Given the hypothetical thermochemical equation: A + B —> C + D ΔH = - 430 kJ Which among the following statements is correct about this reaction? a. The reaction is endothermic. b. The equation may be written as A + B + 430 kJ C + D c. The heat content of C and D is greater than the heat content of A and B. d. The heat content of A and B is greater than the heat content of C and D

Q: The specific heat capacity of lead is 0.13 J/g°C. How much heat (in J) is required to raise the…

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Q: If 50.0 g of water at 25.0 °C absorbs 14.5 kJ of heat, what is the final temperature of the water?…

A: Given  q = 14.5 kJ = 14500 J C = 4.184 J/g.°C Ti = 25°C Tf = ?

Q: A 6.84 g mass of a metal was heated to 103.61°C and then plunged into 100.0 g of water at 23.08°C.…

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Q: When gasoline burns in a car engine, the heat released causes the products CO2 and H2O to expand,…

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Q: 7.00 Jof heat is added to 10.00g of gold, which is initially at 25°C. The heat capacity of gold is…

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Q: A chemist must add 3,352 kJ of heat to 2 mol solid Al2O3 to cause it to break down to form 4 mol…

A: Given: Heat supplied to solid Al2O3 = 3352kJno of moles of Al2O3 taken  = 2molno of mol of Al formed…

Q: solid, or to measure the energy of a solution phase reaction. A student heats 65.30 grams of gold to…

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Q: In a good calorimeter with a lid, 50.0 gram sample of liquid water at 25.0 °C is mixed with 32.87…

A: a. It gained by cold water b. Heat lost by hot water c. According to law of thermodynamics the total…

Q: A student wants a chemical reaction that will produce the most amount of heat to use for heating…

A: The reactions that produce heat are called exothermic reactions. We will use this to answer the…

Q: An engineering student wants to study the heat transfer between a 50 g of heated block of iron (cFe…

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Q: Consider the following data: When metals A and B are placed in contact with each other, which of the…

A: Answer is Option (B)

Q: A chemist measures the energy change AH during the following reaction: Cl,(g)+H,(g) → 2 HCl(g)…

A: Exothermic reactions are those in which energy is released.

Q: Given the thermochemical equation SO2(g) + 1/2 O2(g) ---> SO (g) ΔH = -99kJ/mol how much heat is…

A: Given :-  SO2(g) + 1/2O2(g) → SO3(g)  ∆H = -99kJ/mol  To calculate :-  amount of heat evolved from…

Q: When a 3.46-g sample of solid sodium nitrate dissolves in 41.5 g of water in a coffee-cup…

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Q: A sample of 24.9 g of ammonium nitrate, NH4N03, was dissolved in 121.3g of water in a coffee cup…

A: Mass of sample (ammonium nitrate) = 24.9 gram Mass of water = 121.3 gram Specific heat of solution =…

Q: 100 g of water at 86 °C is mixed with 200 g of water at 20 °C. What is the final temperature of the…

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Q: Magnesium burns in air to produce a bright light and is often used in fireworks displays. The…

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Q: What mass of natural gas (CH4) must burn to emit 267 kJ of heat?CH4(g) + 2 O2(g) ¡ CO2(g) + 2…

A: It is given that when 1 mole of methane is burned with 2 moles of oxygen to release carbon dioxide…

Q: The energy content of raisin bread is 13.1 kJ/g. Calculate the temperature increase when a slice of…

A: Given data:

Q: Evaporating sweat cools the body because evaporation is an endothermic process:H2O(l)…

A: Evaporation: The process in which liquid convert into vapor or gaseous form is called evaporation.…

Q: The thermochemical equation showing the formation of ammonia (NH3) from its elements is: N2 (g) + 3…

A: a. Lost to the surroundings when one mole of hydrogen is used up in the reaction. b. Absorbed from…

Q: The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine…

A: The balanced reaction taking place is given as, => 2 Na (s) + Cl2 (g) -----> 2 NaCl (s)…

Q: 1. During an experiment, a student added 35 J of heat to a system. At the same time, the environment…

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Q: CaCO3(s) + 2 HCl(aq) –––> CaCl2(aq) + H2O(l) + CO2(g); ∆H° = -15.2 kJ Given the thermochemical…

A: We have to calculate the amount of heat liberated.

