To begin the experiment, 1.5g of methane ch4 is burned in a bomb calorimeter containing 1,000 grams of water. the initial temperature of water is 25°c. the specific heat of water is 4.184 j/g°c. the heat capacity of the calorimeter is 695 j/°c . after the reaction the final temperature of the water is 37°c. 1. using the formula q =m• c• δt ,calculate the heat absorbed by the water. show work. 2. the total heat absorbed by the water and the calorimeter can be calculated by adding the heat calculated in steps 3 and 4. the amount of heat released by the reaction is equal to the amount of heat absorbed with the negative sign as this is an exothermic reaction. using the formula ∆h = -(qcal + qwater), calculate the total heat of combustion. show work. 3. calculate the experimental molar heat of combustion in kj/mol? show work. 4. given the formula: % error = ((accepted value-experimental value)/accepted value) * 100, calculate the percent error for the experiment. show work

Mass of methane takne = 1.5g

moles of methane used = masss / molar mass = 1.5 / 16 = 0.094 moles

mass of water = 1000 g

Initial temperature of water = 25 C

final temperature = 37 C

specific heat of water = 4.184 J /g C

1) Heat absorbed by water = q =m• C• ΔT = 1000 X 4.184 x (37-25) =  50208 Joules

2) Heat absorbed by calorimeter = Heat capacity X ΔT = 695 X (37-25) = 8340 J

3) Total heat of combustion = heat absorbed by water + calorimeter = 50208 + 8340 = 58548 Joules

This heat is released by 0.094 moles of methane

So heat released by one mole of methane =

                            - 622851.06 Joules = 622.85 kJ / mole

4) standard enthalpy of combustion = -882 kJ / mole

Error = (882-622.85) X 100 / 882 = 24.84 %

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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each chemical family is represented as a group or column on the periodic table. based on chemical properties, there are 6 types of chemical families. group 1 represents alkali metals, group 2 represents alkaline earth metals, groups 3 to 12 represent transition metals, groups 13 to 16 represent non-metals and other metals, group 17 represents halogens and group 18 represents noble gases.