5765J is needed to raise the temperature of 50.0 g of an unknown substance from 25°C to its melting point at 327 C? What is the identity of the unknown substance? Substance Specific Heat (c) Lead 0.128 Iron 0.448 Glass 0.837 Ice 2.090

Q: Calculate the amount of heat (in kJ) required to raise the temperature of 1.65 lb of water from 294K…

A: Given : Initial temperature =  294K Final temperature =  303K Mass of water = 1.65lb

Q: A 110.0-g sample of a gray-colored, unknown, pure metal was heated to 92.0 oC and put into a…

A: Assuming specific heat of metal is C. Since all the heat released by metal in reaching the final…

Q: A 125 gram piece of metal is heated to 288°C and dropped into 85.0 grams of water at 26.0°C.  If the…

A: We have 125 g of metal of temperature 288°C, 85 g of water at 26°C , both have final temperature as…

Q: A 12.3 g chunk of metal is heated up to 95°C and  dropped into an insulated vessel containing 157 g…

A: The question is based on the concept of law of conservation of energy . whatever heat lost by the…

Q: If the specific heat of methanol is 2.51 J/K-g, how many joules are necessary to raise the…

A:

Q: Which sample will reach the lowest final temperature when all samples evolve 12.5 J of heat and all…

A: Since, Q =m.c.St WHERE Q = heat energy M =mass of metal C= specific heat of metal Triangle T =…

Q: A 28.3-g piece of iron initially at 84.4 °C is submerged into 107.2 g of water at 12.2 °C. What is…

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Q: A beaker contained 76.4 g of water at 18.97°C. A 85.48-g sample of metal at 51.36°C was placed in…

A: Given that Mass of water = 76.4 g Mass of metal = 85.48 g Initial temperature of water = 18.97°C…

Q: How many milliliters of water at 21 °C with a density of 1.00 g/mL must be mixed with 220 mL of…

A:

Q: A glass containing 200. g of H2O at 20°C was placed in a refrigerator. The water loses 11.7 kJ as it…

A: Specific heat capacity - Amount of heat required to raise temprature by 1 degree of one gram…

Q: t takes 52.0 J to raise the temperature of an 9.00 g piece of unknown metal from 13.0∘C to 25.0 ∘C.…

A: According to the question we have, The heat required to raise the temperature of the metal is given…

Q: The specific heat capacities of copper, gold, and cobalt are given. Based on this information, which…

A: Specific heat capacity means the amount of heat required to raise the temperature of 1 gram of a…

Q: Macmillan The temperature of a sample of iron increased by 23.7 °C when 261 J of heat was applied.…

A: Amount of heat,Q required to raise the temperature of a substance of mass ,m and specific heat…

Q: Calculate amount of heat (in kJ) required to raise the temperature of a 79.0 g of a substance by…

A: The solution is as follows:

Q: Substance Specific Heat, c (J/g×°C) Water 4.184 Granite 0.803 Mercury 0.140 Silver 0.235 Aluminum…

A: Heat given by Aluminum = heat taken by water

Q: A 31.1 g wafer of pure gold at 69.3 is submerged into 64.2 g of water at 27.8 in an insulated…

A: given: mass of gold = 31.3 g initial temperature of gold = 69.3oC mass of water = 64.2 g initial…

Q: The temperature of a sample of silver increased by 23.4 °C when 273 J of heat was applied. Substance…

A: Given: Increase in temperature, ∆T = 23.4°C Heat given, q = 273 J Specific heat for silver = 0.235…

Q: neat re

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Q: A 127 gg piece of metal is heated to 2.80×102 ∘C∘C and dropped into 83.5 gg of water at 26.0 ∘C∘C.…

A: In case of mixing hot metal with water, the heat lost by metal is equal to the heat gain by the…

Q: A beaker contained 66.1 g of water at 11.36°C. A 81.45-g sample of metal at 59.04°C was placed in…

A:

Q: The temperature of a sample of iron increased by 23.7 when 261 J of heat was applied. What is the…

A: Given :- change in temperature "∆T" = 23.7°C amount of heat absorbed "q" = 261 J specific heat for…

Q: A piece of metal weighing 71.35 g was heated to 96.6oC and then put into 42.95 g of water (initially…

A: The heat released or absorbed (q) when the temperature of any substance is raised is calculated as:…

