Chapter 7a D2L Homework

3379 Which of the following Homeowners policies provides coverage for damage caused to a roof by the weight of accumulated ice and snow? a. HO-0 Form b. HO-1 Form c. HO-2 Form d. HO-4 Form

Direction: Given the picture below answer the guide questions Stage light effects as dry ice sublimes Guide Questions 1. How can this effect be achieved using CO2 or dry ice? 2. What does LPG stand for? How can a gas be liquefied? 3. What conditions are needed to convert a gas into a liquid?

Question 36 286 L of hydrogen gas at STP reacts with excess chorine gas according to the following balanced chemical equation: H2(g) + Cl2(g) –→2HCI(g). Assume ideal gas conditions. What is the maximum amount of gas product that can be formed at STP? (Hint: One-step calculation only.) O 572 L O 286 L O 143 L O 858 L

1) Using the formulas in this lab module for various shapes, calculate the volume of a solid ball made of concrete whose radius from core to outward point is 45mm. Show all work. smulov sr heqxe how lle won2 lig

Based on the kinetic molecular model, solids usually have higher densities compare two liquids. However, ice , a solid form of H2O floats on liquid water which means ice is less dense than water. What do you think is the reason for this phenomenon? What is the biological significance of this concept?

Safari 7:34 AM Sun Oct 1 Patterns in Natur...ule 3 assignment 2 Home LE Calibri Bold Italic (E Patterns in Nature Module 3 Assignment 1. Why is glass not a mineral? Insert Draw Layout Review View References BI ●●● U aA 2. Describe several ways in which minerals can form. Directions: Answer each question as thoroughly as possible. Please make sure all of your answers are in your own words. 3. Name two different patterns of crystal growth. Define each one. ili 4. What is a geode? Which type of crystal growth do geodes exhibit? ㅁㅇ =✓ 5. If a mineral is very hard, which type of chemical bonds would that mineral most likely have in its atomic structure, and why? A 19% 0 :

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Consider this list of substances: H2O, Ni, KI, CH4. Match these substances with the properties below.   Question 9 options:     Conducts electricity as a solution in water     Consists of a molecule with a tetrahedral electron pair geometry     Conducts electricity in the solid state     Can undergo hydrogen bonding with water   .   H2O .   Ni .   KI .   CH4

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Potassium reacts with water to release hydrogen gas according to the following equation 2K(s) + 2H2O(L) > 2KOH(aq) + H2(g) What mass of potassium is needed to produce 50 L of H2 at SATP a. 158 g b. 79 g c. 316 g d. 950 g

A substance has a low melting point. It does not conduct electricity either when melted or in the solid. It is most likely: 1. Chlorine (Cl₂) 2. Diamond (C) 3. Copper (Cu) 4. Calcium oxide (CaO) 5. Graphite (C) 02 O O لا 4 5 0 1

1. When a chunk of dry ice (solid carbon dioxide) is placed out in the air, the solid gradually disappears and a gas is formed above the solid. Does it go through chemical or physical change has occurred? Explain. 2. When the molecules of the solid CO2 becomes free upon exposure to the air. What happened to the bonds of the molecule?

KINDLY WRITE IN GOOD PENMANSHIP PLEASE BECAUSE SOMETIMES I CAN'T UNDERSTAND THE WRITINGS.  CHEMISTRY OF METALS IS THE TOPIC ACT G-1

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28 °C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28 °C is 28.3 mmHg.     5.0 x 1022     5.2 x 1022     3.8 x 1025     5.4 x 1023     3.8 x 1023

What is the melting point of the substance modeled by this heating curve? F. 150 135 120 E 105 90 75 В C 60 45 30A 15 Heat (kJ) Temp. (°C)

A hypothetical element, Le, has a body centered cubic structure with a density of 6.57 g/cm3. Calculate its atomic radius in pm. Atomic Mass: Le: 55.334 g/mol Round your answer to 2 decimal places. Add your answer

(Record your answer with rounded answer to proper significant digits and the proper units.) 1.How many moles of butane (C4H10(g)) were combusted in the presence of excess oxygen gas if 55.8 L of water vapour at STP is collected?Hint: Write a balanced chemical reaction equation first. 2.One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur. 16H2S(g)+8SO2(g)----->16H2O(g)+3S8(s)  8.75 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur dioxide. Calculate the mass, in kg, of sulfur produced.

Aspirin has a higher molar mass compared to salicylic acid, however aspirin melts at a lower temperature than salicylic acid. Provide a brief explanation for this observation. Table 1 Compound: Formula: Salicylic Acid C;H6O3 Aspirin C9H3O4 Molar Mass: 138.12 Melting point: Ka 158-160°C 1.08 x 10³ 180.15 140-142°C 2.72 x 10$ pKa Solubility (g/100ML) 2.99 4.57 0.18 0.25

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Consider the melting points of the substances below (see figures for two compounds). Explain the trend in melting point using your knowledge of intermolecular forces. (In the structures below, carbon is black, hydrogen is white, and oxygen is red.) Substance Melting Point (°C) Molar Mass (g/mol) Cl2 −102 71 Ethyl formate (CH3CH2OCHO) −80 74 Propionic acid (CH3CH2COOH) −20 74 Br2 −7.2 160

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