Q: A 2.5 g sample of NH4NO3 is dissolved in 135 g of water in a Styrofoam cup, changing the temperature…

A: Data given: Mass of NH4NO3 dissolved = 2.5 g Mass of water = 135 g Initial temperature, T1 = 25.1 °C…

Q: Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ How much heat is…

A: As the masses of both reactants are given, we need to fist find the limiting reactant. From limiting…

Q: 6.00 J of heat is added to 10.00 g of gold, which is initially at 25°C The heat capacity of gold is…

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Q: How many moles of H2 are required to produce -2151 kJ of heat in the following reaction? N2 (g) + 3…

A: The balanced reaction taking place is given as, =>

Q: Consider the following thermochemical reaction for kerosene: 2 C12H26 (1) + 37 O2 (g) 24 CO2 (g) +…

A: The given balanced chemical equation is: 2 C12H26 (l) + 37 O2 (g)→ 24 CO2 (g) + 26 H2O (l)…

Q: 1. The thermochemical equation showing the formation of ammonia, NH, from its elements is Nalg) +…

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Q: 150. g of water (Cs = 4.184 J/g°C) at 20.0 °C is added to a coffee cup calorimeter. A 35.0 g sample…

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Q: 200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The…

A: Concept - Reaction is in between HNO3 and KOH. these both are strong acid and strong base, so the…

Q: A system receives 525 J of heat from its surroundings and delivers 465 J of work to its…

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Q: How much heat energy is required to raise the temperature of 0.366 kg of copper from 23.0 C to 60 C?…

A: The mass of copper is = 0.366 kg The raise in temperature is = 60-23 = 37oC The heat capacity of…

Q: How much heat has to be added to 513 g of copper at 22.3°C to raise the temperature of the copper to…

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Q: A 1.00g sample of octane is burned in a calorimeter that contains 1.20kg of water. The temperature…

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Q: Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ How much heat is…

A: Using the concept of limiting reagent, we can easily find the number of moles of the reaction that…

Q: 9. How much heat will be transferred when 14.9 g of ammonia reacts with excess oxygen according to…

A: Given :- 4NH3 + 5O2 →4NO + 6H2O  ∆H = -1170 kJ  To calculate :-  Amount of heat transferred on…

Q: The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine…

A: The number of moles of any substance can be obtained by dividing the mass by molar mass which may be…

Q: 81. The specific heat capacity of iron is 0.461 J[g x K) and the specific heat capacity of titanium…

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Q: A chemist measures the energy change AH during the following reaction: C,Hg(9)+50,(9) → 3 CO 2(g)+…

A: Answer :-  a) Exothermic  b) Yes, released  c) 1.83 × 103 kJ…

Q: 2) The specific heat capacity of iron is 0.461 J/g K and 0.544 J/g K for titanium. A sample…

A: Given,Specific heat capacity of iron = 0.461J/gK.Specific heat capacity of titanium = 0.544J/gK.Mass…

Q: 11) q of combustion of the food sample equals a) q absorbed by the calorimeter -q absorbed by the…

A: We have given that  11) q of combustion of the food sample equals   a) q absorbed by the calorimeter…

Q: Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the…

A: Given  ∆H0rxn  = -393.5 kJ       | unit of ∆H0rxn = kJ not k  Amount of heat energy produced = 5*102…

Q: One origin of SO3 is the combustion of sulfur, which is present in small quantities in coal. S(s) +…

A: Given the formation of SO3(g) from sulfur, and combustion enthalpy ofsulfur and sulfur dioxide.we…

Q: 2 NO(g) + O2(g) ––––> 2 NO2(g); ∆H° = –114.4 kJ Given the thermochemical equation above, how much…

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Q: When a 0.740-g sample of trinitrotoluene (TNT), C,H,N‚O§, is burned in a bomb calorimeter, the…

A: Mass given = 0.740 g  Heat capacity = 3.35 KJ°C-  Initial Temperature = 23.4 °C  Final temperature =…

Q: An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water…

A: a) Since the metal is losing heat as the temperature of the metal is going down from 99.1 °C to 25.7…

Q: A group of students place 15.41g of a metal into a test tube. They place the test tube into a beaker…

A: Given, mass of the metal = Wmetal = 15.41 g  Mass of the water = Wwater = 10.47 g Initial…