Module 6 Unit 2 Assignment D

P4(9) + 6CI2(g) → 4PCI3(g) 8.02 L of P4(g) is mixed with 10.4 L of Cl2(g) and reacts with 100% yield. What volume of PCI3(g) is produced? Assume all gases are at the same temperature and pressure. 2.60 L 32.1 L O 15.6 L O 2.01 L 6.93 L

Balance the following reactions that occur among volcanic gases. 1st attempt Part 1 (1 point) Χ X₁ He δ. SO2(g) + O2(g) — SO3(g) I Part 2 (1 point) X X₁ "He δ. H₂S(g) + 02(g) SO2(g) + H₂O(g) Part 3 (1 point)

2 H2 (g) + O2 (g) -> 2 H2O (g) a. How many moles of water are produced if 32.8 L are collected?  b. If 72.56 g of oxygen reacts, what volume of water will this produce?

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Suppose we performed Lab 1 examining two different metals: A and B. Metal B has a larger molar mass than Metal A. For both metals, 1 mole of the metal produces 1 mole of hydrogen gas. If the same mass of metal was used in the experiment, how would the volume of hydrogen gas produced be different between the 2 metals? (Each metal was reacted separately) Select one: O Metal A would produce a larger volume of hydrogen gas O Metal B would produce a larger volume of hydrogen gas O Both metals would produce the same volume of hydrogen gas

One day in lab, while taking apart a complicated distillation apparatus, your friend Lisa (an expert chemist) says this: "Group 2A metal hydrides react with water to produce hydroxides and hydrogen gas." Using Lisa's statement, and what you already know about chemistry, predict the products of the following reaction. Be sure your chemical equation is balanced! BaH₂(s) + H₂O(1)→

A sample of gas mixture from a neon sign contains 3.48 x 10-4 mol Ne and 1.12 x 10- mol Kr. What are the mass percentages of Ne and Kr in the gas mixture? Mass percentages of Ne = % Mass percentages of Kr = %3D

1. Give at least 2 significant examples of chemical reactions that falls on change in intrinsic properties and production of light. 2. Enumerate chemical reaction that may bring benefit or harm to life as well as to environment. Give 1 example for beneficial and 1 for harmful 3. Given the statements, write the chemical equation and label the reactant and product a. Aluminum (Al) reacts to oxygen (O2) to form Aluminum oxide (Al2O3). b. The reaction of sulfuric acid (H2SO4) and sodium hydroxide to produce sodium sulfate (Na2SO4) and water

i need the answer quickly

Use the sample experimental data to calculate the mass of sample (BaCl2•xH2O) Mass of pan 15.110 g Mass of pan+ sample before heating 17.452 g Mass of pan+ sample after heating 17.107 g

Please answer question 8 parts A and B

<7 of 11 Metal Ca Fe Cu Mg A B с assroom.collegeboard.org D Observations All the calcium reacted in less than 30 seconds. There was a vigorous production of a gas. ©*** Most of the iron reacted very slowly. There was a slow production of a gas. Some of the iron never totally reacted. No visible reaction. A student puts samples of four different metals of equal mass into HCl(aq) and records observations in the table. Which of the following ranks the metals from least reactive to most reactive? Ca Fe Cu < Mg of the magnesium reacted in about three minutes. There was a moderate production of a gas. Ca < Mg < Fe < Cu 43% 10:50 Cu Fe < Mg < Ca :D Cu Ca Mg < Fe Submit : ||| f(x) H 8

Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction: __CaF2 + __ H2SO4 → __CaSO4 + __ HF. In one batch, 500 g of CaF2 was made to react with 250 g of H2SO4 . Atomic weights: Ca=40, F=19, H=1, S=32, O=16 How many grams of CaF2 can be produced from 250 g of H2SO4 (final answers should be in 3 significant figures)?

What is the mass of 0.5 mole of nitrogen gas? O 1.20 x 1023 g O 28.0 g O 14.0 g O 6.02 x 1023 g O 3.01 x 1023 g

What is an extensive property? What is an extensive property of oxygen?

1. Give reasons why the helium atom is smaller than the cesium atom. 2. A student got a problem wrong.  They were asked, “How many grams of MgCl2 (molar mass = 95.21 g/mol) are needed to make 3.16 L of a 0.500 M MgCl2 solution?”  The correct answer is 150. but the student got 1.58.  What mistake did the student make? 3. To solve the following problem what is the reason you must subtract the vapor pressure of water, 24 torr, from the total pressure, 747 torr in order to solve the problem? “A 500.0-mL sample of H2 gas is collected over water at 298 K and 747 torr.  What volume would the dry H2 gas occupy at STP?  (Given: the vapor pressure of water at 298K is 24 torr).” By the way, the answer is .436 liters. NOTE:  I am not asking you to solve this problem.  I am asking the reason for subtracting the vapor pressure.  If you simply solve the problem, you will get no points.

In 2001, about 54. million tons of sulfuric acid was produced in the United States. Calculate the amount of sulfur (in grams and moles) used to produce that amount of sulfuric acid. Round each of your answers to 2 significant digits. Note: Reference the Conversion factors for non-SI units table for additional information. Part: 0 / 2 Part 1 of 2 I mol × 5 00 ob Ar