The heat from a candy bar's Calories can raise the temperature of a 4.50 kg bucket of water from 4°C to 68°C. How many Calories are in the candy bar?
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- The heat capacity (Cp) 0f an hal0genated 0rganic c0p0und, chl0r0f0rm is given by the f0ll0w equati0n. Equati0n (1) Cp (J/mol K) = 19.8 +0.22 T – 0.00026 T2 (a) 0btain a new equati0n that uses T in Fahrenheit (b) Calculate the Cp 0f chl0r0f0rm at 300 K using Equation (1) (c) Calculate the Cp 0f chl0r0f0rm at 80 F using the equati0n you derived in (a)5.33 What is the difference between specific heat and heatcapacity? What are the units for these two quantities?Which is the intensive property and which is theextensive property?You are camping and need to cook all your food using your camp stove which runs off of propane.If you wanted to warm up your giant mug (67.628 fluid ounces) of morning coffee from 10°C to 80°C,what mass of propane would you have to use?The ΔHcomb for propane is -2219.2 kJ/mol, the density of coffee is 1.0002 g/mL, and the specific heatcapacity of coffee is equal to that of water.1 fluid ounce = 0.0295735 L
- calculate the heat gained by the water: Q=CmΔT heat lost by sample: ms* cs *(Ts-T) = mw *cw (T -Tcw) + mc *cc *(T-Tcw) solve for the specific heat of the unknown known unknown (ms) mass of unknown= 240.40g (Cs) specific heat of sample: ? (Ts) Temp initial of sample: assume 100°C (mc) mass of dry cup: 31.3g (mw) mass of water: 127.3g (cw) specific heat of water: 4186 J/kg °C (Tcw) initial temp of water: 12°C (Cc) specific heat of cup: use Aluminium 900 J/kg °C (T) final temp 23°C (I tried it and I'm not sure if I have a correct answer, so if you can please do it step by step to show me where I made mistakes)Calculations for the Specidfic Heat for an Unknown Metal Trial 1 Trial 2 Mass of unknown metal(g) 18.371 18.371 Mass of calorimeter cup(g) 1.891 1.891 mass of calorimeter and water(g) 47.231 46.502 Tempature of boiling water bath (C) 98.50 99.2 Initial tempature of calorimeter water(C) 23.5 23.4 Final Tempature of water and metal(C) 24.8 24.8 Mass of water(g) Tempature change of water(C) (Do not include a negative sign) Heat gained by water (cal) (do not include negative sign) heat lost by metal(cal) (do not include negative sign) tempatire change of metal(C) (do not include negative sign) Specific heat of metal [cal/g. C] Specific heat of metal [J/(g. C)] Average specific heat of metal [J/(g·°C)] Identify the Metal based on the average specific heat in J/(g·°C)The gas inside a cylinder expands against a constant external pressure of 1.00 atm from a volume of 5.00 L to a volume of 13.00 L. In doing so, it turns a paddle immersed in 1.00 L water. Calculate the temperature increase of the water, assuming no loss of heat to the surroundings or frictional losses in the mechanism. Take the density of water to be 1.00 g cm-3 and its specific heat to be 4.18 J K-1g-1.
- Determine the structures of the molecules described in the following problems. Also note, in the combustion of N containing compounds, N2(g) is made. 7. Recognizing that the binding of a particular protein to DNA is an exothermic reaction at 310K, with DH= -300 kJ/mol, How many protein molecules will need to bind (react) to change the temperature of an coli cell to 315K. (Assume that the cell is full of pure water, heat capacity is 1cal/g, density 1g/ml, and the volume of the cell is a femtoliter). Does this seem likely? (The most abundant proteins have about 70,000 copies per cell. )which version of the specific heat equation is both correct and is set up to solve for the final temp?In a calorimetry 0.100 moles of NH4NO3(s) disolved in water. when the temperature decreeses 5.8 degrees celsius, and mass = 108g what is the molar entalphy change of solution? Specific heat capacity is same as water = 4.184 Jg-1K-1. Answer the question with errorslimits when the uncerainty of the temperature is 0.1 degrees celsius.
- Write the equation for the complete combustion of octane. If the heat of combustion of octane is -5294 kJ/mol, determine how many kJ of energy could be obtained from the combustion of one gallon of gasoline (assume the density is 703 kg/m3. Show ALL workUsing the data below, calculate ∆Hrxn for: HCl(aq) + NH3(aq) ® NH4Cl(aq) The reaction of 50.0 mL of 1.00 M HCl with 50.0 mL of 1.00 M NH3 causes a temperature rise of 6.4 ̊C in the resulting 100.0 mL of solution. The NH4Cl solution has density 1.005 g/mL and specific heat capacity 3.97 J/g ̊C. Pay careful attention to sig figs in this problem.In constant pressure calorimeter 75.0 ml is mixed with 1.25 M Hydrocloric acid solution is mixed with 75.0 ml of 1.25 M Sodium hydroxide solution. the density of the final solution is 1.00g/ml and the the solution both initially 21.45c, reach a maximum temperature of 28.32c when mixed. based on this information, and estimating the solution's heat capacity as 4.18Jg-1c-1, what is the amount of heat in Kilojoules, transferred in this reaction?