Module Eleven Lesson One Activity

Please correct answer and don't use hand rating

Please provide only typed answer solution no handwritten solution needed allowed

I need help on part C and part D

The internal energy can be increased by ________. (a) transferring heat from the surroundings to the system (b) transferring heat from the system to the surroundings (c) doing work on the system

help  please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

A calorimeter is used to measure the heat absorbed or released in a chemical .1 or physical process by measuring the

INSTRUCTURE Privacy Policy Acceptable Use Policy Facebo DELL Section 8: Endothermic and Exothermic 1. Label the following diagrams as endothermic or exothermic reactions. reactants products AH 0 products Time Time 2. reactions absorb heat and reactions release heat. 3. What happens to the temperature inside a container in which an endothermic reaction is occurring? 4. What happens to the temperature surrounding a container in which an endothermic reaction is occurring? 5. Label the following as endothermic or exothermic. H2 (g) + S (s) Label the following as endothermic or exothermic. a. Vaporization b. Condensation H2S (1) + 86kJ H2 (g) + S (s) - H2S (1) + 86kJ 6. c. Freezing d. Melting

. The _____ must be collected in order to determine the caloric content of food using a bomb calorimeter.     change in water weight the rate at which food burns change in water temperature change in volume of water lost

Peisalla lamacron Nar. ,202 Date Name Section galauvinstenos Pre-Laboratory Assignment 1. Read an authoritative source for a discussion of preparing and interpreting a graph, especially the extrapolation of a curve. 2. A student determined the calorimeter constant of the calorimeter, using the procedure described in this module. The student added 50.00 mL of cold water to 50.00 mL of heated, distilled water in a Styrofoam cup. The initial temperature of the cold water was 21.00 °C and of the hot water, 29.15 °C. The maximum temperature of the mixture was found to be 24.81 °C. Assume the density of water is 1.00 g mL¯1 and the specific heat is 4.184 J g¯K gniwollot bns of toh bine botollon ot ssb om (1) Determine the AT for the hot water and the cold water. mit At cold water = 24.8I- 21,00 = 3.81°COn आनी AT hot = 24.81- 29.15 = - 4.34°C 60.ES 2.0 0LES 8. 0.1 0.0 If 0.8 28.5S Calculate N 0.4 08.TT gabxim 02 4.34°C hot water 81 answer cold water 381°C dogesn boximnu sdt to anuiSTeqmad mom…

Identify two sources of error in this experimentation.

33 - A piece of zinc (Zn) is immersed in aqueous hydrochloric acid solution. According to this which of the followings is wrong?    A) It produces hydrogen gas as the same amount (in moles) of zinc consumed in the reaction.   B) Zinc (Zn) replaces acid hydrogen.  C) Produces hydrogen gas.  D) Zinc piece does not react with acid solution.  E) Initially Zinc (Zn) is zero (0) charged.

PLEASE ANSWER

The question I need help on is in the photo below. Thank you :)

When using a coffee cup calorimeter to determine the specific heat of a metal sample errors can occur in the procedure.  Which of the following procedural errors would lead to a specific heat value being calculated that is lower than the accepted value?  Check all that apply.   When the metal was placed into the coffee cup calorimeter some water splashed out of the cup.         After the metal was heated (to its initial temperature) there was a significant time delay before it was placed into the coffee cup calorimeter.         After the mass of water in the coffee cup calorimeter was measured and recorded some of the water evaporated.         The lid was not placed on the coffee cup calorimeter during the experiment.         The mass of the metal was measured incorrectly. The actual mass of the metal used was greater than what was recorded.         The "final" temperature was read before the metal and water had reached equilibrium         The calorimeter used in…

please .part b!

17

create a poem about endothermic and exothermic reactions with 4 paragraphs and 4 stanzas

Find the heat change of the reaction. CH4 (g) + 2 Cl2 (g) à CCI4 (g) + 2 H2 (g) Substance AHf (kJ/mol) CH4 (g) -74.85 CCI4 (g) -135 Type your answer...

Which of the following statements is/are CORRECT? A system is defined as an object or collection of objects being studied. Surroundings are defined as everything outside of the system being studied. In an endothermic reaction, heat is transferred from the system to the surroundings.   a) 1 only b) 2 only c) 3 only                d) 1 and 2                e) 1, 2, and 3

When substances are dissolved in water, they can absorb or release heat. Describe how you would use a calorimeter to determine the amount of heat required or released to when 10 grams of sugar is dissolved in 100 grams of water. Describe how you would calculate the heat absorbed or released by the sugar with the data you collect. (Do no perform any calculations.)

I Review | Constants | Periodic Table Calorimetry is a method used to measure enthalpy, or heat, changes that occur during chemical processes. Two common calorimeters are constant-pressure calorimeters and constant-volume (or "bomb") Part A calorimeters. A simple constant-pressure calorimeter can be made from a foam coffee cup and a thermometer; energy changes in a reaction are observed via a temperature change of the solution in the cup. Bomb calorimeters are used to measure combustion and other gas- producing reactions, where the reaction is observed in a strong, sealed vessel. The idea behind calorimeters is that if they are sufficiently insulated from the outside environment, any energy gained or lost in the chemical reaction will be directly observable as a temperature and/or pressure change in the calorimeter. A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 174 g of solution. The reaction caused the temperature of…

Endothermic Reactions vs. Exothermic Reactions Worksheet Process System Exo Endo Explanation 1. An ice cube melts after being left out on the table. 2. Cooking an egg in a frying pan. 3. Burning a match. 4. Dynamite explodes in the destruction of a building. 5. Making ice cubes. 6. A puddle of water evaporates. 7. Plants making sugar through photosynthesis acer

TEXT ANSWER Question 13 A calorimeter holds 45 g water at 22.0°C. A sample of hot iron is added to the water, and the final temperature of the water and iron is 28.0°C. What is the change in enthalpy asso- ciated with the change in the water's temperature? J Note: The specific heat of water is 4.18 g°C. Use the formula AH = -cmAT Show your work. Normal ÷ A A √x Enter your answer here 中山 2 Tx BIUS X ||| |||