An ice cube of mass 9.0 \(\rm g}\) at temperature 0\(^\circ CI) is added to a cup of coffee, whose temperature is 85 \({\rm Acirc C}\) and which contains 110 {\rm g}) of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0N {\m(kJ}}}{{\m{mol}}}), Part A Find the temperature of the coffee after the ice melts. Express your answer using two significant figures. AM) = circ (\rm CH

12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. calorimeter itself.)

Calcium acetate, Ca(CH3COO)2 has a molar mass of 158.17 g/mol. In a constant pressure calorimeter, 44.2 g of Ca(CH3COO)2 is dissolved in 861g of water at 25.00 °C. The heat produced by the solution was determined to be 15kJ. What is the final temperature of the solution? q= - msAT SH20 = 4.184 29.0 °C O 18.4 °C O 64.6 °C O 33.8 °C O 3.96 °C O 21.0 °C

Which of the following reactions occuring at 25° C defines the standard enthalpy of formation (TriangleHf) of liquid water? - 2 H (g) + O (g) -> H2O (l) - H2O(g) + O (g) -> H2O (l) - H2 (g) + ½O2 (g) -> H2O (l) - 2 H2 (g) + O2 (g) -> 2 H2O (l)

The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = au

Hw.77.

15 g of solid MgCl2 is mixed with 30 g of water in a calorimeter that absorbs no heat. Which equation calculates the temperature change?   Question 16 options:   (15 g / 53.49 g mol–1 × –159850 J mol–1)  / (30 g × 4.184 J g–1 °C–1)    (15 g / 53.49 g mol–1 × 159850 J mol–1)  / (30 g × 4.184 J g–1 °C–1)   –(15 g / 53.49 g mol–1 × –159850 J mol–1)  / (45 g × 4.184 J g–1 °C–1)

What is the specific heat capacity of a substance of mass 159.5 g that increases in temperature from 22.2 °C to 25.2 °C after absorbing 1.15 kJ of energy in the form of heat? Express your answer in J g-1 °C-1. Do not try to identify the substance.

The enthalpy of combustion of methane gas, CH4(g), is about -9.0*102 kJ/mol. When methanegas reacts with O2(g), the products are carbon dioxide CO2(g) and water H2O(l). How much heatis released during the combustion of methane gas when 4.0 mols of O2(g) are consumed. Express your answer in kJ.A. 3.0*102 kJB. 6.0*102 kJC. 9.0*102 kJD. 12*102 kJE. 18*102 kJ

A 3.450 g of propane (molar mass = 44.11 g/mol) was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 24.000 degrees celsius and its total heat capacity was 76.65 kJ * C^-1. The reaction raised the temperature of the calorimeter to 28.965 degrees celsius.  a. What is the heat exchangged by the reaction in kilojoules, qrxn?  b. Calculate the deltaE rxn for the combustion of propane in kilojoules per mole c. Work in this reaction is done on the system, done on the surroundings, or equal to zero? Why?