A 12.8 g piece of aluminum (which has a molar heat capacity of 24.03 j/°c·mol) is heated to 82.4°c and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 j/g°c) initially at 22.3°c. the final temperature of the water is 25.7°c. ignoring significant figures, calculate the mass of water in the calorimeter.

ssolvedc. all of the KC1O3 is dissolved d. none of the KC1O3 is dissolved​

weighs 4.010-g. Calculate the percent by mass of CaCl2 in the original mixture.

na at this temperature. You may assume the volume of the solution doesn't change as the O is dissolved.

r. In the laboratory a general chemistry student finds that when 5.15 g of NH4Br(s) are dissolved in 105.00 g of water, the temperature of the solution drops from 23.82 to 21.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.76 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Br(s) in kJ/mol.

hat melts at 180 oC . If the tank is heated, what is the maximum pressure that will be attained in the tank before the plug melts and releases gas?

atm to 101 kPa. A. Volume increases by 200% B. Volume decreases to 50% of its original value C. Volume decreases by 100% D. Volume increases by 100% E. Volume does not change

ance. If the sample is paramagnetic, the mass reading of the balance will increase when the field is switched on. Based on their electron configurations, predict whether these elements are paramagnetic or diamagnetic. a. Paramagnetic b. Diagmagnetic

hat forms; (c) the composition and amount of each phase present at 728°C; (d) the composition and amount of each phase present at 726°C; and (e) the composition and amount of each microconstituent present at 726°C

ne of the fuels. Which fuel will emit the least amount of CO2? 1. Calculate the number of grams needed of each fuel: 2. Calculate the number of moles of each fuel: 3. Write down the balanced chemical equation for the combustion of the fuels: 4. Calculate the number of moles of CO2 produced by burning each fuel to produce 1.000 x 103 kJ. Which fuel will emit the least amount of CO2?

stilled water is added until the total volume of solution is 250 ml portion of the diluted solution is measured out with a pipet and titrated with a standard solution of sodium hydroxide. The neutralization reaction is as follows: HC2H3O2 (aq) + OH- (aq) --> C2H3O2- (aq) + H2O (l)It is found that 16.7 mL of 0.0500 M NaOH is needed to titrate 25.0 mL of the diluted vinegar. Calculate the molarity of the diluted vinegar.