How much energy is needed to boil water? How much energy would it take to boil 1 liter of water?
To calculate this you have to use the specific heat capacity of water which is 4.184J/gram/Celsius. So if you start from room temperature of 21C, and make it to 100C, the boiling point of water, then the temperature change is 79C. The energy needed E=SH times change in temperature times the total mass in grams(Which is 1000gram for a liter of water). That gives you 4.184•79•1000 which is 330,536J, or 330.54KJ. Kaiser T, MD.
At 1,000 degrees Celsius, the pressure of oxygen gas from the decomposition of copper (II) OXIDE (CuO) is?
At 1,000 degrees Celsius, the pressure of oxygen gas from the decomposition of copper (II) OXIDE (CuO) is 2.5 atm: 4CuO (s) <---> 2Cu2O (s) + O2 (g) The calculated fraction of CuO that will decompose if 1.26 mole of it is placed in a 6.0 L flask at 1,000 degrees Celsius is: PLEASE SHOW ALL OF YOUR WORK!! A. 0.234 B. 0.345 C. 0.456 D. 0.543 E. 0.634
Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water?
delta t = m x Kf x i i = 1 with 1 particle in solution molar mass of C2H6O2 = 62.068 g / mole so we have 500 / 62.068 moles of solute = 8.06 moles these are in 500 g of water so moles / kg of water = 16.11 moles / Kg = m so delta t = 16.11 x 0.512 x 1 = 8.25 oC the solution boils at 108 oC
How much current is needed to produce 300 Celsius heat in copper wire?
With the information given, the answer is indeterminable.Firstly, 300 Celsius is not heat; it is simply temperature. Heat needs to be defined as a unit of work or energy as explained further below.Secondly, you also need to specify the size and quantity of the copper wire to be heated , as well as its current temperature.Heat is measured in units of work, typically Joules or calories. One calorie is the quantity of heat required to raise the temperature of 1 gram of water by 1 degree Celsius.In an electrical conductor, like copper, heat results from the conversion of electrical energy (current relative to electrical resistance) to heat energy (Joules or calories) as a result of movement of electrons in the conductor. This conversion of electrical energy to heat is defined by Joule's first law, a function of the current and electrical resistance in the conductor, basically a product of the square of the current in amperes and the resistance of the conductor.The heat produced from conversion of electron motion can be calculated knowing the Current and Resistance of the conductor. To determine the change in temperature , the mass (derived from quantity)of the conductor material is needed, as well as the time that current is flowing. The reference below describes Joule Heating and shows this calculation rather simply.Joule Heating Joule heating is the basis of electric resistance welding, sometimes known as spot welding or seam welding used extensively in industry to join metals. James Prescott Joule
If 10 g of ice at - 10° C is added to 50 g of water at 15° C, what is the temperature of the mixture?
You need to understand 3 concepts to solve this answer.Firstly, You have to use the principle of calorimetry (measuring heat content of a system) to get the answer for this question.The principle goes like this:heat gained by a system(ice) = heat given by a system (water).That means the heat absorbed by ice will be equal to the heat given by the water.Secondly,now since you know the principle, next step is to know the formula of heat given or taken, that isQ= m*c*(t2-t1)where,m=mass of the substancec=heat capacity of substance (ice=2.1kJ/kgK, water=4.2kJ/kgK)t2-t1=change in temperature of the substanceNow the last but not the least concept, you must know what is latent heat, you see while there is a change of state that is when solid converts to liquid or liquid to water there is no change in temperature with the absorption of heat and that value for ice to water is 336kJ/kg.So this is the process is which is gonna happen, as the ice comes in contact with water, its temperature will rise upto 0 deg celsius. At that temperature which is the melting point of ice, it converts into water without any change in temperature. After complete conversion it again absorbs heat to reach a state where the converted ice and the water are at same temperatures (thermal equillibrium).So your final formula would be:Heat given by water = heat absorbed by ice + latent heat + heat absorbed by water (melted ice)mw*cw*(tw-T) = mice*cice*(tice-0) +336 +mmw*cmw*(T-0)The only unknown here is T =mixture temperature.Hope you got the science. :)
How much energy does it take to raise the temperature of an average room by 10 degrees?
Assuming you want to only increase the temperature of the 'air' in the room (and not the walls and other things), the calculation will use the specific heat capacity of air, the mass of air and the temperature difference to arrive at the amount of energy needed.Assuming the height of the room is about 10 ft tall, the total volume of the room is 10 x 300 = 3000 cu.ft.Amount of energy needed to raise temperature is given by the formula: specific heat capacity of substance x mass of substance x temperature difference1. Specific heat capacity of air is 1.006 kJ/kgC2. mass of air: density of air is 0.036 kg/cu.ft. mass = density x volume = 0.037 x 3000 = 111KG3. Temperature differential = 70C - 60C = 10Cenergy needed = 1.006 x 111 x 10 = 1116 KJPower is energy transferred / second. That means, your 1000W space heater can transfer 1000J of energy / second. So time taken to heat up this space will be:1116000 / 1000 = 1116 seconds. In other words: 18.6 minutes.This of course assumes that the output power of your heater is 1000W. If the 'input' is 1000W, you may want to find out the efficiency of your heater and then arrive at the actual output power of the heater by the formula output power = input power x efficiency.
A perfect gas at 27°C is heated at constant pressure till its volume is doubled. What will be its final temperature?
According to ideal gas equation PV=nRTP=pressure of gas,V=volume of gas=volume of container,T=temperaturueV1 =INITIAL VOLUME ,V2 =FINAL VOLUMET1 =INITIAL TEMPERATURE =27+273=300T2 =FINAL TEMPERATUREAccording to question,V2 =2 x V1Therefore,V1/V2 = T1/T2V1/2V1=300/T2T2 =FINAL TEMPERATURE=600KVidyanchal Academythank you
A gas expands from 2 liters to 6 liters against a constant pressure of 0.5 ATM on absorbing 200J of heat. What is change in internal energy?
ΔH = ΔU + PΔV... (Definition of Enthalpy change)At constant pressure (for isobaric process)ΔH = q….Hence, ΔU = q - PΔV (1st law of thermodynamics)ΔU = 200 - 0.5*101325 *(0.006–0.002)ΔU = -2.65 JAll the sign conventions were considered and pressure and volume were converted to their respective SI units.1 atm pressure = 101325 Pa1 liter volume = 0.001 cubic m.
540 g of ice at 0°C is mixed with 540 g of water at 80°C. What is the final temperature of the mixture?
Ice at 0°C has a total latent heat ofQ=m*L = 540*80 = 43200 cal.Now for water to come at 0°C and it's state to remain as water, we need to remove heat from it which is given by,Q= m*Cp*(∆T) = 540* 1* 80 = 43200 cal.So, we can see thatHeat released by water to reach from 80°C to 0°C = heat required by ice to melt into water at 0°C.So, the ice will melt to water and it's temperature will be 0°C.Hence, the final state would be water at 0°C.So, the answer is A.Hope this help you.Thanks.