1. 3.65g of butane is burned underneath a cup holding 1.00L of water at 21.0°C. The final temperature of the water will be 74.6°C. Show this using proper caculations. (ΔHcomb = -3325 kJ/mol)

When 6.30 g sample of solid potassium hydroxide (MM= 56.11g/mol) is dissolved in 101.00 g of water (at 21.2 degrees Celsius) the temperature of the resulting solution is 38.8 degrees Celsius. What is the AH for this dissolution reaction? Assume the specific heat of the solution is the same as water. Only include the numerical value not units or labels.

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

The burning of 28g of vegetable cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5°C to 28.1 Calculate the amount of heat absorbed by the water using the specific heat of water at 4.18 J/gºC.

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

Octane (C8H18) is a component of gasoline that burns according to the following equation:  C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?

A group of students place 15.41g of a metal into a test tube. They place the test tube into a beaker of boiling water until the temperature of the metal was 89.8°C. Then they quickly place the heated metal into a beaker of 10.47g of water with an initial temperature of 16.4°C. The temperature of the mixturecame to rest at 26.1°C. What is the specific heat of the metal used? (CH2O = 4.18 J/g°C)

When one mole of C6H6 is burned, 3.27 MJ of heat is produced. When the heat from burning 5.27 g of C6H6 is added to 5.69 kg of water at 21.0 ∘C, what is the final temperature of the water?