1.10 g of glucose was completely burnt in a copper calorimeter. The temperature of the water

increased from 25.85 °C to 36.50 °C.

Calculate the enthalpy of combustion of glucose from the data below. Assuming the heat released by combustion reaction is absorbed by both water and copper calorimeter.

Mass of water/g 200.00
Specific heat capacity of water: 4.18
Mass of copper/g 120.00
Specific heat capacity of copper/g-1K-1

You didn't write in the heat capacity of the calorimete

q = [mass H2O x specific heat H2O x (delta T)] + [Ccal x (delta T)
q = [200 x 4.18 x (36.50-25.85)] + Ccal x (36.50-25.85)] = ?
That is q for 1.10 g. You don't say but most problems like this want enthalpy of combustion per mol. To convert to kJ/mol do this.
q from above x 180 g/1.10 g = ? in J/mol and usually these are convert to kJ/mol. Finally the heat of combustion is the negative of q. q is the heat absorbed by the calorimeter but the combustion gives off heat so it is negative.

Well, to calculate the enthalpy of combustion of glucose, we need to determine the heat absorbed by both the water and the copper calorimeter.

First, let's calculate the heat absorbed by the water using the formula:

Qwater = mwater * cwater * ΔT

Where:
mwater = mass of water = 200.00 g
cwater = specific heat capacity of water = 4.18 g^-1K^-1
ΔT = change in temperature = (36.50°C - 25.85°C)

Qwater = 200.00 g * 4.18 g^-1K^-1 * (36.50°C - 25.85°C)

Now, let's calculate the heat absorbed by the copper calorimeter using the formula:

Qcopper = mcopper * ccopper * ΔT

Where:
mcopper = mass of copper = 120.00 g
ccopper = specific heat capacity of copper = ccopper/g-1K-1 (you didn't provide the specific value)

Unfortunately, it seems I'm missing the specific heat capacity of copper, and I can't solve the question without it. But let me tell you a joke instead!

Why don't scientists trust atoms?

Because they make up everything!

To calculate the enthalpy of combustion of glucose, we need to first calculate the heat absorbed by the water and copper calorimeter.

1. Calculate the heat absorbed by the water:
Q_water = m_water * c_water * ΔT_water

where:
m_water = mass of water = 200.00 g
c_water = specific heat capacity of water = 4.18 g-1K-1
ΔT_water = change in temperature of water = final temperature - initial temperature = 36.50 °C - 25.85 °C

Q_water = 200.00 g * 4.18 g-1K-1 * (36.50 °C - 25.85 °C)

2. Calculate the heat absorbed by the copper calorimeter:
Q_copper = m_copper * c_copper * ΔT_copper

where:
m_copper = mass of copper = 120.00 g
c_copper = specific heat capacity of copper = to be given

You mention that the specific heat capacity of copper is given as "specific heat capacity of copper/g-1K-1," but the value for the specific heat capacity is missing. Please provide the specific heat capacity of copper.

Once we have the value for the specific heat capacity of copper, we can calculate the heat absorbed by the copper calorimeter:

Q_copper = 120.00 g * (specific heat capacity of copper) * ΔT_copper

3. Calculate the total heat absorbed (Q_total):
Q_total = Q_water + Q_copper

4. Calculate the enthalpy of combustion of glucose:
Enthalpy of combustion of glucose = Q_total / mass of glucose

Please provide the specific heat capacity of copper so that we can complete the calculation.

To calculate the enthalpy of combustion of glucose, we need to use the equation:

Q = m × c × ΔT

where Q is the heat absorbed or released, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, we need to calculate the heat absorbed by both the water and the copper calorimeter.

Heat absorbed by water:
Qw = mw × cw × ΔTw

where mw is the mass of the water, cw is the specific heat capacity of water, and ΔTw is the change in temperature of the water.

Heat absorbed by copper calorimeter:
Qc = mc × cc × ΔTc

where mc is the mass of the copper calorimeter, cc is the specific heat capacity of copper, and ΔTc is the change in temperature of the calorimeter.

First, let's calculate the heat absorbed by the water:
Qw = (200.00 g) × (4.18 g-1K-1) × (36.50 °C - 25.85 °C)

Next, calculate the heat absorbed by the copper calorimeter:
Qc = (120.00 g) × (specific heat capacity of copper) × (36.50 °C - 25.85 °C)

The next step is to calculate the total heat absorbed by both the water and the calorimeter:
Qt = Qw + Qc

Since the heat released by the combustion reaction is absorbed by both the water and the copper calorimeter, the total heat absorbed is equal to the heat released by the reaction.

Next, let's calculate the molar mass of glucose (C6H12O6), which is 180.16 g/mol.

The enthalpy of combustion can be calculated using the equation:

ΔHcomb = Qt / moles of glucose

To find the moles of glucose in the sample, use the equation:

Moles of glucose = mass of glucose / molar mass of glucose

Finally, substitute the values into the equation to obtain the enthalpy of combustion of glucose.