Q: Calculate the amount of heat (in KJ) required to raise the temperature of a 86.0g sample of ethanol…

A:

Q: A 20.33 g sample of a substance is initially at 28.5 °C. After absorbing 2325 J of heat, the…

A: • The values provided in the question are:-  i) Mass of a substance, m = 20.33 g  ii) Initial…

Q: A 50 gram sample of iron (with a heat capacity of 0.450 J/g ºC) is heated to 100.0 ºC. It is then…

A: Answer :-  Heat absorbed by the calorimeter = 1111 J…

Q: 2.33 g of methane (CH4) is burned in a bomb calorimeter (heat capacity =2.677 ×104   J/°C), 2.33 g…

A: The objective of this question is to find the final temperature reached by the calorimeter when 2.33…

Q: The amount of energy needed to heat 2.00 g mercury from 50.0°C to 85°C is 9.87 J. The specific heat…

A: Given: Mass of mercury=2.00 g Temperature change, ∆T=(85-50.0)°C=35 °C Heat needed q =9.87 J…

Q: Calculate the heat required to increase the temperature of 581 grams of water from 22°C to 90°C? The…

A:

Q: A 0.334-g sample of naphthalene (C₁0Hg) is burned in a bomb calorimeter and the temperature…

A: we have to calculate the heat of combustion for burning 0.334 g naphthalene

Q: A 46.78 g sample of a substance is initially at 26.6 °C. After absorbing 2893 J of heat, the…

A:

Q: The temperature of a sample of copper increased by 24.7 °C when 257 J of heat was applied. What is…

A: • The values provided in the question are:-  i) Temperature change of a sample of copper, ∆T = 24.7…

Q: A 51.74 g sample of a substance is initially at 25.6 °C. After absorbing 2939 J of heat, the…

A:

Q: It takes 55.0 JJ to raise the temperature of an 9.60 gg piece of unknown metal from 13.0∘C∘C to 24.4…

A:

Q: A beaker contained 69.68 g of water at 15.25°C. A 81.2-g sample of metal at 52.22°C was placed in…

A: Given that : The mass of water (mw)= 69.68 g Temperature of water = 15.25°C The mass of sample (mm)…

Q: beaker contained 69.68 g of water at 15.25°C. A 81.2-g sample of metal at 52.22°C was placed in it,…

A:

Q: When a 43.0 g sample of metal at 100.0 oC is added to 38.0 g of water at 23.72 oC, the final…

A:

Q: Determine the final temperature of a gold nugget (mass = 376 g) that starts at 288 K and loses 4.85…

A: Specific Heat Capacity of gold is =0.128 J/gc Initial temperature = T1 = 288K…

Q: Determine the final temperature of a gold nugget (mass = 376 g) that starts at 288 K and loses 4.85…

A:

Q: A sample of lead is heated and placed in a 151.0 g container of water at 22.0 oC.  The final…

A: The heat released by the sample of lead is equal to the heat required to raise the temperature of…

Q: Samples of three metals are prepared: potassium, silver, and rubidium. All of the samples have the…

A: It is given that potassium, rubidium and silver are dropped in a coffee cup calorimeter and need to…

Q: The temperature of a sample of silver increased by 22.9 °C when 255 J of heat was applied. Substance…

A:

Q: Calculate the amount of heat (in J) required to raise the temperature of 38 g of iron from 26°C to…

A: q = mc∆T  q is the amount of heat energy required  m is the mass of substance  c is the specific…

Q: A piece of iron (mass = 25.0 g) at 368 K is placed in a styrofoam coffee cup containing 25.0 ml of…

A:

Q: A piece of metal with a mass of 59.047 g was heated to 98.0°C and then put into 100.0g of water…

A: Given: Mass of the metal = 59.047 g The initial temperature of the metal = 98.0 oC The mass of water…

Q: The temperature of a sample of aluminum increased by 23.5 °C when 257 J of heat was applied. What is…

A:

Q: Which statement best defines specific heat? The amount of heat required to increase the temperature…

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Q: A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is…

A: A hot piece of silver is submerged into cold water, as a result heat will flow from hot silver to…

Q: For the chemical reaction H₂ (g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol. What is the enthalpy for…

A:

Q: It takes 55.0 JJ to raise the temperature of an 11.9 gg piece of unknown metal from 13.0∘C∘C to 24.3…

A:

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates). 

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.