 0, 1 31.998 g 02 18 g H,0 A. 1.0 mole 0, 2.0 mole H,0 B. 1.0 mole 0, 18 g H,0 C. 2.0 mole H,O 2.0 mole 0 D. 2.0 mole H, O