a reaction known to release 1.78 kilojoule of heat takes place in a calorimeter containing 0.100L of soln. the temperature rose by 3.65C. next, a small peice of caco3 was placed in same calorimeter and 0.100L of dilute Hcl was poured over it. the temperature of the calorimeter rose by 3.57 celsius.what is the heat in kilojoules released by the reaction?

Question

a reaction known to release 1.78 kilojoule of heat takes place in a calorimeter containing 0.100L of soln. the temperature rose by 3.65C. next, a small peice of caco3 was placed in same calorimeter and 0.100L of dilute Hcl was poured over it. the temperature of the calorimeter rose by 3.57 celsius.what is the heat in kilojoules released by the reaction?

Answer 1

First, please note that Hcl doesn't mean anything nor does caco3. You MUST learn not to take shortcuts or make typos.

Take a look at this site on the web and see if it describes exactly what the question asks.
http://en.wikipedia.org/wiki/Calorimeter_constant

Answer 2

To find the heat released by the reaction, we can use the equation:

q = mcΔT

where:
q = heat released or absorbed (in joules)
m = mass of the solution (in grams)
c = specific heat capacity of the solution (in J/g·°C)
ΔT = change in temperature (in °C)

Firstly, we need to calculate the mass of the solution (water) in grams.

Density of water = 1 g/mL

So, 0.100 L of water is equal to 0.100 L * 1 g/mL = 0.100 g of water.

Given:
ΔT1 = change in temperature for the reaction = 3.65°C
m1 = mass of water (solution) = 0.100 g

Using q = mcΔT, we can calculate the heat released in the reaction:

q1 = m1 * c * ΔT1

Now, let's calculate q1.

Next, we need to calculate the heat released by the reaction when a small piece of CaCO3 reacts with dilute HCl in the same calorimeter.

Given:
ΔT2 = change in temperature for the reaction = 3.57°C
m2 = mass of water (solution) = 0.100 g

Again, using q = mcΔT, we can calculate the heat released in the reaction:

q2 = m2 * c * ΔT2

Now, let's calculate q2.

Finally, to find the heat released by the reaction, we need to subtract the heat released in the second reaction from the heat released in the first reaction:

q_total = q1 - q2

Now, let's calculate q_total and convert it to kilojoules.

Answer 3

To determine the heat released by the reaction, we can use the equation:

q = mcΔT

Where:
q is the heat released (in joules)
m is the mass of the solution (in grams)
c is the specific heat capacity of the solution (in J/g°C)
ΔT is the change in temperature (in °C)

First, we need to calculate the mass of the solution. We know that the solution has a volume of 0.100 L, but we need the mass in grams. To do this, we need the density of the solution or the molarity of the solution. Since those values are not provided, let's assume the density of the solution is approximately equal to the density of water, which is 1.00 g/mL.

So, the mass of the solution is:
mass = volume × density = 0.100 L × 1.00 g/mL = 0.100 kg

Next, we calculate the heat released by the reaction using the equation above:
q = mcΔT
= (0.100 kg) × c × (3.65 °C)

Now, we need to calculate the specific heat capacity (c) of the solution. Since the specific heat capacity is not given, we assume it to be approximately equal to the specific heat capacity of water, which is 4.18 J/g°C.

Substituting the values:
q = (0.100 kg) × (4.18 J/g°C) × (3.65°C)
= 1.521 J

Finally, we convert the heat from joules to kilojoules:
q = 1.521 J ÷ 1000
= 0.001521 kJ

Therefore, the heat released by the reaction is approximately 0.001521 kilojoules (or 1.521 joules).